Question

The equilibrium constant for the reaction
$C{O}_{\left(g\right)}+H_2{O}_{\left(g\right)}\rightleftharpoons C{O}_{2\left(g\right)}+H_{2\left(g\right)}$ at a certain temperature is $2.2$. Initially one mole of CO and one mole of $H_{2}O$ are placed in a $2.0$L container. What are the concentrations of all the substances when the reaction reached equilibrium?
$\left(\right[C{O}_2]=[H_2]=0.2986M,[CO]=[H_{2}O]=0.2014M)$

Answer 1

${CO}_{\left(g\right)}+H_2{O}_{\left(g\right)}\rightleftharpoons {CO}_{2\left(g\right)}+H_{2\left(g\right)}$

$0.2014$ $0.2014$ $0.2986$ $0.2986$ initial

$0.2014-x$ $0.2014-x$ $0.2986+x$ $0.2986+x$

$K_C=\frac{{[2.2986+x]}^2}{{[0.2014-x]}^2}$

$2.2=\frac{{[0.2986+x]}^2}{{[0.2014-x]}^2}\Rightarrow x=10.7$