Question

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.

Answer 1

(a) forward direction

(b) forward direction

(c) backward direction.

Step-by-step 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.