id int64 1 14M | domain stringclasses 6
values | topic stringclasses 23
values | subtopic stringclasses 37
values | difficulty int64 1 8 | unit_type stringclasses 3
values | title stringlengths 14 86 | content stringlengths 203 553 | key_equations stringclasses 23
values | prerequisites stringclasses 29
values | learning_objective stringclasses 37
values |
|---|---|---|---|---|---|---|---|---|---|---|
6,401 | chemistry | acids_bases | strong_acid_ph | 4 | worked_example | pH of strong acid at concentration 0.004998 M | A strong monoprotic acid is fully dissociated. At concentration 0.004998 mol/L, [H⁺] = 0.004998 M and pH = −log₁₀[H⁺] = 2.301. 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. |
6,402 | chemistry | acids_bases | strong_acid_ph | 4 | worked_example | pH of strong acid at concentration 0.002007 M | A strong monoprotic acid is fully dissociated. At concentration 0.002007 mol/L, [H⁺] = 0.002007 M and pH = −log₁₀[H⁺] = 2.698. 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. |
6,403 | chemistry | acids_bases | strong_acid_ph | 4 | worked_example | pH of strong acid at concentration 1.2298e-04 M | A strong monoprotic acid is fully dissociated. At concentration 1.2298e-04 mol/L, [H⁺] = 1.2298e-04 M and pH = −log₁₀[H⁺] = 3.91. 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. |
6,404 | chemistry | acids_bases | strong_acid_ph | 4 | worked_example | pH of strong acid at concentration 0.02593 M | A strong monoprotic acid is fully dissociated. At concentration 0.02593 mol/L, [H⁺] = 0.02593 M and pH = −log₁₀[H⁺] = 1.586. 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. |
6,405 | chemistry | acids_bases | strong_acid_ph | 4 | worked_example | pH of strong acid at concentration 0.0225 M | A strong monoprotic acid is fully dissociated. At concentration 0.0225 mol/L, [H⁺] = 0.0225 M and pH = −log₁₀[H⁺] = 1.648. 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. |
6,406 | chemistry | acids_bases | strong_acid_ph | 4 | worked_example | pH of strong acid at concentration 0.001655 M | A strong monoprotic acid is fully dissociated. At concentration 0.001655 mol/L, [H⁺] = 0.001655 M and pH = −log₁₀[H⁺] = 2.781. 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. |
6,407 | chemistry | acids_bases | strong_acid_ph | 4 | worked_example | pH of strong acid at concentration 0.01947 M | A strong monoprotic acid is fully dissociated. At concentration 0.01947 mol/L, [H⁺] = 0.01947 M and pH = −log₁₀[H⁺] = 1.711. 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. |
6,408 | chemistry | acids_bases | strong_acid_ph | 4 | worked_example | pH of strong acid at concentration 0.0043 M | A strong monoprotic acid is fully dissociated. At concentration 0.0043 mol/L, [H⁺] = 0.0043 M and pH = −log₁₀[H⁺] = 2.366. 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. |
6,409 | chemistry | acids_bases | strong_acid_ph | 4 | worked_example | pH of strong acid at concentration 2.7532e-04 M | A strong monoprotic acid is fully dissociated. At concentration 2.7532e-04 mol/L, [H⁺] = 2.7532e-04 M and pH = −log₁₀[H⁺] = 3.56. 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. |
6,410 | chemistry | acids_bases | strong_acid_ph | 4 | worked_example | pH of strong acid at concentration 0.009611 M | A strong monoprotic acid is fully dissociated. At concentration 0.009611 mol/L, [H⁺] = 0.009611 M and pH = −log₁₀[H⁺] = 2.017. 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. |
6,411 | chemistry | acids_bases | strong_acid_ph | 4 | worked_example | pH of strong acid at concentration 1.9076e-04 M | A strong monoprotic acid is fully dissociated. At concentration 1.9076e-04 mol/L, [H⁺] = 1.9076e-04 M and pH = −log₁₀[H⁺] = 3.72. 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. |
6,412 | chemistry | acids_bases | strong_acid_ph | 4 | worked_example | pH of strong acid at concentration 0.004486 M | A strong monoprotic acid is fully dissociated. At concentration 0.004486 mol/L, [H⁺] = 0.004486 M and pH = −log₁₀[H⁺] = 2.348. 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. |
6,413 | chemistry | acids_bases | strong_acid_ph | 4 | worked_example | pH of strong acid at concentration 0.005233 M | A strong monoprotic acid is fully dissociated. At concentration 0.005233 mol/L, [H⁺] = 0.005233 M and pH = −log₁₀[H⁺] = 2.281. 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. |
6,414 | chemistry | acids_bases | strong_acid_ph | 4 | worked_example | pH of strong acid at concentration 0.001082 M | A strong monoprotic acid is fully dissociated. At concentration 0.001082 mol/L, [H⁺] = 0.001082 M and pH = −log₁₀[H⁺] = 2.966. 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. |
6,415 | chemistry | acids_bases | strong_acid_ph | 4 | worked_example | pH of strong acid at concentration 0.007781 M | A strong monoprotic acid is fully dissociated. At concentration 0.007781 mol/L, [H⁺] = 0.007781 M and pH = −log₁₀[H⁺] = 2.109. 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. |
6,416 | chemistry | acids_bases | strong_acid_ph | 4 | worked_example | pH of strong acid at concentration 0.05894 M | A strong monoprotic acid is fully dissociated. At concentration 0.05894 mol/L, [H⁺] = 0.05894 M and pH = −log₁₀[H⁺] = 1.23. 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. |
