Question

Consider the following system at equilibrium where K. = 9.52x10-2 and AH° = 18.8 kJ/mol at 350 K. CH4 (g) + CCl4 (g) – 2 CH2Cl2 (g) The production of CH2Cl2 (g) is favored by: Indicate True (T) or False (F) for each of the following: - 1. decreasing the temperature. 2. decreasing the pressure (by changing the volume). 3. increasing the volume. 4. adding CH2Cl2 - 5. adding CC14 -

Answer 1

1)

Decreasing Temperature will shift the reaction in a direction which release heat as per Le chatelier Principle

Forward reaction is endothermic in nature

hence, backward reaction will be favoured

So, Equilibrium moves to reactant side

The production of CH2Cl2 will not be favoured

Answer: F

2)

Decrease the pressure will shift the reaction in a direction which have greater gaseous molecules as per Le chatelier Principle

Here, number of gaseous molecules is same on both side

So equilibrium will not be effected

So, No effect on equilibrium

The production of CH2Cl2 will not be favoured

Answer: F

3)

Increasing volume will decrease the pressure which in turn shift the reaction in a direction which have greater gaseous molecules as per Le chatelier Principle

Here, number of gaseous molecules is same on both side

So equilibrium will not be effected

So, No effect on equilibrium

The production of CH2Cl2 will not be favoured

Answer: F

4)

Adding product will shift the reaction in the direction of reactant as per Le chatelier Principle

So, Equilibrium moves to reactant side

The production of CH2Cl2 will not be favoured

Answer: F

5)

Adding reactant will shift the reaction in the direction of product as per Le chatelier Principle

So, Equilibrium moves to product side

The production of CH2Cl2 will be favoured

Answer: T