Ai a certain temperature the following equilibrillium is established
$CO (g) + {NO}_{2} (g) ⇌ {CO}_{2} (g) + NO (g)$
One mole of each of the four gases is mixed in one litter container and the reaction is allowed to reach equilibrium state. When excess of baryta water $[Ba ({OH}_{2})]$ is added to the equilibrium mixture, the weight of white precipitate obtained is 236.4 gm. the equilibrium constant $K_{c}$ of the following reaction is :

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1.2

2.25

2.1

3.6

answer is B.

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Detailed Solution

In the following reaction

$CO + NO ⇌ {CO}_{2} + NO$

$1 - x 1 - x$ $1 + x 1 + x$

${CO}_{2} + Ba (OH)_{2} ⟶ {BaCO}_{3} ↓ + H_{2} O$

$n = \frac{236.4}{197} = 1.2 \Rightarrow x = 0.2$

$K_{C} = \frac{1.2 \times 1.2}{0.8 \times 0.8} = 2.25$

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