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Equilibrium Constant and Standard Free Energy Change

Two equilibri...

Question

Two equilibria are simultaneously existing in a vessel at $25^{\circ} C$
$N O (g) + N O_{2} (g) ⇌ N_{2} O_{3} (g) K_{p_{1}} 2 N O_{2} (g) ⇌ N_{2} O_{4} (g) K_{p_{2}} = 8 a t m^{- 1}$
Initially only $N O (g) a n d N O_{2} (g)$ are present in 3 : 5 mole ratio. The total pressure at equilibrium is 5.5 atm and the partial pressure of $N O_{2}$ at equilibrium is 0.5 atm. The incorrect statement regarding the above equilibria is

A

K_{p_{1}}

for the equilibrium is

0.4 a t m^{- 1}

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B

Partial pressure of

N_{2} O_{4}

at equilibrium is 2 atm

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C

Partial pressure of

N_{2} O_{3}

at equilibrium is 2 atm

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D

Partial pressure of NO at equilibrium is 2.5 atm

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Solution

The correct option is C Partial pressure of $N_{2} O_{3}$ at equilibrium is 2 atm
$N O (g) + N O_{2} (g) ⇌ N_{2} O_{3} (g) 3 P 5 P 0 3 P - x (5 p - x - 2 y) x 2 N O_{2} (g) ⇌ N_{2} O_{4} (g) 5 P - x - 2 y y K_{p_{2}} = \frac{P_{N_{2} O_{4}}}{(P_{N O_{2}})^{2}} \Rightarrow 8 = \frac{P_{N_{2} O_{4}}}{(0.5)^{2}} P_{N_{2} O_{4}} = 2 a t m ∴ y = 2 a t m P_{t o t a l} = P_{N O} + P_{N O_{2}} + P_{N_{2} O_{3}} + P_{N_{2} O_{4}} 5.5 = 3 P - x + 0.5 + x + 2 3 P = 3 \Rightarrow P = 1 5 P - x - 2 y = 0.5 5 \times 1 - x - 2 \times 2 = 0.5 \Rightarrow x = 0.5 a t m . P_{N_{2} O_{3}} = x = 0.5 a t m ∴ P_{N O} = 3 - 0.5 = 2.5 a t m K_{p 1} = \frac{P_{N_{2} O_{3}}}{(P_{N O}) (P_{N O_{2}})} = \frac{0.5}{2.5 \times 0.5} = 0.4 a t m^{- 1} ∴ P_{N O} = 2.5 a t m, P_{N O_{2}} = 0.5 a t m, P_{N_{2} O_{3}} = 0.5 a t m, P_{N_{2} O_{4}} = 2 a t m$

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Similar questions

Q. Two equilibria are simultaneously exist in a vessel at

25^{\circ} C

N O (g) + N O_{2} (g)_{p 1} N_{2} O_{3} (g)

2 N O_{2} (g) K_{p 2} = 8 a t m ⇌ N_{2} O_{4} (g)

If initially only NO and

N O_{2}

are present in a 3:5 mole ratio and the total pressure at equilibrium is 5.5 atm with the pressure of

N O_{2}

at 0.5 atm, calculate

K_{p 1}

.

Q. Two equilibria are simultaneously exist in a vessel at

25^{\circ} C

N O (g) + N O_{2} (g)_{p 1} N_{2} O_{3} (g)

2 N O_{2} (g) K_{p 2} = 8 a t m ⇌ N_{2} O_{4} (g)

If initially only NO and

N O_{2}

are present in a 3:5 mole ratio and the total pressure at equilibrium is 5.5 atm with the pressure of

N O_{2}

at 0.5 atm. Select the correct option(s) from the following:

Q. Two equilibria exist simultaneously in a vessel at

25^{\circ} C

\begin{matrix} N O (g) & + & N O_{2} (g) & K_{P 1} = 0.4 a t m^{- 1} ⇌ & N_{2} O_{3} (g) \end{matrix}

\begin{matrix} 2 N O_{2} (g) & K_{P 2} = 8 a t m^{- 1} ⇌ & N_{2} O_{4} (g) \end{matrix}

If initially only

N O

N O_{2}

are present in a 3:5 mole ratio and the final pressure at equilibrium of

N O_{2}

at 0.5 atm, then calculate total pressure (in atm) at equilibrium.

N O

N O_{2}

are mixed, the following equilibria are readily obtained;

2 N O_{2} ⇌ N_{2} O_{4}, K_{P} = 6.8 a t m^{- 1} a n d N O + N O_{2} ⇌ N_{2} O_{3}

In an experiment when

N O

N O_{2}

are mixed in the ratio of 1 : 2, the find total pressure was 5.05 atm and the partial pressure of

N_{2} O_{4}

was 1.7 atm. Calculate the equilibrium partial pressure of NO in atmosphere.

Q. Two equilibria exist simultaneously in a vessel at

25^{\circ} C

\begin{matrix} N O (g) & + & N O_{2} (g) & K_{P 1} = 0.4 a t m^{- 1} ⇌ & N_{2} O_{3} (g) \end{matrix}

\begin{matrix} 2 N O_{2} (g) & K_{P 2} = 8 a t m^{- 1} ⇌ & N_{2} O_{4} (g) \end{matrix}

If initially only

N O

N O_{2}

are present in a 3:5 mole ratio and the final pressure at equilibrium of

N O_{2}

at 0.5 atm, then calculate total pressure (in atm) at equilibrium.

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