Consider the following reversible reaction at equilibrium: CO(g)+ Cl₂(g) COCl₂(g). If chlorine gas is added to the reaction vessel, the equilibrium will shift to the right.

Question

Quizplus · Accepted Answer

According to Le Chatelier's principle, the addition of chlorine gas (which is a reactant) will cause the equilibrium to shift to the right in order to consume the added chlorine gas. Therefore, the forward reaction will be favored and more product (COCl) will be formed.

Consider the Following Reversible Reaction at Equilibrium: CO(g)+ Cl2(g)

Consider the Following Reversible Reaction at Equilibrium: CO(g)+ Cl₂(g)