In the reaction #SO_2Cl_2 harr SO_2 + Cl_2#, heat is evolved. What happens when chlorine (#Cl_2#) is added to the equilibrium mixture at constant volume?

Question

In the reaction #SO_2Cl_2 harr  SO_2 + Cl_2#, heat is evolved. What happens when chlorine (#Cl_2#) is added to the equilibrium mixture at constant volume?

Henry Antrim · Accepted Answer

reactions will always move to relieve stress. Adding #Cl_2# to the reaction will cause the reaction to move to the left producing more #SO_2Cl_2#

Increasing the concentration of #Cl_2# will increase the concentration of the products on the right side of the equilibrium equation. To decrease the concentration of the products the equilibrium will move to the left producing more reactants.

Since there are two volumes of gas in the products on the left and only one volume in the reactants, increasing the pressure will also cause the equilibrium to move to the left. This movement to the left will lessen the system's stress by lowering the total volume, which will lower the pressure.

Since heat is a product, raising the temperature will likewise cause the equilibrium to move to the left.

Kai Bowman · Answer

undefined Adding more chlorine (Cl2) to the equilibrium mixture at constant volume will shift the equilibrium to the right, favoring the formation of SO2 and Cl2. This occurs because the increase in the concentration of Cl2 disturbs the equilibrium, prompting the system to counteract the change by producing more products.