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1,201 | chemistry | acids_bases | strong_acid_ph | 4 | worked_example | pH of strong acid at concentration 0.04867 M | A strong monoprotic acid is fully dissociated. At concentration 0.04867 mol/L, [H⁺] = 0.04867 M and pH = −log₁₀[H⁺] = 1.313. This relation follows directly from the definition of pH and the complete dissociation assumption. | pH = -log10 [H+] | mole_concept; logarithmic functions | Calculate the pH of a strong monoprotic acid solution. |
1,202 | chemistry | acids_bases | strong_acid_ph | 4 | worked_example | pH of strong acid at concentration 0.02166 M | A strong monoprotic acid is fully dissociated. At concentration 0.02166 mol/L, [H⁺] = 0.02166 M and pH = −log₁₀[H⁺] = 1.664. This relation follows directly from the definition of pH and the complete dissociation assumption. | pH = -log10 [H+] | mole_concept; logarithmic functions | Calculate the pH of a strong monoprotic acid solution. |
1,203 | chemistry | acids_bases | strong_acid_ph | 4 | worked_example | pH of strong acid at concentration 1.4989e-04 M | A strong monoprotic acid is fully dissociated. At concentration 1.4989e-04 mol/L, [H⁺] = 1.4989e-04 M and pH = −log₁₀[H⁺] = 3.824. This relation follows directly from the definition of pH and the complete dissociation assumption. | pH = -log10 [H+] | mole_concept; logarithmic functions | Calculate the pH of a strong monoprotic acid solution. |
1,204 | chemistry | acids_bases | strong_acid_ph | 4 | worked_example | pH of strong acid at concentration 0.09432 M | A strong monoprotic acid is fully dissociated. At concentration 0.09432 mol/L, [H⁺] = 0.09432 M and pH = −log₁₀[H⁺] = 1.025. This relation follows directly from the definition of pH and the complete dissociation assumption. | pH = -log10 [H+] | mole_concept; logarithmic functions | Calculate the pH of a strong monoprotic acid solution. |
1,205 | chemistry | acids_bases | strong_acid_ph | 4 | worked_example | pH of strong acid at concentration 0.003875 M | A strong monoprotic acid is fully dissociated. At concentration 0.003875 mol/L, [H⁺] = 0.003875 M and pH = −log₁₀[H⁺] = 2.412. This relation follows directly from the definition of pH and the complete dissociation assumption. | pH = -log10 [H+] | mole_concept; logarithmic functions | Calculate the pH of a strong monoprotic acid solution. |
1,206 | chemistry | equilibrium | equilibrium_constant | 6 | explanation | Meaning of equilibrium constant K = 39.91 | For a reversible reaction at a fixed temperature, the equilibrium constant K is a thermodynamic quantity determined solely by the standard Gibbs free-energy change: K = exp(−ΔG° / R T). In the present illustration K = 39.91. When Q (reaction quotient) < K the forward reaction is spontaneous; when Q > K the reverse reac... | K = exp(-ΔG° / R T); ΔG = ΔG° + R T ln Q | thermodynamics_first_law; mole_concept | Interpret the magnitude of an equilibrium constant and its relation to ΔG°. |
1,207 | chemistry | equilibrium | equilibrium_constant | 6 | explanation | Meaning of equilibrium constant K = 994.6 | For a reversible reaction at a fixed temperature, the equilibrium constant K is a thermodynamic quantity determined solely by the standard Gibbs free-energy change: K = exp(−ΔG° / R T). In the present illustration K = 994.6. When Q (reaction quotient) < K the forward reaction is spontaneous; when Q > K the reverse reac... | K = exp(-ΔG° / R T); ΔG = ΔG° + R T ln Q | thermodynamics_first_law; mole_concept | Interpret the magnitude of an equilibrium constant and its relation to ΔG°. |
1,208 | chemistry | equilibrium | equilibrium_constant | 6 | explanation | Meaning of equilibrium constant K = 698 | For a reversible reaction at a fixed temperature, the equilibrium constant K is a thermodynamic quantity determined solely by the standard Gibbs free-energy change: K = exp(−ΔG° / R T). In the present illustration K = 698. When Q (reaction quotient) < K the forward reaction is spontaneous; when Q > K the reverse reacti... | K = exp(-ΔG° / R T); ΔG = ΔG° + R T ln Q | thermodynamics_first_law; mole_concept | Interpret the magnitude of an equilibrium constant and its relation to ΔG°. |
1,209 | chemistry | equilibrium | equilibrium_constant | 6 | explanation | Meaning of equilibrium constant K = 0.003988 | For a reversible reaction at a fixed temperature, the equilibrium constant K is a thermodynamic quantity determined solely by the standard Gibbs free-energy change: K = exp(−ΔG° / R T). In the present illustration K = 0.003988. When Q (reaction quotient) < K the forward reaction is spontaneous; when Q > K the reverse r... | K = exp(-ΔG° / R T); ΔG = ΔG° + R T ln Q | thermodynamics_first_law; mole_concept | Interpret the magnitude of an equilibrium constant and its relation to ΔG°. |
1,210 | chemistry | equilibrium | equilibrium_constant | 6 | explanation | Meaning of equilibrium constant K = 8.733 | For a reversible reaction at a fixed temperature, the equilibrium constant K is a thermodynamic quantity determined solely by the standard Gibbs free-energy change: K = exp(−ΔG° / R T). In the present illustration K = 8.733. When Q (reaction quotient) < K the forward reaction is spontaneous; when Q > K the reverse reac... | K = exp(-ΔG° / R T); ΔG = ΔG° + R T ln Q | thermodynamics_first_law; mole_concept | Interpret the magnitude of an equilibrium constant and its relation to ΔG°. |
1,211 | chemistry | equilibrium | equilibrium_constant | 6 | explanation | Meaning of equilibrium constant K = 0.03973 | For a reversible reaction at a fixed temperature, the equilibrium constant K is a thermodynamic quantity determined solely by the standard Gibbs free-energy change: K = exp(−ΔG° / R T). In the present illustration K = 0.03973. When Q (reaction quotient) < K the forward reaction is spontaneous; when Q > K the reverse re... | K = exp(-ΔG° / R T); ΔG = ΔG° + R T ln Q | thermodynamics_first_law; mole_concept | Interpret the magnitude of an equilibrium constant and its relation to ΔG°. |
1,212 | chemistry | equilibrium | equilibrium_constant | 6 | explanation | Meaning of equilibrium constant K = 79.02 | For a reversible reaction at a fixed temperature, the equilibrium constant K is a thermodynamic quantity determined solely by the standard Gibbs free-energy change: K = exp(−ΔG° / R T). In the present illustration K = 79.02. When Q (reaction quotient) < K the forward reaction is spontaneous; when Q > K the reverse reac... | K = exp(-ΔG° / R T); ΔG = ΔG° + R T ln Q | thermodynamics_first_law; mole_concept | Interpret the magnitude of an equilibrium constant and its relation to ΔG°. |
1,213 | chemistry | equilibrium | equilibrium_constant | 6 | explanation | Meaning of equilibrium constant K = 318.8 | For a reversible reaction at a fixed temperature, the equilibrium constant K is a thermodynamic quantity determined solely by the standard Gibbs free-energy change: K = exp(−ΔG° / R T). In the present illustration K = 318.8. When Q (reaction quotient) < K the forward reaction is spontaneous; when Q > K the reverse reac... | K = exp(-ΔG° / R T); ΔG = ΔG° + R T ln Q | thermodynamics_first_law; mole_concept | Interpret the magnitude of an equilibrium constant and its relation to ΔG°. |