6,417 | chemistry | equilibrium | equilibrium_constant | 6 | explanation | Meaning of equilibrium constant K = 0.01994 | 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 = 0.01994. 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°. |
6,418 | chemistry | equilibrium | equilibrium_constant | 6 | explanation | Meaning of equilibrium constant K = 2.348 | 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 = 2.348. 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°. |
6,419 | chemistry | equilibrium | equilibrium_constant | 6 | explanation | Meaning of equilibrium constant K = 71.2 | 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 = 71.2. 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°. |
6,420 | chemistry | equilibrium | equilibrium_constant | 6 | explanation | Meaning of equilibrium constant K = 0.003886 | 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 = 0.003886. 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°. |
6,421 | chemistry | equilibrium | equilibrium_constant | 6 | explanation | Meaning of equilibrium constant K = 96.31 | 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 = 96.31. 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°. |
6,422 | chemistry | equilibrium | equilibrium_constant | 6 | explanation | Meaning of equilibrium constant K = 196.7 | 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 = 196.7. 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°. |
6,423 | chemistry | equilibrium | equilibrium_constant | 6 | explanation | Meaning of equilibrium constant K = 39.71 | 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 = 39.71. 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°. |
6,424 | chemistry | equilibrium | equilibrium_constant | 6 | explanation | Meaning of equilibrium constant K = 69.73 | 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 = 69.73. 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°. |
6,425 | chemistry | equilibrium | equilibrium_constant | 6 | explanation | Meaning of equilibrium constant K = 0.07624 | 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 = 0.07624. 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°. |
6,426 | chemistry | equilibrium | equilibrium_constant | 6 | explanation | Meaning of equilibrium constant K = 0.105 | 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 = 0.105. 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°. |
6,427 | chemistry | equilibrium | equilibrium_constant | 6 | explanation | Meaning of equilibrium constant K = 349.1 | 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 = 349.1. 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°. |
6,428 | chemistry | equilibrium | equilibrium_constant | 6 | explanation | Meaning of equilibrium constant K = 0.005262 | 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 = 0.005262. 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°. |
6,429 | chemistry | equilibrium | equilibrium_constant | 6 | explanation | Meaning of equilibrium constant K = 114.8 | 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 = 114.8. 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°. |
6,430 | chemistry | equilibrium | equilibrium_constant | 6 | explanation | Meaning of equilibrium constant K = 46.06 | 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 = 46.06. 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°. |
6,431 | chemistry | equilibrium | equilibrium_constant | 6 | explanation | Meaning of equilibrium constant K = 0.2466 | 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 = 0.2466. 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°. |
6,432 | chemistry | equilibrium | equilibrium_constant | 6 | explanation | Meaning of equilibrium constant K = 0.007829 | 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 = 0.007829. 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°. |
6,433 | chemistry | equilibrium | equilibrium_constant | 6 | explanation | Meaning of equilibrium constant K = 3.355 | 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 = 3.355. 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°. |
6,434 | chemistry | equilibrium | equilibrium_constant | 6 | explanation | Meaning of equilibrium constant K = 43.54 | 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 = 43.54. 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°. |
6,435 | chemistry | equilibrium | equilibrium_constant | 6 | explanation | Meaning of equilibrium constant K = 125.5 | 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 = 125.5. 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°. |
6,436 | chemistry | equilibrium | equilibrium_constant | 6 | explanation | Meaning of equilibrium constant K = 0.0428 | 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 = 0.0428. 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°. |
6,437 | chemistry | equilibrium | equilibrium_constant | 6 | explanation | Meaning of equilibrium constant K = 247.7 | 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 = 247.7. 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°. |
6,438 | chemistry | equilibrium | equilibrium_constant | 6 | explanation | Meaning of equilibrium constant K = 134.2 | 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 = 134.2. 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°. |
6,439 | chemistry | equilibrium | equilibrium_constant | 6 | explanation | Meaning of equilibrium constant K = 98.9 | 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 = 98.9. 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°. |
