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4,701 | chemistry | equilibrium | equilibrium_constant | 6 | explanation | Meaning of equilibrium constant K = 0.8509 | 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 = 0.8509. 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°. |
4,702 | chemistry | equilibrium | equilibrium_constant | 6 | explanation | Meaning of equilibrium constant K = 27.71 | 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 = 27.71. 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°. |
4,703 | chemistry | equilibrium | equilibrium_constant | 6 | explanation | Meaning of equilibrium constant K = 3.3 | 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 = 3.3. 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°. |
4,704 | chemistry | equilibrium | equilibrium_constant | 6 | explanation | Meaning of equilibrium constant K = 0.02139 | 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 = 0.02139. 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°. |
4,705 | chemistry | equilibrium | equilibrium_constant | 6 | explanation | Meaning of equilibrium constant K = 4.479 | 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 = 4.479. 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°. |
4,706 | chemistry | equilibrium | equilibrium_constant | 6 | explanation | Meaning of equilibrium constant K = 40.46 | 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 = 40.46. 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°. |
4,707 | chemistry | equilibrium | equilibrium_constant | 6 | explanation | Meaning of equilibrium constant K = 0.164 | 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 = 0.164. 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°. |
4,708 | chemistry | equilibrium | equilibrium_constant | 6 | explanation | Meaning of equilibrium constant K = 0.1094 | 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 = 0.1094. 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°. |
4,709 | chemistry | equilibrium | equilibrium_constant | 6 | explanation | Meaning of equilibrium constant K = 86.98 | 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 = 86.98. 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°. |
4,710 | chemistry | equilibrium | equilibrium_constant | 6 | explanation | Meaning of equilibrium constant K = 4.607 | 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 = 4.607. 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°. |
4,711 | chemistry | equilibrium | equilibrium_constant | 6 | explanation | Meaning of equilibrium constant K = 32.37 | 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 = 32.37. 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°. |
4,712 | chemistry | equilibrium | equilibrium_constant | 6 | explanation | Meaning of equilibrium constant K = 307.3 | 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 = 307.3. 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°. |
4,713 | chemistry | equilibrium | equilibrium_constant | 6 | explanation | Meaning of equilibrium constant K = 7.472 | 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 = 7.472. 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°. |
4,714 | chemistry | equilibrium | equilibrium_constant | 6 | explanation | Meaning of equilibrium constant K = 0.006737 | 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 = 0.006737. 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°. |
4,715 | chemistry | equilibrium | equilibrium_constant | 6 | explanation | Meaning of equilibrium constant K = 0.01342 | 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 = 0.01342. 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°. |
4,716 | chemistry | equilibrium | equilibrium_constant | 6 | explanation | Meaning of equilibrium constant K = 0.01851 | 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 = 0.01851. 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°. |
4,717 | chemistry | equilibrium | equilibrium_constant | 6 | explanation | Meaning of equilibrium constant K = 0.4096 | 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 = 0.4096. 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°. |
4,718 | chemistry | equilibrium | equilibrium_constant | 6 | explanation | Meaning of equilibrium constant K = 0.109 | 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 = 0.109. 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°. |
4,719 | chemistry | equilibrium | equilibrium_constant | 6 | explanation | Meaning of equilibrium constant K = 8.4 | 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 = 8.4. 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°. |
4,720 | chemistry | equilibrium | equilibrium_constant | 6 | explanation | Meaning of equilibrium constant K = 0.3583 | 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 = 0.3583. 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°. |
4,721 | chemistry | equilibrium | equilibrium_constant | 6 | explanation | Meaning of equilibrium constant K = 0.05126 | 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 = 0.05126. 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°. |
4,722 | chemistry | equilibrium | equilibrium_constant | 6 | explanation | Meaning of equilibrium constant K = 0.2094 | 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 = 0.2094. 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°. |
4,723 | chemistry | equilibrium | equilibrium_constant | 6 | explanation | Meaning of equilibrium constant K = 84.65 | 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 = 84.65. 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°. |
