Question

1) Consider the following reaction at equilibrium. What effect will reducing the pressure of the reaction mixture have on the system? Xe(g) + 2 F2(g) ? XeF4(g) a)The equilibrium constant will decrease. b)No effect will be observed. c)The reaction will shift to the right in the direction of products. d) The equilibrium constant will increase e) The reaction will shift to the left in the direction of reactants.

Answer 1

Answer: e) The reaction will shift to the left in the direction of reactants.

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.

For the given equation:

$Xe(g)+2F_2(g)\leftrightharpoons XeF_4(g)$

If the pressure is reduced, the volume will increase 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. As the number of moles of gas molecules is greater at the reactant side. So, the equilibrium will shift in the left direction. i.e. towards reactants.