1,214 | chemistry | equilibrium | equilibrium_constant | 6 | explanation | Meaning of equilibrium constant K = 0.002165 | For a reversible reaction at a fixed temperature, the equilibrium constant K is a thermodynamic quantity determined solely by the standard Gibbs free-energy change: K = exp(−ΔG° / R T). In the present illustration K = 0.002165. When Q (reaction quotient) < K the forward reaction is spontaneous; when Q > K the reverse r... | K = exp(-ΔG° / R T); ΔG = ΔG° + R T ln Q | thermodynamics_first_law; mole_concept | Interpret the magnitude of an equilibrium constant and its relation to ΔG°. |
1,215 | chemistry | equilibrium | equilibrium_constant | 6 | explanation | Meaning of equilibrium constant K = 951.4 | For a reversible reaction at a fixed temperature, the equilibrium constant K is a thermodynamic quantity determined solely by the standard Gibbs free-energy change: K = exp(−ΔG° / R T). In the present illustration K = 951.4. When Q (reaction quotient) < K the forward reaction is spontaneous; when Q > K the reverse reac... | K = exp(-ΔG° / R T); ΔG = ΔG° + R T ln Q | thermodynamics_first_law; mole_concept | Interpret the magnitude of an equilibrium constant and its relation to ΔG°. |
1,216 | chemistry | equilibrium | equilibrium_constant | 6 | explanation | Meaning of equilibrium constant K = 0.02072 | For a reversible reaction at a fixed temperature, the equilibrium constant K is a thermodynamic quantity determined solely by the standard Gibbs free-energy change: K = exp(−ΔG° / R T). In the present illustration K = 0.02072. When Q (reaction quotient) < K the forward reaction is spontaneous; when Q > K the reverse re... | K = exp(-ΔG° / R T); ΔG = ΔG° + R T ln Q | thermodynamics_first_law; mole_concept | Interpret the magnitude of an equilibrium constant and its relation to ΔG°. |
1,217 | chemistry | equilibrium | equilibrium_constant | 6 | explanation | Meaning of equilibrium constant K = 120 | For a reversible reaction at a fixed temperature, the equilibrium constant K is a thermodynamic quantity determined solely by the standard Gibbs free-energy change: K = exp(−ΔG° / R T). In the present illustration K = 120. When Q (reaction quotient) < K the forward reaction is spontaneous; when Q > K the reverse reacti... | K = exp(-ΔG° / R T); ΔG = ΔG° + R T ln Q | thermodynamics_first_law; mole_concept | Interpret the magnitude of an equilibrium constant and its relation to ΔG°. |
1,218 | chemistry | equilibrium | equilibrium_constant | 6 | explanation | Meaning of equilibrium constant K = 60.86 | For a reversible reaction at a fixed temperature, the equilibrium constant K is a thermodynamic quantity determined solely by the standard Gibbs free-energy change: K = exp(−ΔG° / R T). In the present illustration K = 60.86. When Q (reaction quotient) < K the forward reaction is spontaneous; when Q > K the reverse reac... | K = exp(-ΔG° / R T); ΔG = ΔG° + R T ln Q | thermodynamics_first_law; mole_concept | Interpret the magnitude of an equilibrium constant and its relation to ΔG°. |
1,219 | chemistry | equilibrium | equilibrium_constant | 6 | explanation | Meaning of equilibrium constant K = 0.1345 | For a reversible reaction at a fixed temperature, the equilibrium constant K is a thermodynamic quantity determined solely by the standard Gibbs free-energy change: K = exp(−ΔG° / R T). In the present illustration K = 0.1345. When Q (reaction quotient) < K the forward reaction is spontaneous; when Q > K the reverse rea... | K = exp(-ΔG° / R T); ΔG = ΔG° + R T ln Q | thermodynamics_first_law; mole_concept | Interpret the magnitude of an equilibrium constant and its relation to ΔG°. |
1,220 | chemistry | equilibrium | equilibrium_constant | 6 | explanation | Meaning of equilibrium constant K = 108.5 | For a reversible reaction at a fixed temperature, the equilibrium constant K is a thermodynamic quantity determined solely by the standard Gibbs free-energy change: K = exp(−ΔG° / R T). In the present illustration K = 108.5. When Q (reaction quotient) < K the forward reaction is spontaneous; when Q > K the reverse reac... | K = exp(-ΔG° / R T); ΔG = ΔG° + R T ln Q | thermodynamics_first_law; mole_concept | Interpret the magnitude of an equilibrium constant and its relation to ΔG°. |
1,221 | chemistry | equilibrium | equilibrium_constant | 6 | explanation | Meaning of equilibrium constant K = 117.8 | For a reversible reaction at a fixed temperature, the equilibrium constant K is a thermodynamic quantity determined solely by the standard Gibbs free-energy change: K = exp(−ΔG° / R T). In the present illustration K = 117.8. When Q (reaction quotient) < K the forward reaction is spontaneous; when Q > K the reverse reac... | K = exp(-ΔG° / R T); ΔG = ΔG° + R T ln Q | thermodynamics_first_law; mole_concept | Interpret the magnitude of an equilibrium constant and its relation to ΔG°. |
1,222 | chemistry | equilibrium | equilibrium_constant | 6 | explanation | Meaning of equilibrium constant K = 0.01139 | For a reversible reaction at a fixed temperature, the equilibrium constant K is a thermodynamic quantity determined solely by the standard Gibbs free-energy change: K = exp(−ΔG° / R T). In the present illustration K = 0.01139. When Q (reaction quotient) < K the forward reaction is spontaneous; when Q > K the reverse re... | K = exp(-ΔG° / R T); ΔG = ΔG° + R T ln Q | thermodynamics_first_law; mole_concept | Interpret the magnitude of an equilibrium constant and its relation to ΔG°. |
1,223 | chemistry | equilibrium | equilibrium_constant | 6 | explanation | Meaning of equilibrium constant K = 3.59 | For a reversible reaction at a fixed temperature, the equilibrium constant K is a thermodynamic quantity determined solely by the standard Gibbs free-energy change: K = exp(−ΔG° / R T). In the present illustration K = 3.59. When Q (reaction quotient) < K the forward reaction is spontaneous; when Q > K the reverse react... | K = exp(-ΔG° / R T); ΔG = ΔG° + R T ln Q | thermodynamics_first_law; mole_concept | Interpret the magnitude of an equilibrium constant and its relation to ΔG°. |
1,224 | chemistry | equilibrium | equilibrium_constant | 6 | explanation | Meaning of equilibrium constant K = 68.75 | For a reversible reaction at a fixed temperature, the equilibrium constant K is a thermodynamic quantity determined solely by the standard Gibbs free-energy change: K = exp(−ΔG° / R T). In the present illustration K = 68.75. When Q (reaction quotient) < K the forward reaction is spontaneous; when Q > K the reverse reac... | K = exp(-ΔG° / R T); ΔG = ΔG° + R T ln Q | thermodynamics_first_law; mole_concept | Interpret the magnitude of an equilibrium constant and its relation to ΔG°. |
1,225 | chemistry | equilibrium | equilibrium_constant | 6 | explanation | Meaning of equilibrium constant K = 15.34 | For a reversible reaction at a fixed temperature, the equilibrium constant K is a thermodynamic quantity determined solely by the standard Gibbs free-energy change: K = exp(−ΔG° / R T). In the present illustration K = 15.34. When Q (reaction quotient) < K the forward reaction is spontaneous; when Q > K the reverse reac... | K = exp(-ΔG° / R T); ΔG = ΔG° + R T ln Q | thermodynamics_first_law; mole_concept | Interpret the magnitude of an equilibrium constant and its relation to ΔG°. |
1,226 | chemistry | equilibrium | equilibrium_constant | 6 | explanation | Meaning of equilibrium constant K = 304.7 | For a reversible reaction at a fixed temperature, the equilibrium constant K is a thermodynamic quantity determined solely by the standard Gibbs free-energy change: K = exp(−ΔG° / R T). In the present illustration K = 304.7. When Q (reaction quotient) < K the forward reaction is spontaneous; when Q > K the reverse reac... | K = exp(-ΔG° / R T); ΔG = ΔG° + R T ln Q | thermodynamics_first_law; mole_concept | Interpret the magnitude of an equilibrium constant and its relation to ΔG°. |
