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Effect on Kc

If the follow...

Question

If the following reaction has achieved equilibrium in a closed system: $N_{2} O_{4} (g) ⇌ 2 N O_{2} (g)$ . Which of the following is(are) increased by decreasing the size of the container?
I. The value of $K$
II. The concentration of $N_{2} O_{4} (g)$
III. The rate of the reverse reaction

I only

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III only

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I and II only

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II and III only

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I, II and III

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Solution

The correct option is D II and III only
By decreasing the size of the container, we decrease the volume and hence increase the pressure. The equilibrium will shift to the left-hand side so that there is a decrease in the number of moles of gaseous species.
Hence, the following are increased.
II. The concentration of $N_{2} O_{4} (g)$
III. The rate of the reverse reaction
However, the value of the equilibrium constant $K$ is unaffected.

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[C r (N O_{2})_{3} (N H_{3})_{3}]

K_{3} [F e (C_{2} O_{4})_{3}]

[C o C l_{2} (e n)_{2}]^{+}

[C o B r C l (o x)_{2}]^{3 -}

N_{2} O_{4} (g) \to 2 N O_{2} (g)

N_{2} O_{4} (g)

N O_{2}

4.8 \times 10^{- 2}

1.2 \times 10^{- 2}

N_{2} O_{4} (g) ⇌ 2 N O_{2} (g); K_{C} = 4

[N_{2} O_{4}] = [N O_{2}] = 0.1 M

K_{c} = Q

2 N O_{2} (g) \to N_{2} O_{4} (g)

N_{2} O_{4} (g)

2 N O_{2}

N_{2} O_{4} (g)

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