(A): The equilibrium constant for a reaction having positive ΔH^∘ increases with increase of tem

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(A): The equilibrium constant for a reaction having positive...

(A): The equilibrium constant for a reaction having positive $\Delta H^{\circ}$ increases with increase of temperature.
(R): The temperature dependence of the equilibrium constant is related to $\Delta \mathrm{H}^{\circ}$ and not $\Delta \mathrm{H}^{\circ}$ for the reaction.

Key Concepts

Gibbs Free Energy (?G°)

Gibbs free energy (?G°) is a thermodynamic potential that combines enthalpy and entropy to predict the spontaneity of a reaction. Although ?G° is related to the equilibrium constant through the relation ?G° = -RT ln K, it is the enthalpy change (?H°) that primarily dictates how K shifts with temperature, highlighting the different roles these thermodynamic quantities play.

Enthalpy Change (?H°)

?H° represents the standard enthalpy change of a reaction, indicating whether a reaction is endothermic or exothermic. It is a crucial factor in determining the temperature sensitivity of the equilibrium constant. The van't Hoff equation shows that the magnitude and sign of ?H° directly influence how K responds to changes in temperature.

Equilibrium Constant

The equilibrium constant is a numerical value that expresses the ratio of the concentrations or partial pressures of products to reactants at equilibrium for a chemical reaction. Its value provides insight into the favorability of the reaction and the position of equilibrium under a given set of conditions.

Temperature Dependence of Equilibrium

This concept examines how the equilibrium constant changes with temperature. According to principles such as the van’t Hoff equation, the equilibrium constant for an endothermic reaction (positive ?H°) increases with an increase in temperature, while for an exothermic reaction it decreases. This relationship is central in predicting the behavior of chemical systems under varying thermal conditions.

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