Chapter 14, Problem 14.57QE

Interpretation Introduction

Interpretation:

The concentration of all species after the attainment of equilibrium in the following reaction has to be determined.

  $\text{CO}\left(\text{g}\right)+{\text{H}}_{\text{2}}\left(\text{g}\right)\rightleftharpoons {\text{CH}}_2\text{O}\left(\text{g}\right)$

Concept Introduction:

The condition of equilibrium is a state of balance of processes that runs in opposite directions. At equilibrium, the formation of a product from the reactant balances the formation of a reactant from the product. Also, the change in concentration of reaction and product seems to be negligible at equilibrium state.

The general equilibrium reaction is as follows:

  $a\text{A}+b\text{B}\rightleftharpoons c\text{C}+d\text{D}$

Here,

$\text{A}$ and $\text{B}$ are the reactants.

$\text{C}$ and $\text{D}$ are products.

$a$ and $b$ are the stoichiometric coefficients of reactants.

$c$ and $d$ are the stoichiometric coefficients of products.

The expression of the equilibrium constant for the above reaction is as follows:

  $K_{\text{p}}=\frac{P_{\text{C}}^c{P}_{\text{D}}^d}{P_{\text{A}}^a{P}_{\text{B}}^b}$

Here,

$K_{\text{p}}$ is the equilibrium constant.

$P_{\text{C}}$ is the partial pressure of $\text{C}$.

$P_{\text{D}}$ is the partial pressure of $\text{D}$.

$P_{\text{A}}$ is the partial pressure of $\text{A}$.

$P_{\text{B}}$ is the partial pressure of $\text{B}$.