Chapter 15, Problem 15.141SP

Interpretation Introduction

Interpretation:

Whether the given reaction ${\text{CO}}_{\text{2}}\left(\text{g}\right)\rightleftharpoons {\text{N}}_{\text{2}}\left(\text{g}\right)\text{+CO}\left(\text{g}\right){\text{+N}}_{\text{2}}\text{O}\left(\text{g}\right)$ is exothermic or endothermic needs to be determined in terms of kinetics.

Concept introduction:

For the equilibrium reaction, the expression for the equilibrium constant is the ratio of concentration of product to reactant raised to their stoichiometric coefficients.

The equilibrium constant can also be calculated in terms of partial pressure of each gas at equilibrium. It is denoted by symbol K_pand equal to the ratio of partial pressure of product to reactant. A reaction is said to be endothermic if heat is required to start the reaction and it is exothermic if heat is released.