4,724 | chemistry | equilibrium | equilibrium_constant | 6 | explanation | Meaning of equilibrium constant K = 0.001618 | 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 = 0.001618. 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°. |
4,725 | chemistry | equilibrium | equilibrium_constant | 6 | explanation | Meaning of equilibrium constant K = 563.7 | 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 = 563.7. 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°. |
4,726 | chemistry | equilibrium | equilibrium_constant | 6 | explanation | Meaning of equilibrium constant K = 0.3392 | 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 = 0.3392. 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°. |
4,727 | chemistry | equilibrium | equilibrium_constant | 6 | explanation | Meaning of equilibrium constant K = 0.009578 | 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 = 0.009578. 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°. |
4,728 | chemistry | equilibrium | equilibrium_constant | 6 | explanation | Meaning of equilibrium constant K = 12.42 | 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 = 12.42. 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°. |
4,729 | chemistry | equilibrium | equilibrium_constant | 6 | explanation | Meaning of equilibrium constant K = 101.2 | 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 = 101.2. 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°. |
4,730 | chemistry | equilibrium | equilibrium_constant | 6 | explanation | Meaning of equilibrium constant K = 0.6159 | 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 = 0.6159. 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°. |
4,731 | chemistry | equilibrium | equilibrium_constant | 6 | explanation | Meaning of equilibrium constant K = 0.003132 | 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 = 0.003132. 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°. |
4,732 | chemistry | equilibrium | equilibrium_constant | 6 | explanation | Meaning of equilibrium constant K = 13.07 | 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 = 13.07. 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°. |
4,733 | chemistry | equilibrium | equilibrium_constant | 6 | explanation | Meaning of equilibrium constant K = 0.004059 | 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 = 0.004059. 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°. |
4,734 | chemistry | equilibrium | equilibrium_constant | 6 | explanation | Meaning of equilibrium constant K = 149.6 | 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 = 149.6. 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°. |
4,735 | chemistry | equilibrium | equilibrium_constant | 6 | explanation | Meaning of equilibrium constant K = 66.27 | 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 = 66.27. 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°. |
4,736 | chemistry | equilibrium | equilibrium_constant | 6 | explanation | Meaning of equilibrium constant K = 0.001184 | 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 = 0.001184. 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°. |
4,737 | chemistry | equilibrium | equilibrium_constant | 6 | explanation | Meaning of equilibrium constant K = 0.08206 | 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 = 0.08206. 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°. |
4,738 | chemistry | equilibrium | equilibrium_constant | 6 | explanation | Meaning of equilibrium constant K = 2.806 | 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 = 2.806. 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°. |
4,739 | chemistry | equilibrium | equilibrium_constant | 6 | explanation | Meaning of equilibrium constant K = 0.2013 | 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 = 0.2013. 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°. |
4,740 | 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. |
4,741 | 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. |
4,742 | 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. |
4,743 | 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. |
4,744 | 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. |
4,745 | 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. |
4,746 | 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. |
4,747 | 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. |
4,748 | 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. |
4,749 | 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. |
4,750 | 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. |
4,751 | 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. |
4,752 | 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. |
4,753 | 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. |
4,754 | 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. |
4,755 | 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. |
4,756 | 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. |
4,757 | 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. |
4,758 | 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. |
4,759 | 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. |
4,760 | 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. |
4,761 | 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. |
4,762 | 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. |
4,763 | 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. |
4,764 | 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. |
4,765 | 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. |
