Chapter 17, Problem 17.21P

(a)

Interpretation Introduction

Interpretation : The ${\text{K}}_{\text{c}}$ value for the given reaction should be calculated with the help of the reaction:

  $\begin{array}{l}2\text{NO}\left(g\right)+2{\text{H}}_{\text{2}}\left(g\right)\rightleftharpoons {\text{N}}_{\text{2}}\left(g\right)+2{\text{H}}_{\text{2}}\text{O}\left(g\right)K_{\text{c}1}=6.5\times {10}^2\\ \text{NO}\left(g\right)+{\text{H}}_2\left(g\right)\rightleftharpoons \raisebox{1ex}{$1$}\!\left/ \!\raisebox{-1ex}{$2$}\right.{\text{N}}_2\left(g\right)+{\text{ H}}_{\text{2}}\text{O}\left(g\right)K_{\text{c}2}=?\end{array}$

Concept Introduction: When a chemical process reaches equilibrium, the equilibrium constant gives insight into the interaction between the reactants and products. It can be expressed as $K_{\text{c}}$ .

  $A +B \rightleftharpoons C+D$

  $K_{\text{c}}=\frac{[aC][aD]}{[aA][aB]}$

Here, ‘a’ represents the active mass.

(b)

Interpretation Introduction

Interpretation : The $K_c$ value for the given reaction should be calculated with the help of e treaction:

  $\begin{array}{l}2\text{NO}\left(g\right)+2{\text{H}}_{\text{2}}\left(g\right)\rightleftharpoons {\text{N}}_{\text{2}}\left(g\right)+2{\text{H}}_{\text{2}}\text{O}\left(g\right)K_{\text{c}1}=6.5\times {10}^2\\ {\text{2N}}_{\text{2}}\left(g\right)+4{\text{H}}_{\text{2}}\text{O}\left(g\right)\rightleftharpoons 4\text{NO}\left(g\right)+{\text{ 4H}}_{\text{2}}\left(g\right)K_{\text{c}2}=?\end{array}$

Concept Introduction : The equilibrium constants for the reaction which are ratio of gaseous and aqueous products and reactant molecules. It can be expressed as $K_p$ or $K_c$ .

  $A +B \leftrightarrow C+D$

  $K=Kc=\frac{[aC][aD]}{[aA][aB]}$

  $K=Kp=\frac{[PC][PD]}{[PA][PB]}$

Here, ‘a’ represents the active mass and ‘P’ represents the partial pressure.