Question

Each of the following reactions is allowed to come to equilibrium and then the volume is changed as indicated. Predict the effect (shift right, shift left, or no effect) of the indicated volume change. Drag the appropriate items to their respective bins.
CO(g) + H2O(g) <=> CO2(g) + H2(g)(volume is decreased)PCl3(g) + Cl2(g) <=> PCl5(g)(volume is increased)CaCO3(s)<=> CaO(s) + CO2(g)(volume is increased)

Answer 1

Explanation:

Any change in the equilibrium is studied on the basis of Le-Chatelier's principle.

This principle states that if there is any change in the variables of the reaction, the equilibrium will shift in the direction to minimize the effect.

Increase the volume

If the volume of the container is increased, the pressure will decrease according to Boyle's Law.

Now, according to the Le-Chatlier's principle, the equilibrium will shift in the direction where increase in pressure is taking place.And in order balance pressure reaction will go in direction where gaseous moles are more.

$CO(g) + H_2O(g)\rightleftharpoons CO_2(g) + H_2(g)$(volume is decreased)

Number of moles of gases are same on both sides so, equilibrium will not get effected by increasing the volume.

$PCl3(g) + Cl2(g) \rightleftharpoons PCl5(g)$(volume is increased)

On increasing volume pressure increases the gaseous moles on reactant sides are more so, the reaction will shift in left direction.

$CaCO_3(s)\rightleftharpoons CaO(s) + CO_2(g)$ (volume is increased)

On increasing volume pressure increases the gaseous moles on product sides are more so, the reaction will shift in right direction.