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Question

For which of the following reactions at equilibrium at constant temperature, doubling the volume will shift equilibrium towards right?

A
N2O4(g)2NO2(g)
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B
CaCO3(s)CaO(s)+CO2(g)
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C
2CO(g)+O22CO2(g)
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D
N2(g)+O2(g)2NO(g)
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Solution

The correct option is B CaCO3(s)CaO(s)+CO2(g)

Calculating Δng
Option A : 21=1=+ve
Option B : 10=1=+ve
Option C : 23=1=ve
Option D : 22=0

Doubling the volume would reduce the pressure and shift the equilibrium in the direction where there is more number of moles of gases i.e where Δngis +ve
In choices (A) and (B), Δng is +ve, and thus on doubling volume, the equilibrium will shift to the right.

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