For the reaction NO 2+ CO leftharpoons NO + CO 2 one mole of NO 2 and 2 moles of C O were kept in a vessel. Calculate the equilibrium constant Kp if at equilibrium 25 % of initial amount CO is consumed

Question

For the reaction NO 2+ CO leftharpoons NO + CO 2 one mole of NO 2 and 2 moles of C O were kept in a vessel. Calculate the equilibrium constant Kp if at equilibrium 25 % of initial amount CO is consumed (A) (1/2) (B) (1/3) (C) 1 (D) (1/4)

Tardigrade Admin · Accepted Answer

In this question, we have to assume that volume of the vessel is

1 L

.

Given,

α = 2 \times \frac{25}{100} = 0.5

\Rightarrow K_{C} = \frac{[ NO ] [ C O _{2} ]}{[ N O _{2} ] [ CO ]}

= \frac{0.5 \times 0.35}{0.5 \times 1.5} = \frac{1}{3} = K_{p}

Because,

Δ n_{g} = (1 + 1) - (1 + 1) = 0

\Rightarrow K_{p} = K_{C} (RT)^{Δ n_{ε}} = K_{C} (RT)^{0} = K_{C}

\Rightarrow K_{p} = \frac{1}{3}

Q. For the reaction $N O_{2} + CO ⇌ NO + C O_{2}$ one mole of $N O_{2}$ and 2 moles of $CO$ were kept in a vessel. Calculate the equilibrium constant $K_{p}$ if at equilibrium $25%$ of initial amount $CO$ is consumed

$\frac{1}{2}$

$\frac{1}{3}$

$1$

$\frac{1}{4}$

Q. For the reaction NO2​+CO⇌NO+CO2​ one mole of NO2​ and 2 moles of CO were kept in a vessel. Calculate the equilibrium constant Kp​ if at equilibrium 25% of initial amount CO is consumed

21​

31​

1

41​

In this question, we have to assume that volume of the vessel is 1L. Given, α=2×10025​=0.5 ⇒KC​=[NO2​][CO][NO][CO2​]​ =0.5×1.50.5×0.35​=31​=Kp​ Because, Δng​=(1+1)−(1+1)=0 ⇒Kp​=KC​(RT)Δnε​=KC​(RT)0=KC​ ⇒Kp​=31​

Q. For the reaction $N O_{2} + CO ⇌ NO + C O_{2}$ one mole of $N O_{2}$ and 2 moles of $CO$ were kept in a vessel. Calculate the equilibrium constant $K_{p}$ if at equilibrium $25%$ of initial amount $CO$ is consumed

$\frac{1}{2}$

$\frac{1}{3}$

$1$

$\frac{1}{4}$