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Standard XII

Chemistry

Law of Mass Action

The initial p...

Question

The initial pressure of $C O C l_{2}$ is $1000$ torr. The total pressure of the system becomes $1500$ torr, when the equilibrium $C O C l_{2} (g) ⇌ C O (g) + C l_{2} (g)$ is attained at constant temperature. The value of $k_{p}$ (in torr) of the reaction is

1500

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1000

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2500

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500

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Solution

The correct option is D $500$
$\begin{matrix} C O C l_{2} (g) & ⇋ & C O (g) & + & C l_{2} (g) at t = 0 & 1000 torr & 0 & 0 at eqm. & 1000 - x & x & x \end{matrix}$

Total pressure at equilibrium $(P_{1}) = 1000 - x + x + x = 1500 \Rightarrow x = 500 torr$

$∴ K_{p} = \frac{P_{C O} \times P_{C l_{2}}}{(P_{C O C l_{2}})} \Rightarrow K_{p} = \frac{500 \times 500}{500} = 500 torr$

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Similar questions

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NO and $B r_{2}$ at initial partial pressure of 98.4 and 41.3 torr, respectively were allowed to react at 300K. At equilibrium the total pressure was 110.5 torr. Calculate the value of KP for the following reaction at 300K.

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The initial pressure of COCl2 is 1000 torr. The total pressure of the system becomes 1500 torr, when the equilibrium COCl2(g)⇌CO(g)+Cl2(g) is attained at constant temperature. The value of kp (in torr) of the reaction is

The correct option is D 500COCl2(g)⇋CO(g)+Cl2(g)at t=01000 torr00at eqm.1000−xxx Total pressure at equilibrium (P1)=1000−x+x+x=1500⇒x=500 torr ∴Kp=PCO×PCl2(PCOCl2)⇒Kp=500×500500=500 torr

The initial pressure of $C O C l_{2}$ is $1000$ torr. The total pressure of the system becomes $1500$ torr, when the equilibrium $C O C l_{2} (g) ⇌ C O (g) + C l_{2} (g)$ is attained at constant temperature. The value of $k_{p}$ (in torr) of the reaction is