Explanation:
As per Le Chatelier's principle, any disturbance caused in an equilibrium reaction will tend to shift the equilibrium in a direction away from the disturbance.
As the given reaction is as follows.
[tex]X(g) \rightleftharpoons Y(g) + Z(s)[/tex]
- As Z is a solid, so any increase or decrease in its concentration will not disturb the equilibrium. This means no change is taking place.
- As number of moles of gaseous species is the same on each side. Hence, decrease in volume will not affect the equilibrium. This means no change is taking place.
- Since, it is an exothermic reaction which means heat is releasing on the product side. This also means heat is absorbed on the reactant side. Hence, heat is decreasing on reactant side.
Therefore, when we increase the temperature then equilibrium will shift in the backward direction, that is, shift to left.
- When we remove some X then it means there will be a decrease in the concentration of reactants. Hence, equilibrium will shift on the reactant side which means equilibrium will shift to left.
- When we remove some Y then there will be a decrease in concentration of product. Hence, equilibrium will shift on product side which means equilibrium will shift to right.
- When more Y is added then there will be an increase in the concentration of product and a decrease in concentration of reactant. Hence, equilibrium will shift on reactant side which means equilibrium will shift to left.
- When more X is added then concentration of reactant increases. Hence, equilibrium will shift on product side. This means equilibrium will shift to right.
