Chapter 15.6, Problem 15.6.4SR

Interpretation Introduction

Interpretation:

The exothermic and endothermic should be identified given the equilibrium reactions with two different temperatures ${\text{(T}}_{\text{1}}{\text{and T}}_{\text{2}}\text{)}\text{.}$

Concept Introduction:

Equilibrium Concentrations: Concentration of the products to the respective molar concentration of reactants it is called equilibrium constant. If the K value is less than one the reaction will move to the left side and the K values is higher (or) greater than one the reaction will move to the right side of reaction.

Free energy: The change in the standard energy of the system that occurs during a reaction is therefore equal to the change in the enthalpy $(\text{ΔH)}$ of the system minus the change in the respective product of the temperature at the times of entropy of the system, the following equation $\text{G=H-(TS) or (ΔG=ΔH-TΔS)}$.

Exothermic reaction: This type of chemical reaction release energy by light or heat. Endothermic reaction: This type of chemical reactions that is accompanied by the absorption of heat.