1,227 | chemistry | equilibrium | equilibrium_constant | 6 | explanation | Meaning of equilibrium constant K = 0.001477 | For a reversible reaction at a fixed temperature, the equilibrium constant K is a thermodynamic quantity determined solely by the standard Gibbs free-energy change: K = exp(−ΔG° / R T). In the present illustration K = 0.001477. When Q (reaction quotient) < K the forward reaction is spontaneous; when Q > K the reverse r... | K = exp(-ΔG° / R T); ΔG = ΔG° + R T ln Q | thermodynamics_first_law; mole_concept | Interpret the magnitude of an equilibrium constant and its relation to ΔG°. |
1,228 | chemistry | equilibrium | equilibrium_constant | 6 | explanation | Meaning of equilibrium constant K = 15.97 | For a reversible reaction at a fixed temperature, the equilibrium constant K is a thermodynamic quantity determined solely by the standard Gibbs free-energy change: K = exp(−ΔG° / R T). In the present illustration K = 15.97. When Q (reaction quotient) < K the forward reaction is spontaneous; when Q > K the reverse reac... | K = exp(-ΔG° / R T); ΔG = ΔG° + R T ln Q | thermodynamics_first_law; mole_concept | Interpret the magnitude of an equilibrium constant and its relation to ΔG°. |
1,229 | chemistry | equilibrium | equilibrium_constant | 6 | explanation | Meaning of equilibrium constant K = 484.6 | For a reversible reaction at a fixed temperature, the equilibrium constant K is a thermodynamic quantity determined solely by the standard Gibbs free-energy change: K = exp(−ΔG° / R T). In the present illustration K = 484.6. When Q (reaction quotient) < K the forward reaction is spontaneous; when Q > K the reverse reac... | K = exp(-ΔG° / R T); ΔG = ΔG° + R T ln Q | thermodynamics_first_law; mole_concept | Interpret the magnitude of an equilibrium constant and its relation to ΔG°. |
1,230 | chemistry | equilibrium | equilibrium_constant | 6 | explanation | Meaning of equilibrium constant K = 2.408 | For a reversible reaction at a fixed temperature, the equilibrium constant K is a thermodynamic quantity determined solely by the standard Gibbs free-energy change: K = exp(−ΔG° / R T). In the present illustration K = 2.408. When Q (reaction quotient) < K the forward reaction is spontaneous; when Q > K the reverse reac... | K = exp(-ΔG° / R T); ΔG = ΔG° + R T ln Q | thermodynamics_first_law; mole_concept | Interpret the magnitude of an equilibrium constant and its relation to ΔG°. |
1,231 | chemistry | equilibrium | equilibrium_constant | 6 | explanation | Meaning of equilibrium constant K = 2.391 | For a reversible reaction at a fixed temperature, the equilibrium constant K is a thermodynamic quantity determined solely by the standard Gibbs free-energy change: K = exp(−ΔG° / R T). In the present illustration K = 2.391. When Q (reaction quotient) < K the forward reaction is spontaneous; when Q > K the reverse reac... | K = exp(-ΔG° / R T); ΔG = ΔG° + R T ln Q | thermodynamics_first_law; mole_concept | Interpret the magnitude of an equilibrium constant and its relation to ΔG°. |
1,232 | chemistry | equilibrium | equilibrium_constant | 6 | explanation | Meaning of equilibrium constant K = 0.01347 | For a reversible reaction at a fixed temperature, the equilibrium constant K is a thermodynamic quantity determined solely by the standard Gibbs free-energy change: K = exp(−ΔG° / R T). In the present illustration K = 0.01347. When Q (reaction quotient) < K the forward reaction is spontaneous; when Q > K the reverse re... | K = exp(-ΔG° / R T); ΔG = ΔG° + R T ln Q | thermodynamics_first_law; mole_concept | Interpret the magnitude of an equilibrium constant and its relation to ΔG°. |
1,233 | chemistry | equilibrium | equilibrium_constant | 6 | explanation | Meaning of equilibrium constant K = 847.3 | For a reversible reaction at a fixed temperature, the equilibrium constant K is a thermodynamic quantity determined solely by the standard Gibbs free-energy change: K = exp(−ΔG° / R T). In the present illustration K = 847.3. When Q (reaction quotient) < K the forward reaction is spontaneous; when Q > K the reverse reac... | K = exp(-ΔG° / R T); ΔG = ΔG° + R T ln Q | thermodynamics_first_law; mole_concept | Interpret the magnitude of an equilibrium constant and its relation to ΔG°. |
1,234 | chemistry | equilibrium | equilibrium_constant | 6 | explanation | Meaning of equilibrium constant K = 194.9 | For a reversible reaction at a fixed temperature, the equilibrium constant K is a thermodynamic quantity determined solely by the standard Gibbs free-energy change: K = exp(−ΔG° / R T). In the present illustration K = 194.9. When Q (reaction quotient) < K the forward reaction is spontaneous; when Q > K the reverse reac... | K = exp(-ΔG° / R T); ΔG = ΔG° + R T ln Q | thermodynamics_first_law; mole_concept | Interpret the magnitude of an equilibrium constant and its relation to ΔG°. |
1,235 | chemistry | equilibrium | equilibrium_constant | 6 | explanation | Meaning of equilibrium constant K = 0.8982 | For a reversible reaction at a fixed temperature, the equilibrium constant K is a thermodynamic quantity determined solely by the standard Gibbs free-energy change: K = exp(−ΔG° / R T). In the present illustration K = 0.8982. When Q (reaction quotient) < K the forward reaction is spontaneous; when Q > K the reverse rea... | K = exp(-ΔG° / R T); ΔG = ΔG° + R T ln Q | thermodynamics_first_law; mole_concept | Interpret the magnitude of an equilibrium constant and its relation to ΔG°. |
1,236 | chemistry | equilibrium | equilibrium_constant | 6 | explanation | Meaning of equilibrium constant K = 0.0715 | For a reversible reaction at a fixed temperature, the equilibrium constant K is a thermodynamic quantity determined solely by the standard Gibbs free-energy change: K = exp(−ΔG° / R T). In the present illustration K = 0.0715. When Q (reaction quotient) < K the forward reaction is spontaneous; when Q > K the reverse rea... | K = exp(-ΔG° / R T); ΔG = ΔG° + R T ln Q | thermodynamics_first_law; mole_concept | Interpret the magnitude of an equilibrium constant and its relation to ΔG°. |
1,237 | chemistry | equilibrium | equilibrium_constant | 6 | explanation | Meaning of equilibrium constant K = 0.8762 | For a reversible reaction at a fixed temperature, the equilibrium constant K is a thermodynamic quantity determined solely by the standard Gibbs free-energy change: K = exp(−ΔG° / R T). In the present illustration K = 0.8762. When Q (reaction quotient) < K the forward reaction is spontaneous; when Q > K the reverse rea... | K = exp(-ΔG° / R T); ΔG = ΔG° + R T ln Q | thermodynamics_first_law; mole_concept | Interpret the magnitude of an equilibrium constant and its relation to ΔG°. |
1,238 | chemistry | equilibrium | equilibrium_constant | 6 | explanation | Meaning of equilibrium constant K = 0.00348 | For a reversible reaction at a fixed temperature, the equilibrium constant K is a thermodynamic quantity determined solely by the standard Gibbs free-energy change: K = exp(−ΔG° / R T). In the present illustration K = 0.00348. When Q (reaction quotient) < K the forward reaction is spontaneous; when Q > K the reverse re... | K = exp(-ΔG° / R T); ΔG = ΔG° + R T ln Q | thermodynamics_first_law; mole_concept | Interpret the magnitude of an equilibrium constant and its relation to ΔG°. |
