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The partial p...

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The partial pressures of ${C H}_{3} O H, C O$ and $H_{2}$ in the equilibrium mixture for the reaction $C O + 2 H_{2} ⇌ {C H}_{3} O H$ at $427^{o} C$ are $2.0, 1.0$ and $0.1$ atm respectively. The value of $K_{p}$ for the decomposition of ${C H}_{3} O H$ into $C O$ and $H_{2}$ is:

A

1 \times 10^{2} a t m

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B

2 \times 10^{2} {a t m}^{- 1}

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C

50 {a t m}^{2}

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D

5 \times 10^{- 3} {a t m}^{2}

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Solution

The correct option is D $5 \times 10^{- 3} {a t m}^{2}$
The decomposition reaction is :
${C H}_{3} O H ⇌ C O + 2 H_{2}$
$K_{P} = \frac{P_{C O} P_{H 2}^{2}}{P_{C H 3 O H}}$

$K_{P} = \frac{1.0 a t m \times (0.1 a t m)^{2}}{2.0 a t m}$

$K_{P} = 5 \times 10^{- 3} {a t m}^{2}$

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Similar questions

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