Chapter U6, Problem SI2RE

Interpretation Introduction

(a)

Interpretation:

The equilibrium constant equation for the given reversible reaction needs to be determined.

$A\left(aq\right)+B\left(aq\right)\rightleftharpoons C\left(aq\right)+D\left(aq\right)$

Concept introduction:

An equilibrium reaction is represented as follows:

$A+B\rightleftharpoons AB$

For the above reaction, the change in concentration of A and B is equal to that of AB.

For the above reaction, equilibrium constant can be represented as follows:

$K=\frac{\left[AB\right]}{\left[A\right]\left[B\right]}$

Here, K is equilibrium constant.

Explanation of Solution

The given reaction is represented as follows:

$A\left(aq\right)+B\left(aq\right)\rightleftharpoons C\left(aq\right)+D\left(aq\right)$

The equilibrium constant equation for the above reaction will be:

$K=\frac{\left[C\left(aq\right)\right]\left[D\left(aq\right)\right]}{\left[A\left(aq\right)\right]\left[B\left(aq\right)\right]}$

Interpretation Introduction

(b)

Interpretation:

The equilibrium constant equation for the given reversible reaction of needs to be written.

$\text{CO}\left(g\right)+{\text{Cl}}_{\text{2}}\left(g\right)\rightleftharpoons {\text{COCl}}_{\text{2}}\left(g\right)$

Concept introduction:

An equilibrium reaction is represented as follows:

$A+B\rightleftharpoons AB$

For the above reaction, the change in concentration of A and B is equal to that of AB.

For the above reaction, equilibrium constant can be represented as follows:

$K=\frac{\left[AB\right]}{\left[A\right]\left[B\right]}$

Here, K is equilibrium constant.

Explanation of Solution

The given reaction is represented as follows:

$\text{CO}\left(g\right)+{\text{Cl}}_{\text{2}}\left(g\right)\rightleftharpoons {\text{COCl}}_{\text{2}}\left(g\right)$

The equilibrium constant equation can be represented as follows:

$K=\frac{\left[{\text{COCl}}_{\text{2}}\left(g\right)\right]}{\left[\text{CO}\left(g\right)\right]\left[{\text{Cl}}_{\text{2}}\left(g\right)\right]}$

(c)

Interpretation Introduction

Interpretation:

The equilibrium constant equation for the given reversible reaction needs to be determined.

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

Concept introduction:

An equilibrium reaction is represented as follows:

$A+B\rightleftharpoons AB$

For the above reaction, the change in concentration of A and B is equal to that of AB.

For the above reaction, equilibrium constant can be represented as follows:

$K=\frac{\left[AB\right]}{\left[A\right]\left[B\right]}$

Here, K is equilibrium constant.

Explanation of Solution

The given reaction is represented as follows:

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

The equilibrium constant equation for the above reaction can be represented as follows:

$K=\frac{\left[\text{CO}\left(g\right)\right]\left[{\text{H}}_{\text{2}}\text{O}\left(g\right)\right]}{\left[\text{HCOOH}\left(g\right)\right]}$

Here, water is included in the equilibrium expression because it is in vapor form not in solid or liquid form. Only the species in solid and liquid form are not represented in the equilibrium expression.