1,239 | chemistry | equilibrium | equilibrium_constant | 6 | explanation | Meaning of equilibrium constant K = 0.02487 | For a reversible reaction at a fixed temperature, the equilibrium constant K is a thermodynamic quantity determined solely by the standard Gibbs free-energy change: K = exp(−ΔG° / R T). In the present illustration K = 0.02487. When Q (reaction quotient) < K the forward reaction is spontaneous; when Q > K the reverse re... | K = exp(-ΔG° / R T); ΔG = ΔG° + R T ln Q | thermodynamics_first_law; mole_concept | Interpret the magnitude of an equilibrium constant and its relation to ΔG°. |
1,240 | chemistry | equilibrium | equilibrium_constant | 6 | explanation | Meaning of equilibrium constant K = 0.02055 | For a reversible reaction at a fixed temperature, the equilibrium constant K is a thermodynamic quantity determined solely by the standard Gibbs free-energy change: K = exp(−ΔG° / R T). In the present illustration K = 0.02055. When Q (reaction quotient) < K the forward reaction is spontaneous; when Q > K the reverse re... | K = exp(-ΔG° / R T); ΔG = ΔG° + R T ln Q | thermodynamics_first_law; mole_concept | Interpret the magnitude of an equilibrium constant and its relation to ΔG°. |
1,241 | chemistry | equilibrium | equilibrium_constant | 6 | explanation | Meaning of equilibrium constant K = 1.441 | For a reversible reaction at a fixed temperature, the equilibrium constant K is a thermodynamic quantity determined solely by the standard Gibbs free-energy change: K = exp(−ΔG° / R T). In the present illustration K = 1.441. When Q (reaction quotient) < K the forward reaction is spontaneous; when Q > K the reverse reac... | K = exp(-ΔG° / R T); ΔG = ΔG° + R T ln Q | thermodynamics_first_law; mole_concept | Interpret the magnitude of an equilibrium constant and its relation to ΔG°. |
1,242 | chemistry | equilibrium | equilibrium_constant | 6 | explanation | Meaning of equilibrium constant K = 0.001009 | For a reversible reaction at a fixed temperature, the equilibrium constant K is a thermodynamic quantity determined solely by the standard Gibbs free-energy change: K = exp(−ΔG° / R T). In the present illustration K = 0.001009. When Q (reaction quotient) < K the forward reaction is spontaneous; when Q > K the reverse r... | K = exp(-ΔG° / R T); ΔG = ΔG° + R T ln Q | thermodynamics_first_law; mole_concept | Interpret the magnitude of an equilibrium constant and its relation to ΔG°. |
1,243 | chemistry | equilibrium | equilibrium_constant | 6 | explanation | Meaning of equilibrium constant K = 321.6 | For a reversible reaction at a fixed temperature, the equilibrium constant K is a thermodynamic quantity determined solely by the standard Gibbs free-energy change: K = exp(−ΔG° / R T). In the present illustration K = 321.6. When Q (reaction quotient) < K the forward reaction is spontaneous; when Q > K the reverse reac... | K = exp(-ΔG° / R T); ΔG = ΔG° + R T ln Q | thermodynamics_first_law; mole_concept | Interpret the magnitude of an equilibrium constant and its relation to ΔG°. |
1,244 | chemistry | equilibrium | equilibrium_constant | 6 | explanation | Meaning of equilibrium constant K = 0.01617 | For a reversible reaction at a fixed temperature, the equilibrium constant K is a thermodynamic quantity determined solely by the standard Gibbs free-energy change: K = exp(−ΔG° / R T). In the present illustration K = 0.01617. When Q (reaction quotient) < K the forward reaction is spontaneous; when Q > K the reverse re... | K = exp(-ΔG° / R T); ΔG = ΔG° + R T ln Q | thermodynamics_first_law; mole_concept | Interpret the magnitude of an equilibrium constant and its relation to ΔG°. |
1,245 | chemistry | equilibrium | equilibrium_constant | 6 | explanation | Meaning of equilibrium constant K = 0.006066 | For a reversible reaction at a fixed temperature, the equilibrium constant K is a thermodynamic quantity determined solely by the standard Gibbs free-energy change: K = exp(−ΔG° / R T). In the present illustration K = 0.006066. When Q (reaction quotient) < K the forward reaction is spontaneous; when Q > K the reverse r... | K = exp(-ΔG° / R T); ΔG = ΔG° + R T ln Q | thermodynamics_first_law; mole_concept | Interpret the magnitude of an equilibrium constant and its relation to ΔG°. |
1,246 | chemistry | equilibrium | equilibrium_constant | 6 | explanation | Meaning of equilibrium constant K = 20.03 | For a reversible reaction at a fixed temperature, the equilibrium constant K is a thermodynamic quantity determined solely by the standard Gibbs free-energy change: K = exp(−ΔG° / R T). In the present illustration K = 20.03. When Q (reaction quotient) < K the forward reaction is spontaneous; when Q > K the reverse reac... | K = exp(-ΔG° / R T); ΔG = ΔG° + R T ln Q | thermodynamics_first_law; mole_concept | Interpret the magnitude of an equilibrium constant and its relation to ΔG°. |
1,247 | chemistry | equilibrium | equilibrium_constant | 6 | explanation | Meaning of equilibrium constant K = 325.6 | For a reversible reaction at a fixed temperature, the equilibrium constant K is a thermodynamic quantity determined solely by the standard Gibbs free-energy change: K = exp(−ΔG° / R T). In the present illustration K = 325.6. When Q (reaction quotient) < K the forward reaction is spontaneous; when Q > K the reverse reac... | K = exp(-ΔG° / R T); ΔG = ΔG° + R T ln Q | thermodynamics_first_law; mole_concept | Interpret the magnitude of an equilibrium constant and its relation to ΔG°. |
1,248 | chemistry | equilibrium | equilibrium_constant | 6 | explanation | Meaning of equilibrium constant K = 116.3 | For a reversible reaction at a fixed temperature, the equilibrium constant K is a thermodynamic quantity determined solely by the standard Gibbs free-energy change: K = exp(−ΔG° / R T). In the present illustration K = 116.3. When Q (reaction quotient) < K the forward reaction is spontaneous; when Q > K the reverse reac... | K = exp(-ΔG° / R T); ΔG = ΔG° + R T ln Q | thermodynamics_first_law; mole_concept | Interpret the magnitude of an equilibrium constant and its relation to ΔG°. |
1,249 | chemistry | equilibrium | equilibrium_constant | 6 | explanation | Meaning of equilibrium constant K = 0.0874 | For a reversible reaction at a fixed temperature, the equilibrium constant K is a thermodynamic quantity determined solely by the standard Gibbs free-energy change: K = exp(−ΔG° / R T). In the present illustration K = 0.0874. When Q (reaction quotient) < K the forward reaction is spontaneous; when Q > K the reverse rea... | K = exp(-ΔG° / R T); ΔG = ΔG° + R T ln Q | thermodynamics_first_law; mole_concept | Interpret the magnitude of an equilibrium constant and its relation to ΔG°. |
1,250 | chemistry | equilibrium | equilibrium_constant | 6 | explanation | Meaning of equilibrium constant K = 0.001354 | For a reversible reaction at a fixed temperature, the equilibrium constant K is a thermodynamic quantity determined solely by the standard Gibbs free-energy change: K = exp(−ΔG° / R T). In the present illustration K = 0.001354. When Q (reaction quotient) < K the forward reaction is spontaneous; when Q > K the reverse r... | K = exp(-ΔG° / R T); ΔG = ΔG° + R T ln Q | thermodynamics_first_law; mole_concept | Interpret the magnitude of an equilibrium constant and its relation to ΔG°. |
