Question

Carbon reacts with water vapor at elevated temperatures

\(C(s) + {H_2}O(g) \rightleftharpoons CO(g) + {H_2}(g)\)

\({K_c} = 0.2at100{0^o}C\)

What is the concentration of CO in an equilibrium mixture with \(\left[ {{H_2}O} \right] = 0.500M\)at \(100{0^0}C\)?

Short answer

The equilibrium concentration of CO is 0.316M.

Step-by-step solution

Find the equilibrium concentration of CO:

Let us assume the concentration of CO and \({H_2}\)is X

Find out the value of X

\(\begin{array}{c}{K_C} = \frac{{[{\rm{CO}}] \times \left[ {{{\rm{H}}_2}} \right]}}{{\left[ {{{\rm{H}}_2}{\rm{O}}} \right]}}\\{K_C} = \frac{{X \times X}}{{\left[ {{{\rm{H}}_2}{\rm{O}}} \right]}}\\{X^2} = {K_C} \times \left[ {{{\rm{H}}_2}{\rm{O}}} \right]\\{X^2} = 0.2 \times 0.5\end{array}\)

\(\begin{array}{c}{X^2} = 0.1\\X = 0.316\,M\\\left[ {CO} \right] = 0.316\,M\end{array}\)