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Q.

For the reaction $2 NO (g) + {Cl}_{2} (g) ⇌ 2 NOCl (g)$ , a reaction mixture containing $NO (g)$ and ${Cl}_{2} (g)$ at partial pressures of0.373 atm and 0.310 atm, respectively, is taken and at equilibrium the total pressure of the system is found to be 0.544 atm The value of $K_{p}$ for the reaction is

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a

$0.544 {atm}^{- 1}$

b

$(1 / 0.544) {atm}^{- 1}$

c

$25.04 {atm}^{- 1}$

d

$50.08 {atm}^{- 1}$

answer is D.

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Detailed Solution

$2 NO (g) + {Cl}_{2} (g) ⇌ 2 NOCl (g)$

$0.373 atm-2p 0.310 atm - p 2 p$

$\begin{array}{l} p_{total} = (0.373 atm - 2 p) + (0.310 atm - p) + 2 p = 0.683 atm - p \\ p = 0.683 atm - p_{total} = (0.683 - 0.544) atm = 0.139 atm \end{array}$

$K_{p} = \frac{{(p_{NOCI})}^{2}}{{(p_{NO})}^{2} (p_{{Cl}_{2}})} = \frac{(2 \times 0.139 atm)^{2}}{(0.373 - 2 \times 0.139)^{2} (0.310 - 0.139) {atm}^{3}} = 50.08 {atm}^{- 1}$

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For the reaction 2NO(g)+Cl2(g)⇌2NOCl(g), a reaction mixture containing NO(g) and Cl2(g) at partial pressures of0.373 atm and 0.310 atm, respectively, is taken and at equilibrium the total pressure of the system is found to be 0.544 atm The value of Kp for the reaction is