1,251 | chemistry | equilibrium | equilibrium_constant | 6 | explanation | Meaning of equilibrium constant K = 3.309 | For a reversible reaction at a fixed temperature, the equilibrium constant K is a thermodynamic quantity determined solely by the standard Gibbs free-energy change: K = exp(−ΔG° / R T). In the present illustration K = 3.309. When Q (reaction quotient) < K the forward reaction is spontaneous; when Q > K the reverse reac... | K = exp(-ΔG° / R T); ΔG = ΔG° + R T ln Q | thermodynamics_first_law; mole_concept | Interpret the magnitude of an equilibrium constant and its relation to ΔG°. |
1,252 | chemistry | equilibrium | equilibrium_constant | 6 | explanation | Meaning of equilibrium constant K = 318.7 | For a reversible reaction at a fixed temperature, the equilibrium constant K is a thermodynamic quantity determined solely by the standard Gibbs free-energy change: K = exp(−ΔG° / R T). In the present illustration K = 318.7. When Q (reaction quotient) < K the forward reaction is spontaneous; when Q > K the reverse reac... | K = exp(-ΔG° / R T); ΔG = ΔG° + R T ln Q | thermodynamics_first_law; mole_concept | Interpret the magnitude of an equilibrium constant and its relation to ΔG°. |
1,253 | chemistry | equilibrium | equilibrium_constant | 6 | explanation | Meaning of equilibrium constant K = 44.28 | For a reversible reaction at a fixed temperature, the equilibrium constant K is a thermodynamic quantity determined solely by the standard Gibbs free-energy change: K = exp(−ΔG° / R T). In the present illustration K = 44.28. When Q (reaction quotient) < K the forward reaction is spontaneous; when Q > K the reverse reac... | K = exp(-ΔG° / R T); ΔG = ΔG° + R T ln Q | thermodynamics_first_law; mole_concept | Interpret the magnitude of an equilibrium constant and its relation to ΔG°. |
1,254 | chemistry | equilibrium | equilibrium_constant | 6 | explanation | Meaning of equilibrium constant K = 119.9 | For a reversible reaction at a fixed temperature, the equilibrium constant K is a thermodynamic quantity determined solely by the standard Gibbs free-energy change: K = exp(−ΔG° / R T). In the present illustration K = 119.9. When Q (reaction quotient) < K the forward reaction is spontaneous; when Q > K the reverse reac... | K = exp(-ΔG° / R T); ΔG = ΔG° + R T ln Q | thermodynamics_first_law; mole_concept | Interpret the magnitude of an equilibrium constant and its relation to ΔG°. |
1,255 | chemistry | equilibrium | equilibrium_constant | 6 | explanation | Meaning of equilibrium constant K = 145.9 | For a reversible reaction at a fixed temperature, the equilibrium constant K is a thermodynamic quantity determined solely by the standard Gibbs free-energy change: K = exp(−ΔG° / R T). In the present illustration K = 145.9. When Q (reaction quotient) < K the forward reaction is spontaneous; when Q > K the reverse reac... | K = exp(-ΔG° / R T); ΔG = ΔG° + R T ln Q | thermodynamics_first_law; mole_concept | Interpret the magnitude of an equilibrium constant and its relation to ΔG°. |
1,256 | chemistry | equilibrium | equilibrium_constant | 6 | explanation | Meaning of equilibrium constant K = 579.9 | For a reversible reaction at a fixed temperature, the equilibrium constant K is a thermodynamic quantity determined solely by the standard Gibbs free-energy change: K = exp(−ΔG° / R T). In the present illustration K = 579.9. When Q (reaction quotient) < K the forward reaction is spontaneous; when Q > K the reverse reac... | K = exp(-ΔG° / R T); ΔG = ΔG° + R T ln Q | thermodynamics_first_law; mole_concept | Interpret the magnitude of an equilibrium constant and its relation to ΔG°. |
1,257 | chemistry | equilibrium | equilibrium_constant | 6 | explanation | Meaning of equilibrium constant K = 0.1744 | For a reversible reaction at a fixed temperature, the equilibrium constant K is a thermodynamic quantity determined solely by the standard Gibbs free-energy change: K = exp(−ΔG° / R T). In the present illustration K = 0.1744. When Q (reaction quotient) < K the forward reaction is spontaneous; when Q > K the reverse rea... | K = exp(-ΔG° / R T); ΔG = ΔG° + R T ln Q | thermodynamics_first_law; mole_concept | Interpret the magnitude of an equilibrium constant and its relation to ΔG°. |
1,258 | chemistry | equilibrium | equilibrium_constant | 6 | explanation | Meaning of equilibrium constant K = 448.3 | For a reversible reaction at a fixed temperature, the equilibrium constant K is a thermodynamic quantity determined solely by the standard Gibbs free-energy change: K = exp(−ΔG° / R T). In the present illustration K = 448.3. When Q (reaction quotient) < K the forward reaction is spontaneous; when Q > K the reverse reac... | K = exp(-ΔG° / R T); ΔG = ΔG° + R T ln Q | thermodynamics_first_law; mole_concept | Interpret the magnitude of an equilibrium constant and its relation to ΔG°. |
1,259 | chemistry | equilibrium | equilibrium_constant | 6 | explanation | Meaning of equilibrium constant K = 0.2364 | For a reversible reaction at a fixed temperature, the equilibrium constant K is a thermodynamic quantity determined solely by the standard Gibbs free-energy change: K = exp(−ΔG° / R T). In the present illustration K = 0.2364. When Q (reaction quotient) < K the forward reaction is spontaneous; when Q > K the reverse rea... | K = exp(-ΔG° / R T); ΔG = ΔG° + R T ln Q | thermodynamics_first_law; mole_concept | Interpret the magnitude of an equilibrium constant and its relation to ΔG°. |
1,260 | chemistry | equilibrium | equilibrium_constant | 6 | explanation | Meaning of equilibrium constant K = 0.004038 | For a reversible reaction at a fixed temperature, the equilibrium constant K is a thermodynamic quantity determined solely by the standard Gibbs free-energy change: K = exp(−ΔG° / R T). In the present illustration K = 0.004038. When Q (reaction quotient) < K the forward reaction is spontaneous; when Q > K the reverse r... | K = exp(-ΔG° / R T); ΔG = ΔG° + R T ln Q | thermodynamics_first_law; mole_concept | Interpret the magnitude of an equilibrium constant and its relation to ΔG°. |
1,261 | chemistry | equilibrium | equilibrium_constant | 6 | explanation | Meaning of equilibrium constant K = 0.06465 | For a reversible reaction at a fixed temperature, the equilibrium constant K is a thermodynamic quantity determined solely by the standard Gibbs free-energy change: K = exp(−ΔG° / R T). In the present illustration K = 0.06465. When Q (reaction quotient) < K the forward reaction is spontaneous; when Q > K the reverse re... | K = exp(-ΔG° / R T); ΔG = ΔG° + R T ln Q | thermodynamics_first_law; mole_concept | Interpret the magnitude of an equilibrium constant and its relation to ΔG°. |
1,262 | chemistry | equilibrium | equilibrium_constant | 6 | explanation | Meaning of equilibrium constant K = 0.006587 | For a reversible reaction at a fixed temperature, the equilibrium constant K is a thermodynamic quantity determined solely by the standard Gibbs free-energy change: K = exp(−ΔG° / R T). In the present illustration K = 0.006587. When Q (reaction quotient) < K the forward reaction is spontaneous; when Q > K the reverse r... | K = exp(-ΔG° / R T); ΔG = ΔG° + R T ln Q | thermodynamics_first_law; mole_concept | Interpret the magnitude of an equilibrium constant and its relation to ΔG°. |
