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Coordination and Oxidation Number

The atmospher...

Question

The atmospheric oxidation of NO
$2 N O (g) + O_{2} (g) ⇌ 2 N O_{2} (g)$
was studied with initial pressure of 1 atm of $N O$ and 1 atm of $O_{2}$ ; At equilibrium, partial pressure of oxygen is $0.52$ atm calculate $K_{p}$ of the reaction.

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Solution

$2 N O_{2} (g) + O_{2} (g) ⇌ 2 N O_{2} (g)$

Given at equilibrium $1 - x = 0.52 ⟹ x = 0.48$

Hence $K - p = \frac{(2 x)^{2}}{(1 - 2 x)^{2} (1 - x)} = \frac{0.96 (0.96)}{0.04 (0.04) (0.52)}$

$K_{p} = 1132$ $a t m^{-}$

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Similar questions

Q. The equilibrium constant

K_{p}

of the reaction:

2 S O_{3} (g) ⇌ 2 S O_{2} (g) + O_{2} (g)

is 900 atm at 800 K. A mixture containing

S O_{3}

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having initial partial pressure of 1 and 2 atm. respectively is heated at constant volume to equilibriate. Calculate the partial pressure of

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K, a sample of pure

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2 N O_{2} (g) ⇌ 2 N O (g) + O_{2} (g)

The equilibrium constant

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156.25

atm. Analysis shows that the partial pressure

0.25

atm at equilibrium. The partial pressure of

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In an experiment when

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In an experiment when

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Q. A sample of pure

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