4,766 | 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. |
4,767 | 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. |
4,768 | 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. |
4,769 | 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. |
4,770 | 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. |
4,771 | 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. |
4,772 | 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. |
4,773 | 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. |
4,774 | 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. |
4,775 | 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. |
4,776 | 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. |
4,777 | 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. |
4,778 | 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. |
4,779 | 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. |
4,780 | biology | cell_biology | cell_theory | 1 | explanation | The Cell Theory | The cell theory states that (1) all living organisms are composed of one or more cells, (2) the cell is the basic unit of structure and organization in organisms, and (3) all cells arise from pre-existing cells. This framework unifies microscopic anatomy with the continuity of life and remains a foundational principle ... | null | null | State the three tenets of cell theory and their significance. |
4,781 | biology | cell_biology | prokaryote_eukaryote | 2 | explanation | Prokaryotic and Eukaryotic Cells | Prokaryotic cells lack a membrane-bounded nucleus and membrane-bounded organelles; their genetic material is typically a single circular chromosome located in the nucleoid. Eukaryotic cells possess a true nucleus enclosed by a nuclear envelope and numerous specialized organelles (mitochondria, endoplasmic reticulum, Go... | null | cell_theory | Compare and contrast the structural organization of prokaryotic and eukaryotic cells. |
4,782 | biology | genetics | dna_structure | 4 | explanation | Structure of DNA | Deoxyribonucleic acid (DNA) is a polymer of nucleotide monomers. Each nucleotide consists of a deoxyribose sugar, a phosphate group, and one of four nitrogenous bases (A, T, C, G). Two antiparallel strands form a double helix stabilized by hydrogen bonds between complementary base pairs (A–T, C–G) and by base stacking.... | null | cell_theory | Describe the molecular structure of DNA and the base-pairing rules. |
4,783 | biology | genetics | central_dogma | 5 | explanation | The Central Dogma of Molecular Biology | The central dogma describes the directional flow of genetic information: DNA is transcribed into RNA, and RNA is translated into protein. Reverse transcription (RNA → DNA) occurs in retroviruses, and RNA replication occurs in many RNA viruses, but the dogma correctly emphasizes that sequence information does not flow f... | null | dna_structure | State the central dogma and note its known exceptions. |
4,784 | biology | evolution | natural_selection | 5 | explanation | Natural Selection | Natural selection is the differential survival and reproduction of individuals due to differences in phenotype. When phenotypic variation is heritable and affects fitness, allele frequencies in the population change over generations. Natural selection is the primary mechanism producing adaptation. It is distinct from o... | null | genetics basics | Explain the conditions required for natural selection and its outcome. |
4,785 | biology | physiology | photosynthesis_overview | 4 | explanation | Overview of Photosynthesis | Photosynthesis converts light energy into chemical energy stored in carbohydrates. In oxygenic photosynthesis the overall reaction is 6 CO₂ + 6 H₂O + light → C₆H₁₂O₆ + 6 O₂. Light-dependent reactions occur in the thylakoid membrane and generate ATP and NADPH while evolving O₂. The Calvin cycle (light-independent reacti... | 6 CO2 + 6 H2O + light -> C6H12O6 + 6 O2 | cell_biology | Summarize the overall reaction and the two main stages of oxygenic photosynthesis. |
4,786 | biology | physiology | cellular_respiration | 5 | explanation | Cellular Respiration Overview | Cellular respiration extracts usable energy from organic molecules. In aerobic respiration the overall process is C₆H₁₂O₆ + 6 O₂ → 6 CO₂ + 6 H₂O + energy (ATP + heat). Glycolysis occurs in the cytosol; the citric acid cycle and oxidative phosphorylation occur in mitochondria of eukaryotic cells. The electron-transport ... | C6H12O6 + 6 O2 -> 6 CO2 + 6 H2O + energy | photosynthesis_overview | Outline the major stages of aerobic cellular respiration and their locations. |
4,787 | biology | cell_biology | organelle_function | 3 | practice_problem | Primary function of the vacuole | Question: What is the primary function of the vacuole in a eukaryotic cell? Answer: storage and turgor maintenance in plant cells. Organelles compartmentalize incompatible biochemical processes and increase efficiency by concentrating enzymes and substrates. | null | prokaryote_eukaryote | Identify the principal function of major eukaryotic organelles. |
4,788 | biology | cell_biology | organelle_function | 3 | practice_problem | Primary function of the mitochondrion | Question: What is the primary function of the mitochondrion in a eukaryotic cell? Answer: ATP synthesis via oxidative phosphorylation. Organelles compartmentalize incompatible biochemical processes and increase efficiency by concentrating enzymes and substrates. | null | prokaryote_eukaryote | Identify the principal function of major eukaryotic organelles. |