1,263 | chemistry | equilibrium | equilibrium_constant | 6 | explanation | Meaning of equilibrium constant K = 0.008811 | For a reversible reaction at a fixed temperature, the equilibrium constant K is a thermodynamic quantity determined solely by the standard Gibbs free-energy change: K = exp(−ΔG° / R T). In the present illustration K = 0.008811. When Q (reaction quotient) < K the forward reaction is spontaneous; when Q > K the reverse r... | K = exp(-ΔG° / R T); ΔG = ΔG° + R T ln Q | thermodynamics_first_law; mole_concept | Interpret the magnitude of an equilibrium constant and its relation to ΔG°. |
1,264 | chemistry | equilibrium | equilibrium_constant | 6 | explanation | Meaning of equilibrium constant K = 492.2 | For a reversible reaction at a fixed temperature, the equilibrium constant K is a thermodynamic quantity determined solely by the standard Gibbs free-energy change: K = exp(−ΔG° / R T). In the present illustration K = 492.2. When Q (reaction quotient) < K the forward reaction is spontaneous; when Q > K the reverse reac... | K = exp(-ΔG° / R T); ΔG = ΔG° + R T ln Q | thermodynamics_first_law; mole_concept | Interpret the magnitude of an equilibrium constant and its relation to ΔG°. |
1,265 | chemistry | equilibrium | equilibrium_constant | 6 | explanation | Meaning of equilibrium constant K = 56.37 | For a reversible reaction at a fixed temperature, the equilibrium constant K is a thermodynamic quantity determined solely by the standard Gibbs free-energy change: K = exp(−ΔG° / R T). In the present illustration K = 56.37. When Q (reaction quotient) < K the forward reaction is spontaneous; when Q > K the reverse reac... | K = exp(-ΔG° / R T); ΔG = ΔG° + R T ln Q | thermodynamics_first_law; mole_concept | Interpret the magnitude of an equilibrium constant and its relation to ΔG°. |
1,266 | chemistry | thermochemistry | hess_law | 5 | explanation | Hess's law and enthalpy as a state function | Enthalpy H is a state function: its change between two states is independent of path. Consequently, the enthalpy change of a reaction may be computed by summing the enthalpy changes of any convenient sequence of reactions that net to the same overall transformation (Hess's law). Standard enthalpies of formation provide... | ΔH°_rxn = Σ ΔH°_f(products) - Σ ΔH°_f(reactants) | first_law | Apply Hess's law to compute reaction enthalpies from tabulated formation data. |
1,267 | chemistry | thermochemistry | hess_law | 5 | explanation | Hess's law and enthalpy as a state function | Enthalpy H is a state function: its change between two states is independent of path. Consequently, the enthalpy change of a reaction may be computed by summing the enthalpy changes of any convenient sequence of reactions that net to the same overall transformation (Hess's law). Standard enthalpies of formation provide... | ΔH°_rxn = Σ ΔH°_f(products) - Σ ΔH°_f(reactants) | first_law | Apply Hess's law to compute reaction enthalpies from tabulated formation data. |
1,268 | chemistry | thermochemistry | hess_law | 5 | explanation | Hess's law and enthalpy as a state function | Enthalpy H is a state function: its change between two states is independent of path. Consequently, the enthalpy change of a reaction may be computed by summing the enthalpy changes of any convenient sequence of reactions that net to the same overall transformation (Hess's law). Standard enthalpies of formation provide... | ΔH°_rxn = Σ ΔH°_f(products) - Σ ΔH°_f(reactants) | first_law | Apply Hess's law to compute reaction enthalpies from tabulated formation data. |
1,269 | chemistry | thermochemistry | hess_law | 5 | explanation | Hess's law and enthalpy as a state function | Enthalpy H is a state function: its change between two states is independent of path. Consequently, the enthalpy change of a reaction may be computed by summing the enthalpy changes of any convenient sequence of reactions that net to the same overall transformation (Hess's law). Standard enthalpies of formation provide... | ΔH°_rxn = Σ ΔH°_f(products) - Σ ΔH°_f(reactants) | first_law | Apply Hess's law to compute reaction enthalpies from tabulated formation data. |
1,270 | chemistry | thermochemistry | hess_law | 5 | explanation | Hess's law and enthalpy as a state function | Enthalpy H is a state function: its change between two states is independent of path. Consequently, the enthalpy change of a reaction may be computed by summing the enthalpy changes of any convenient sequence of reactions that net to the same overall transformation (Hess's law). Standard enthalpies of formation provide... | ΔH°_rxn = Σ ΔH°_f(products) - Σ ΔH°_f(reactants) | first_law | Apply Hess's law to compute reaction enthalpies from tabulated formation data. |
1,271 | chemistry | thermochemistry | hess_law | 5 | explanation | Hess's law and enthalpy as a state function | Enthalpy H is a state function: its change between two states is independent of path. Consequently, the enthalpy change of a reaction may be computed by summing the enthalpy changes of any convenient sequence of reactions that net to the same overall transformation (Hess's law). Standard enthalpies of formation provide... | ΔH°_rxn = Σ ΔH°_f(products) - Σ ΔH°_f(reactants) | first_law | Apply Hess's law to compute reaction enthalpies from tabulated formation data. |
1,272 | chemistry | thermochemistry | hess_law | 5 | explanation | Hess's law and enthalpy as a state function | Enthalpy H is a state function: its change between two states is independent of path. Consequently, the enthalpy change of a reaction may be computed by summing the enthalpy changes of any convenient sequence of reactions that net to the same overall transformation (Hess's law). Standard enthalpies of formation provide... | ΔH°_rxn = Σ ΔH°_f(products) - Σ ΔH°_f(reactants) | first_law | Apply Hess's law to compute reaction enthalpies from tabulated formation data. |
1,273 | chemistry | thermochemistry | hess_law | 5 | explanation | Hess's law and enthalpy as a state function | Enthalpy H is a state function: its change between two states is independent of path. Consequently, the enthalpy change of a reaction may be computed by summing the enthalpy changes of any convenient sequence of reactions that net to the same overall transformation (Hess's law). Standard enthalpies of formation provide... | ΔH°_rxn = Σ ΔH°_f(products) - Σ ΔH°_f(reactants) | first_law | Apply Hess's law to compute reaction enthalpies from tabulated formation data. |
1,274 | chemistry | thermochemistry | hess_law | 5 | explanation | Hess's law and enthalpy as a state function | Enthalpy H is a state function: its change between two states is independent of path. Consequently, the enthalpy change of a reaction may be computed by summing the enthalpy changes of any convenient sequence of reactions that net to the same overall transformation (Hess's law). Standard enthalpies of formation provide... | ΔH°_rxn = Σ ΔH°_f(products) - Σ ΔH°_f(reactants) | first_law | Apply Hess's law to compute reaction enthalpies from tabulated formation data. |
1,275 | chemistry | thermochemistry | hess_law | 5 | explanation | Hess's law and enthalpy as a state function | Enthalpy H is a state function: its change between two states is independent of path. Consequently, the enthalpy change of a reaction may be computed by summing the enthalpy changes of any convenient sequence of reactions that net to the same overall transformation (Hess's law). Standard enthalpies of formation provide... | ΔH°_rxn = Σ ΔH°_f(products) - Σ ΔH°_f(reactants) | first_law | Apply Hess's law to compute reaction enthalpies from tabulated formation data. |
