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Byju's Answer

Standard XII

Chemistry

Dalton's Law of Partial Pressures

At certain te...

Question

At certain temperature $(T)$ for the gas phase reaction
$2 H_{2} O (g) + 2 C l_{2} (g) ⇌ 4 H C l (g) + O_{2} (g) K_{p} = 12 \times 10^{8} a t m$
If $C l_{2}, H C l$ and $O_{2}$ are mixed in such a manner than the partial pressure of each is $2 a t m$ and the mixture is brough into contact with excess of liquid water. What would be approximate partial pressure of $C l_{2}$ when equilibrium is attained at temperature $(T)$ ?
[Given: Vapour pressure of water is $380 m m H g$ at temperature $(T)$ ]

3.6 \times 10^{- 5} a t m

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10^{- 4} a t m

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3.6 \times 10^{- 3} a t m

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0.01 a t m

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Solution

The correct option is C $3.6 \times 10^{- 3} a t m$
$K_{p}$ , the pressure constant at equilibrium and $K_{c}$ , the equilibrium constant only changes with the change in temperature and no other factor.
$K_{p} = 12 \times 10^{8} a t m; P a r t i a l P r e s s u r e_{w a t e r} = 0.5 a t m$

$2 H_{2} O (g) + 2 C l_{2} (g) ⇋ 4 H C l (g) + O_{2} (g)$
$0.5 - 2 α$ $2 - 2 α$ $2 + 4 α$ $2 + α$

$K_{p} = \frac{(P_{H C l})^{4} \times P_{O_{2}}}{(P_{H_{2} O})^{2} \times (P_{C l_{2}})^{2}}$

$P_{C l_{2}} = 3.6 \times 10^{- 3} a t m$

Hence, option (C) is correct.

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Similar questions

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