4,789 | biology | cell_biology | organelle_function | 3 | practice_problem | Primary function of the vacuole | Question: What is the primary function of the vacuole in a eukaryotic cell? Answer: storage and turgor maintenance in plant cells. Organelles compartmentalize incompatible biochemical processes and increase efficiency by concentrating enzymes and substrates. | null | prokaryote_eukaryote | Identify the principal function of major eukaryotic organelles. |
4,790 | biology | cell_biology | organelle_function | 3 | practice_problem | Primary function of the lysosome | Question: What is the primary function of the lysosome in a eukaryotic cell? Answer: degradation of macromolecules. Organelles compartmentalize incompatible biochemical processes and increase efficiency by concentrating enzymes and substrates. | null | prokaryote_eukaryote | Identify the principal function of major eukaryotic organelles. |
4,791 | biology | cell_biology | organelle_function | 3 | practice_problem | Primary function of the lysosome | Question: What is the primary function of the lysosome in a eukaryotic cell? Answer: degradation of macromolecules. Organelles compartmentalize incompatible biochemical processes and increase efficiency by concentrating enzymes and substrates. | null | prokaryote_eukaryote | Identify the principal function of major eukaryotic organelles. |
4,792 | biology | cell_biology | organelle_function | 3 | practice_problem | Primary function of the mitochondrion | Question: What is the primary function of the mitochondrion in a eukaryotic cell? Answer: ATP synthesis via oxidative phosphorylation. Organelles compartmentalize incompatible biochemical processes and increase efficiency by concentrating enzymes and substrates. | null | prokaryote_eukaryote | Identify the principal function of major eukaryotic organelles. |
4,793 | biology | cell_biology | organelle_function | 3 | practice_problem | Primary function of the Golgi apparatus | Question: What is the primary function of the Golgi apparatus in a eukaryotic cell? Answer: modification, sorting and packaging of proteins. Organelles compartmentalize incompatible biochemical processes and increase efficiency by concentrating enzymes and substrates. | null | prokaryote_eukaryote | Identify the principal function of major eukaryotic organelles. |
4,794 | biology | cell_biology | organelle_function | 3 | practice_problem | Primary function of the lysosome | Question: What is the primary function of the lysosome in a eukaryotic cell? Answer: degradation of macromolecules. Organelles compartmentalize incompatible biochemical processes and increase efficiency by concentrating enzymes and substrates. | null | prokaryote_eukaryote | Identify the principal function of major eukaryotic organelles. |
4,795 | biology | cell_biology | organelle_function | 3 | practice_problem | Primary function of the Golgi apparatus | Question: What is the primary function of the Golgi apparatus in a eukaryotic cell? Answer: modification, sorting and packaging of proteins. Organelles compartmentalize incompatible biochemical processes and increase efficiency by concentrating enzymes and substrates. | null | prokaryote_eukaryote | Identify the principal function of major eukaryotic organelles. |
4,796 | biology | cell_biology | organelle_function | 3 | practice_problem | Primary function of the chloroplast | Question: What is the primary function of the chloroplast in a eukaryotic cell? Answer: photosynthesis. Organelles compartmentalize incompatible biochemical processes and increase efficiency by concentrating enzymes and substrates. | null | prokaryote_eukaryote | Identify the principal function of major eukaryotic organelles. |
4,797 | biology | cell_biology | organelle_function | 3 | practice_problem | Primary function of the vacuole | Question: What is the primary function of the vacuole in a eukaryotic cell? Answer: storage and turgor maintenance in plant cells. Organelles compartmentalize incompatible biochemical processes and increase efficiency by concentrating enzymes and substrates. | null | prokaryote_eukaryote | Identify the principal function of major eukaryotic organelles. |
4,798 | biology | cell_biology | organelle_function | 3 | practice_problem | Primary function of the endoplasmic reticulum | Question: What is the primary function of the endoplasmic reticulum in a eukaryotic cell? Answer: protein and lipid synthesis. Organelles compartmentalize incompatible biochemical processes and increase efficiency by concentrating enzymes and substrates. | null | prokaryote_eukaryote | Identify the principal function of major eukaryotic organelles. |
4,799 | biology | cell_biology | organelle_function | 3 | practice_problem | Primary function of the vacuole | Question: What is the primary function of the vacuole in a eukaryotic cell? Answer: storage and turgor maintenance in plant cells. Organelles compartmentalize incompatible biochemical processes and increase efficiency by concentrating enzymes and substrates. | null | prokaryote_eukaryote | Identify the principal function of major eukaryotic organelles. |
4,800 | biology | cell_biology | organelle_function | 3 | practice_problem | Primary function of the endoplasmic reticulum | Question: What is the primary function of the endoplasmic reticulum in a eukaryotic cell? Answer: protein and lipid synthesis. Organelles compartmentalize incompatible biochemical processes and increase efficiency by concentrating enzymes and substrates. | null | prokaryote_eukaryote | Identify the principal function of major eukaryotic organelles. |
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