Question

In the reaction, $C\left(s\right)+C{O}_2\left(g\right)\rightleftharpoons 2CO\left(g\right)$, the equilibrium pressure is 12 atm. If 50% of $C{O}_2$ reacts, $K_p$ is__________.

Answer 1

$C\left(s\right)+C{O}_2\left(g\right)\rightleftharpoons 2CO\left(g\right)$
Initial gaseous mole $01$
Gaseous mole at equilibrium $1-\left(50/100\right)(50\times 2)/100$
$\therefore$ Total mole $=1.5$
Total pressure at equilibrium = 12 atm
$\therefore K_p=\frac{{\left(n_{CO}\right)}^2}{\left(n_{C{O}_2}\right)}\times {\left[\frac{P}{\sum n}\right]}^{\Delta n}=\frac{{\left(1\right)}^2}{0.5}\times {\left[\frac{12}{1.5}\right]}^1(\because \Delta n=1)$
$=\frac{12}{0.5\times 1.5}=16atm$