1,276 | chemistry | thermochemistry | hess_law | 5 | explanation | Hess's law and enthalpy as a state function | Enthalpy H is a state function: its change between two states is independent of path. Consequently, the enthalpy change of a reaction may be computed by summing the enthalpy changes of any convenient sequence of reactions that net to the same overall transformation (Hess's law). Standard enthalpies of formation provide... | ΔH°_rxn = Σ ΔH°_f(products) - Σ ΔH°_f(reactants) | first_law | Apply Hess's law to compute reaction enthalpies from tabulated formation data. |
1,277 | chemistry | thermochemistry | hess_law | 5 | explanation | Hess's law and enthalpy as a state function | Enthalpy H is a state function: its change between two states is independent of path. Consequently, the enthalpy change of a reaction may be computed by summing the enthalpy changes of any convenient sequence of reactions that net to the same overall transformation (Hess's law). Standard enthalpies of formation provide... | ΔH°_rxn = Σ ΔH°_f(products) - Σ ΔH°_f(reactants) | first_law | Apply Hess's law to compute reaction enthalpies from tabulated formation data. |
1,278 | chemistry | thermochemistry | hess_law | 5 | explanation | Hess's law and enthalpy as a state function | Enthalpy H is a state function: its change between two states is independent of path. Consequently, the enthalpy change of a reaction may be computed by summing the enthalpy changes of any convenient sequence of reactions that net to the same overall transformation (Hess's law). Standard enthalpies of formation provide... | ΔH°_rxn = Σ ΔH°_f(products) - Σ ΔH°_f(reactants) | first_law | Apply Hess's law to compute reaction enthalpies from tabulated formation data. |
1,279 | chemistry | thermochemistry | hess_law | 5 | explanation | Hess's law and enthalpy as a state function | Enthalpy H is a state function: its change between two states is independent of path. Consequently, the enthalpy change of a reaction may be computed by summing the enthalpy changes of any convenient sequence of reactions that net to the same overall transformation (Hess's law). Standard enthalpies of formation provide... | ΔH°_rxn = Σ ΔH°_f(products) - Σ ΔH°_f(reactants) | first_law | Apply Hess's law to compute reaction enthalpies from tabulated formation data. |
1,280 | chemistry | thermochemistry | hess_law | 5 | explanation | Hess's law and enthalpy as a state function | Enthalpy H is a state function: its change between two states is independent of path. Consequently, the enthalpy change of a reaction may be computed by summing the enthalpy changes of any convenient sequence of reactions that net to the same overall transformation (Hess's law). Standard enthalpies of formation provide... | ΔH°_rxn = Σ ΔH°_f(products) - Σ ΔH°_f(reactants) | first_law | Apply Hess's law to compute reaction enthalpies from tabulated formation data. |
1,281 | chemistry | thermochemistry | hess_law | 5 | explanation | Hess's law and enthalpy as a state function | Enthalpy H is a state function: its change between two states is independent of path. Consequently, the enthalpy change of a reaction may be computed by summing the enthalpy changes of any convenient sequence of reactions that net to the same overall transformation (Hess's law). Standard enthalpies of formation provide... | ΔH°_rxn = Σ ΔH°_f(products) - Σ ΔH°_f(reactants) | first_law | Apply Hess's law to compute reaction enthalpies from tabulated formation data. |
1,282 | chemistry | thermochemistry | hess_law | 5 | explanation | Hess's law and enthalpy as a state function | Enthalpy H is a state function: its change between two states is independent of path. Consequently, the enthalpy change of a reaction may be computed by summing the enthalpy changes of any convenient sequence of reactions that net to the same overall transformation (Hess's law). Standard enthalpies of formation provide... | ΔH°_rxn = Σ ΔH°_f(products) - Σ ΔH°_f(reactants) | first_law | Apply Hess's law to compute reaction enthalpies from tabulated formation data. |
1,283 | chemistry | thermochemistry | hess_law | 5 | explanation | Hess's law and enthalpy as a state function | Enthalpy H is a state function: its change between two states is independent of path. Consequently, the enthalpy change of a reaction may be computed by summing the enthalpy changes of any convenient sequence of reactions that net to the same overall transformation (Hess's law). Standard enthalpies of formation provide... | ΔH°_rxn = Σ ΔH°_f(products) - Σ ΔH°_f(reactants) | first_law | Apply Hess's law to compute reaction enthalpies from tabulated formation data. |
1,284 | chemistry | thermochemistry | hess_law | 5 | explanation | Hess's law and enthalpy as a state function | Enthalpy H is a state function: its change between two states is independent of path. Consequently, the enthalpy change of a reaction may be computed by summing the enthalpy changes of any convenient sequence of reactions that net to the same overall transformation (Hess's law). Standard enthalpies of formation provide... | ΔH°_rxn = Σ ΔH°_f(products) - Σ ΔH°_f(reactants) | first_law | Apply Hess's law to compute reaction enthalpies from tabulated formation data. |
1,285 | chemistry | thermochemistry | hess_law | 5 | explanation | Hess's law and enthalpy as a state function | Enthalpy H is a state function: its change between two states is independent of path. Consequently, the enthalpy change of a reaction may be computed by summing the enthalpy changes of any convenient sequence of reactions that net to the same overall transformation (Hess's law). Standard enthalpies of formation provide... | ΔH°_rxn = Σ ΔH°_f(products) - Σ ΔH°_f(reactants) | first_law | Apply Hess's law to compute reaction enthalpies from tabulated formation data. |
1,286 | chemistry | thermochemistry | hess_law | 5 | explanation | Hess's law and enthalpy as a state function | Enthalpy H is a state function: its change between two states is independent of path. Consequently, the enthalpy change of a reaction may be computed by summing the enthalpy changes of any convenient sequence of reactions that net to the same overall transformation (Hess's law). Standard enthalpies of formation provide... | ΔH°_rxn = Σ ΔH°_f(products) - Σ ΔH°_f(reactants) | first_law | Apply Hess's law to compute reaction enthalpies from tabulated formation data. |
1,287 | chemistry | thermochemistry | hess_law | 5 | explanation | Hess's law and enthalpy as a state function | Enthalpy H is a state function: its change between two states is independent of path. Consequently, the enthalpy change of a reaction may be computed by summing the enthalpy changes of any convenient sequence of reactions that net to the same overall transformation (Hess's law). Standard enthalpies of formation provide... | ΔH°_rxn = Σ ΔH°_f(products) - Σ ΔH°_f(reactants) | first_law | Apply Hess's law to compute reaction enthalpies from tabulated formation data. |
