Magnesium carbonate dissociates to magnesium oxide and carbon dioxide at elevate

Question

Magnesium carbonate dissociates to magnesium oxide and carbon dioxide at elevated temperatures. MgCO3(s) = MgO(s) + CO2(g). A reaction vessel contains these compounds in equilibrium at 300C. What will happen if the volume of the container is reduced by 25% at 300C?

a)the partial pressure of carbon dioxide present at equilibrium will increase.

b) the partial pressure of carbon dioxide present at equilibrium will decrease.

c) the partial pressure of carbon dioxide at equilibrium will be unchanged.

d) the equilibrium constant will have to decrease to compensate for the decrease in volume.

e) more information is needed in order to make a valid judgment.

I know the answer is suppose to be "c," but why? I thought "a" would be correct because the decrease in volume leads to an increase in pressure.

Explanation / Answer

The correct answer will be Option C

Reason: Keq for this reaction will be just [CO2(g)], since the volume change will try to shift the equilibrium, so the concentration must became the same in order to get the same equilibrium constant, since equilibrium only depends on [CO2[, hence the partial pressure must not be changed to same the value of Kp

Hence the correct answer is Option C

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