Consider the following equilibrium system involving SO2, Cl2, and SO2Cl2 (sulfuryl dichloride) : SO2 (g) + Cl2 (g) ⇌ SO2Cl2 (g) Predict how the equilibrium position would change if the temperature remains constant: a. Cl2 gas were added to the system. b. SO2Cl2 were removed from the system. c. SO2 were removed from the system.

(a) forward direction

(b) forward direction

(c) backward direction.

Explanation:

Given, the chemical reaction in equilibrium is,

SO₂ (g) + Cl₂ (g) ⇄ SO₂Cl₂ (g)

The direction of the reaction by changing the concentration can be determined by Le Chatelier's principle,

It states that,

When a reaction is at equlibrium, Changing the concentration, pressure, temperature disturbs the equilibrium, and the reaction again tries to attain equilibrium by counteracting the changes.

(a)

For the reaction, Cl₂ is added to the system, i. e., increasing the concentration of Cl₂, Now, according to Le Chatelier, The reaction will move in forward direction, to reduce the increased amount of Cl₂.

Hence, reaction will go in forward direction.

(b)

Removing SO₂Cl₂ from the system, i. e., decreasing the concentration of SO₂Cl₂, according to Le Chatelier, the reaction will move in forward direction, to increase the amount of reduced SO₂Cl₂.

Hence, reaction will go in forward direction.

(c)

Removing SO₂ from the system, i. e. decreasing the concentration of SO₂, according to Le Chatelier, the reaction will move in backward direction, to increase the amount of reduced SO₂.

Hence, reaction will go in backward direction.