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Chemistry Question on Equilibrium Constant

For which one of the following systems at equilibrium, at constant temperature will the doubling of die volume cause a shift to the right?

A

\ceH2(g)+Cl2(g)<=>HCl(g)\ce{H2(g) + Cl2(g) <=> HCl(g) }

B

\ce2CO(g)+O2(g)<=>2CO2(g)\ce{2CO(g) + O2(g) <=> 2CO2(g) }

C

\ceN2(g)+3H2(g)<=>NH2(g)\ce{N2(g) + 3H2(g) <=> NH2(g) }

D

\cePCl5(g)<=>PCl3(g)+Cl2(g)\ce{PCl5(g) <=> PCl3(g)+Cl2(g) }

Answer

\cePCl5(g)<=>PCl3(g)+Cl2(g)\ce{PCl5(g) <=> PCl3(g)+Cl2(g) }

Explanation

Solution

When volume is increased the cone, decreases & the equilibrium shifts in the direction where more moles are formed.