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Derivation of Kp and Kc

The equilibri...

Question

The equilibrium constant for the reaction $2 S O_{2} + O_{2} ⇋ 2 S O_{3} i s 900 a t m^{- 1} a t 800 K .$ A mixture containing $S O_{3} a n d O_{2}$ having initial pressures of $1 a t m a n d 2 a t m$ is heated to equilibrate. The partial pressure of $O_{2}$ at equilibrium will be

A

0.97 a t m

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B

0.012 a t m

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C

2.01 a t m

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D

0.024 a t m

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Solution

The correct option is C $2.01 a t m$
Correct option is c). Considering the backward reaction we have,
$\begin{matrix} 2 S O_{3} ⇋ & 2 S O_{2} + & O_{2} & K_{P} = 1 / 900 a t m I n i t i a l p r e s s u r e & 1 a t m & 0 & 2 a t m P r e s s u r e a t e q u i l i b r i u m & 1 - x & x & 2 + x / 2 \end{matrix}$
Let partial pressure of $S O_{2} = p_{1}$ and partial pressure of $O_{2} = p_{2}$ and partial pressure of $S O_{3} = p_{3}$
$K <_{p} = (p_{1})^{2} \times (p_{2}) / (p_{3})^{2} = x^{2} (2 + x / 2) / (1 - x)^{2} = 1 / 900$
$A s K_{p}$ for this reaction is very small, $x << 1.$
Taking $2 + x / 2$ as x and $(1 - x)$ as x and solving for x, we get
$X = 0.0236$
Hence, at equilibrium, partial pressure of $S O_{3} = 1 - X = 0.9764 a t m,$
Partial pressure of $S O_{2} = x = 0.0236 a t m$
And Partial pressure of $O_{2} = 2 + x / 2 = 2.0118 a t m$

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Similar questions

Q. The equilibrium constant for the reaction

2 S O_{2} + O_{2} ⇋ 2 S O_{3} i s 900 a t m^{- 1} a t 800 K .

A mixture containing

S O_{3} a n d O_{2}

having initial pressures of

1 a t m a n d 2 a t m

is heated to equilibrate. The partial pressure of

O_{2}

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Q. The equilibrium constant

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

900 {a t m}^{- 1}

800 K

. A mixture containing

{S O}_{3}

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having initial partial pressure of

1

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The equilibrium constant Kp of the reaction, 2 $S O_{2}$ (g) + $O_{2}$ (g) \(\leftrightharpoons\) 2 $S O_{3}$ (g) is 900 atm. at 800 K. A mixture containing $S O_{3}$ and $O_{2}$ having initial pressure of 1 and 2 atm respectively is heated at constant volume to equilibrate. Calculate the partial pressure of $S O_{2}$ gas at 800 K.

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