1,288 | chemistry | thermochemistry | hess_law | 5 | explanation | Hess's law and enthalpy as a state function | Enthalpy H is a state function: its change between two states is independent of path. Consequently, the enthalpy change of a reaction may be computed by summing the enthalpy changes of any convenient sequence of reactions that net to the same overall transformation (Hess's law). Standard enthalpies of formation provide... | ΔH°_rxn = Σ ΔH°_f(products) - Σ ΔH°_f(reactants) | first_law | Apply Hess's law to compute reaction enthalpies from tabulated formation data. |
1,289 | chemistry | thermochemistry | hess_law | 5 | explanation | Hess's law and enthalpy as a state function | Enthalpy H is a state function: its change between two states is independent of path. Consequently, the enthalpy change of a reaction may be computed by summing the enthalpy changes of any convenient sequence of reactions that net to the same overall transformation (Hess's law). Standard enthalpies of formation provide... | ΔH°_rxn = Σ ΔH°_f(products) - Σ ΔH°_f(reactants) | first_law | Apply Hess's law to compute reaction enthalpies from tabulated formation data. |
1,290 | chemistry | thermochemistry | hess_law | 5 | explanation | Hess's law and enthalpy as a state function | Enthalpy H is a state function: its change between two states is independent of path. Consequently, the enthalpy change of a reaction may be computed by summing the enthalpy changes of any convenient sequence of reactions that net to the same overall transformation (Hess's law). Standard enthalpies of formation provide... | ΔH°_rxn = Σ ΔH°_f(products) - Σ ΔH°_f(reactants) | first_law | Apply Hess's law to compute reaction enthalpies from tabulated formation data. |
1,291 | chemistry | thermochemistry | hess_law | 5 | explanation | Hess's law and enthalpy as a state function | Enthalpy H is a state function: its change between two states is independent of path. Consequently, the enthalpy change of a reaction may be computed by summing the enthalpy changes of any convenient sequence of reactions that net to the same overall transformation (Hess's law). Standard enthalpies of formation provide... | ΔH°_rxn = Σ ΔH°_f(products) - Σ ΔH°_f(reactants) | first_law | Apply Hess's law to compute reaction enthalpies from tabulated formation data. |
1,292 | chemistry | thermochemistry | hess_law | 5 | explanation | Hess's law and enthalpy as a state function | Enthalpy H is a state function: its change between two states is independent of path. Consequently, the enthalpy change of a reaction may be computed by summing the enthalpy changes of any convenient sequence of reactions that net to the same overall transformation (Hess's law). Standard enthalpies of formation provide... | ΔH°_rxn = Σ ΔH°_f(products) - Σ ΔH°_f(reactants) | first_law | Apply Hess's law to compute reaction enthalpies from tabulated formation data. |
1,293 | chemistry | thermochemistry | hess_law | 5 | explanation | Hess's law and enthalpy as a state function | Enthalpy H is a state function: its change between two states is independent of path. Consequently, the enthalpy change of a reaction may be computed by summing the enthalpy changes of any convenient sequence of reactions that net to the same overall transformation (Hess's law). Standard enthalpies of formation provide... | ΔH°_rxn = Σ ΔH°_f(products) - Σ ΔH°_f(reactants) | first_law | Apply Hess's law to compute reaction enthalpies from tabulated formation data. |
1,294 | chemistry | thermochemistry | hess_law | 5 | explanation | Hess's law and enthalpy as a state function | Enthalpy H is a state function: its change between two states is independent of path. Consequently, the enthalpy change of a reaction may be computed by summing the enthalpy changes of any convenient sequence of reactions that net to the same overall transformation (Hess's law). Standard enthalpies of formation provide... | ΔH°_rxn = Σ ΔH°_f(products) - Σ ΔH°_f(reactants) | first_law | Apply Hess's law to compute reaction enthalpies from tabulated formation data. |
1,295 | chemistry | thermochemistry | hess_law | 5 | explanation | Hess's law and enthalpy as a state function | Enthalpy H is a state function: its change between two states is independent of path. Consequently, the enthalpy change of a reaction may be computed by summing the enthalpy changes of any convenient sequence of reactions that net to the same overall transformation (Hess's law). Standard enthalpies of formation provide... | ΔH°_rxn = Σ ΔH°_f(products) - Σ ΔH°_f(reactants) | first_law | Apply Hess's law to compute reaction enthalpies from tabulated formation data. |
1,296 | chemistry | thermochemistry | hess_law | 5 | explanation | Hess's law and enthalpy as a state function | Enthalpy H is a state function: its change between two states is independent of path. Consequently, the enthalpy change of a reaction may be computed by summing the enthalpy changes of any convenient sequence of reactions that net to the same overall transformation (Hess's law). Standard enthalpies of formation provide... | ΔH°_rxn = Σ ΔH°_f(products) - Σ ΔH°_f(reactants) | first_law | Apply Hess's law to compute reaction enthalpies from tabulated formation data. |
1,297 | chemistry | thermochemistry | hess_law | 5 | explanation | Hess's law and enthalpy as a state function | Enthalpy H is a state function: its change between two states is independent of path. Consequently, the enthalpy change of a reaction may be computed by summing the enthalpy changes of any convenient sequence of reactions that net to the same overall transformation (Hess's law). Standard enthalpies of formation provide... | ΔH°_rxn = Σ ΔH°_f(products) - Σ ΔH°_f(reactants) | first_law | Apply Hess's law to compute reaction enthalpies from tabulated formation data. |
1,298 | chemistry | thermochemistry | hess_law | 5 | explanation | Hess's law and enthalpy as a state function | Enthalpy H is a state function: its change between two states is independent of path. Consequently, the enthalpy change of a reaction may be computed by summing the enthalpy changes of any convenient sequence of reactions that net to the same overall transformation (Hess's law). Standard enthalpies of formation provide... | ΔH°_rxn = Σ ΔH°_f(products) - Σ ΔH°_f(reactants) | first_law | Apply Hess's law to compute reaction enthalpies from tabulated formation data. |
1,299 | chemistry | thermochemistry | hess_law | 5 | explanation | Hess's law and enthalpy as a state function | Enthalpy H is a state function: its change between two states is independent of path. Consequently, the enthalpy change of a reaction may be computed by summing the enthalpy changes of any convenient sequence of reactions that net to the same overall transformation (Hess's law). Standard enthalpies of formation provide... | ΔH°_rxn = Σ ΔH°_f(products) - Σ ΔH°_f(reactants) | first_law | Apply Hess's law to compute reaction enthalpies from tabulated formation data. |
1,300 | chemistry | thermochemistry | hess_law | 5 | explanation | Hess's law and enthalpy as a state function | Enthalpy H is a state function: its change between two states is independent of path. Consequently, the enthalpy change of a reaction may be computed by summing the enthalpy changes of any convenient sequence of reactions that net to the same overall transformation (Hess's law). Standard enthalpies of formation provide... | ΔH°_rxn = Σ ΔH°_f(products) - Σ ΔH°_f(reactants) | first_law | Apply Hess's law to compute reaction enthalpies from tabulated formation data. |
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