Chemistry
Chemistry
Problem
The gaseous equilibrium CO(g) + Cl₂(g) ⇌ COCl₂(g) is established in a sealed vessel at 500 K. After equilibrium is reached, a small amount of COCl₂(g) is suddenly injected, instantly increasing its concentration. Predict whether the concentration of Cl₂ will increase, decrease, or remain unchanged as the system attains its new equilibrium, and briefly justify your answer.Intuitive explanation
When you suddenly add COCl₂, you push the system away from equilibrium—the reaction quotient jumps above . The system must shift left (toward reactants) to restore balance, which means the reverse reaction consumes COCl₂ and regenerates CO and Cl₂. Since Cl₂ is produced during this leftward shift, its concentration will increase until the new equilibrium is reached at the same value.
Intuitive explanation
When you suddenly add COCl₂, you push the system away from equilibrium—the reaction quotient jumps above . The system must shift left (toward reactants) to restore balance, which means the reverse reaction consumes COCl₂ and regenerates CO and Cl₂. Since Cl₂ is produced during this leftward shift, its concentration will increase until the new equilibrium is reached at the same value.