Chapter 6.5, Problem 6.18P

Calculate the equilibrium constant for each reaction using the balanced chemical equations and the concentrations of the substances at equilibrium.

1. $\text{CO}\left(\text{g}\right)+{\text{H}}_{\text{2}}\text{O}\left(\text{g}\right)\to {\text{CO}}_{\text{2}}\left(\text{g}\right)+{\text{H}}_{\text{2}}\left(\text{g}\right)$
2. $2{\text{NO}}_2\left(g\right)\to {\text{N}}_2{\text{O}}_4\left(g\right)$
3. $\begin{array}{l}\left[\text{CO}\right]=0.0236\text{M;}\left[{\text{H}}_{\text{2}}\text{O}\right]=0.00240\text{M;}\\ \left[{\text{CO}}_{\text{2}}\right]=0.0164\text{M;}\left[{\text{H}}_{\text{2}}\right]=0.0164\text{M;}\\ \left[{\text{NO}}_{\text{2}}\right]=0.0760\text{M;}\left[{\text{N}}_{\text{2}}{\text{O}}_{\text{4}}\right]=1.26\text{M;}\end{array}$