6,440 | chemistry | equilibrium | equilibrium_constant | 6 | explanation | Meaning of equilibrium constant K = 0.009671 | 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 = 0.009671. 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°. |
6,441 | chemistry | equilibrium | equilibrium_constant | 6 | explanation | Meaning of equilibrium constant K = 32.66 | 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 = 32.66. 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°. |
6,442 | chemistry | equilibrium | equilibrium_constant | 6 | explanation | Meaning of equilibrium constant K = 0.001014 | 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 = 0.001014. 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°. |
6,443 | chemistry | equilibrium | equilibrium_constant | 6 | explanation | Meaning of equilibrium constant K = 10.15 | 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 = 10.15. 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°. |
6,444 | chemistry | equilibrium | equilibrium_constant | 6 | explanation | Meaning of equilibrium constant K = 1.212 | 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 = 1.212. 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°. |
6,445 | chemistry | equilibrium | equilibrium_constant | 6 | explanation | Meaning of equilibrium constant K = 4.003 | 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 = 4.003. 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°. |
6,446 | chemistry | equilibrium | equilibrium_constant | 6 | explanation | Meaning of equilibrium constant K = 278 | 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 = 278. 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°. |
6,447 | chemistry | equilibrium | equilibrium_constant | 6 | explanation | Meaning of equilibrium constant K = 0.2166 | 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 = 0.2166. 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°. |
6,448 | chemistry | equilibrium | equilibrium_constant | 6 | explanation | Meaning of equilibrium constant K = 978.7 | 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 = 978.7. 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°. |
6,449 | chemistry | equilibrium | equilibrium_constant | 6 | explanation | Meaning of equilibrium constant K = 0.00502 | 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 = 0.00502. 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°. |
6,450 | chemistry | equilibrium | equilibrium_constant | 6 | explanation | Meaning of equilibrium constant K = 754.9 | 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 = 754.9. 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°. |
6,451 | chemistry | equilibrium | equilibrium_constant | 6 | explanation | Meaning of equilibrium constant K = 0.2104 | 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 = 0.2104. 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°. |
6,452 | chemistry | equilibrium | equilibrium_constant | 6 | explanation | Meaning of equilibrium constant K = 0.01631 | 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 = 0.01631. 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°. |
6,453 | chemistry | equilibrium | equilibrium_constant | 6 | explanation | Meaning of equilibrium constant K = 0.003071 | 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 = 0.003071. 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°. |
6,454 | chemistry | equilibrium | equilibrium_constant | 6 | explanation | Meaning of equilibrium constant K = 0.01445 | 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 = 0.01445. 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°. |
6,455 | chemistry | equilibrium | equilibrium_constant | 6 | explanation | Meaning of equilibrium constant K = 4.692 | 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 = 4.692. 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°. |
6,456 | chemistry | equilibrium | equilibrium_constant | 6 | explanation | Meaning of equilibrium constant K = 87.37 | 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 = 87.37. 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°. |
6,457 | chemistry | equilibrium | equilibrium_constant | 6 | explanation | Meaning of equilibrium constant K = 87.09 | 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 = 87.09. 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°. |
6,458 | chemistry | equilibrium | equilibrium_constant | 6 | explanation | Meaning of equilibrium constant K = 0.001422 | 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 = 0.001422. 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°. |
6,459 | chemistry | equilibrium | equilibrium_constant | 6 | explanation | Meaning of equilibrium constant K = 470 | 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 = 470. 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°. |
6,460 | chemistry | equilibrium | equilibrium_constant | 6 | explanation | Meaning of equilibrium constant K = 0.1783 | 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 = 0.1783. 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°. |
6,461 | chemistry | equilibrium | equilibrium_constant | 6 | explanation | Meaning of equilibrium constant K = 0.002167 | 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 = 0.002167. 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°. |
