Question

The partial pressures of ${CH}_{3}OH,CO$ and $H_2$ in the equilibrium mixture for the reaction $CO+2H_2\rightleftharpoons {CH}_{3}OH$ at ${427}^{o}C$ are $2.0,1.0$ and $0.1$ atm respectively. The value of $K_p$ for the decomposition of ${CH}_{3}OH$ into $CO$ and $H_2$ is:

• A. $1\times {10}^{2}atm$
• B. $2\times {10}^2{atm}^{-1}$
• C. $50{atm}^2$
• D. $5\times {10}^{-3}{atm}^2$

Answer 1

The correct option is D $5\times {10}^{-3}{atm}^2$

The decomposition reaction is :
${CH}_{3}OH\rightleftharpoons CO+2H_2$
$K_P=\frac{P_{CO}{P}_{H2}^2}{P_{CH3OH}}$

$K_P=\frac{1.0atm\times (0.1atm{)}^2}{2.0atm}$

$K_P=5\times {10}^{-3}{atm}^2$