Le Chatelier's Principle for Del N Greater Than Zero
For which of ...
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)+O2⇌2CO2(g)
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D
N2(g)+O2(g)⇌2NO(g)
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Solution
The correct option is BCaCO3(s)⇌CaO(s)+CO2(g)
Calculating Δng
Option A : 2−1=1=+ve
Option B : 1−0=1=+ve
Option C : 2−3=−1=−ve
Option D : 2−2=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.