6,462 | chemistry | equilibrium | equilibrium_constant | 6 | explanation | Meaning of equilibrium constant K = 7.757 | 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 = 7.757. 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°. |
6,463 | chemistry | equilibrium | equilibrium_constant | 6 | explanation | Meaning of equilibrium constant K = 0.003024 | 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 = 0.003024. 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°. |
6,464 | chemistry | equilibrium | equilibrium_constant | 6 | explanation | Meaning of equilibrium constant K = 6.014 | 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 = 6.014. 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°. |
6,465 | chemistry | equilibrium | equilibrium_constant | 6 | explanation | Meaning of equilibrium constant K = 0.002748 | 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 = 0.002748. 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°. |
6,466 | chemistry | equilibrium | equilibrium_constant | 6 | explanation | Meaning of equilibrium constant K = 26.69 | 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 = 26.69. 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°. |
6,467 | chemistry | equilibrium | equilibrium_constant | 6 | explanation | Meaning of equilibrium constant K = 0.002118 | 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 = 0.002118. 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°. |
6,468 | chemistry | equilibrium | equilibrium_constant | 6 | explanation | Meaning of equilibrium constant K = 0.2797 | 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 = 0.2797. 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°. |
6,469 | chemistry | equilibrium | equilibrium_constant | 6 | explanation | Meaning of equilibrium constant K = 0.01156 | 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 = 0.01156. 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°. |
6,470 | chemistry | equilibrium | equilibrium_constant | 6 | explanation | Meaning of equilibrium constant K = 5.987 | 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 = 5.987. 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°. |
6,471 | chemistry | equilibrium | equilibrium_constant | 6 | explanation | Meaning of equilibrium constant K = 0.01498 | 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 = 0.01498. 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°. |
6,472 | chemistry | equilibrium | equilibrium_constant | 6 | explanation | Meaning of equilibrium constant K = 3.124 | 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 = 3.124. 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°. |
6,473 | chemistry | equilibrium | equilibrium_constant | 6 | explanation | Meaning of equilibrium constant K = 0.457 | 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 = 0.457. 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°. |
6,474 | chemistry | equilibrium | equilibrium_constant | 6 | explanation | Meaning of equilibrium constant K = 0.293 | 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 = 0.293. 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°. |
6,475 | chemistry | equilibrium | equilibrium_constant | 6 | explanation | Meaning of equilibrium constant K = 0.007276 | 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 = 0.007276. 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°. |
6,476 | chemistry | equilibrium | equilibrium_constant | 6 | explanation | Meaning of equilibrium constant K = 23.98 | 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 = 23.98. 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°. |
6,477 | 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. |
6,478 | 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. |
6,479 | 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. |
6,480 | 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. |
6,481 | 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. |
6,482 | 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. |
6,483 | 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. |
6,484 | 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. |
6,485 | 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. |
6,486 | 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. |
6,487 | 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. |
6,488 | 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. |
6,489 | 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. |
6,490 | 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. |
6,491 | 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. |
6,492 | 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. |
6,493 | 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. |
6,494 | 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. |
6,495 | 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. |
6,496 | 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. |
6,497 | 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. |
6,498 | 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. |
6,499 | 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. |
6,500 | 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. |
Subsets and Splits
No community queries yet
The top public SQL queries from the community will appear here once available.