Question

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

• A. 1.6atm
• B. 0.16 atm
• C. 16 atm
• D. 160 atm

Answer 1

The correct option is C 16 atm

	$C{O}_2$	$CO$
Initial moles	1	$0$
Equilibrium moles	$0.5$	$1$
Mole fraction	$\frac{0.5}{1.5}=0.33$	$\frac{1}{1.5}=0.66$
Partial pressure	$0.333\times 12=4$	$0.667\times 12=8$

The expression for the equilibrium constant will be $\frac{P_{CO}^2}{P_{C{O}_2}}=\frac{8^2}{4}=16atm$.