Question

Consider the following system at equilibrium where K. = 1.80x10-2 and AH° = 10.4 kJ/mol at 698 K. 2 HI (g) – H2 (g) +12 (g) The production of H2 (g) is favored by: Indicate True (T) or False (F) for each of the following: - - - 1. increasing the temperature. 2. increasing the pressure (by changing the volume). 3. increasing the volume. 4. adding HI 5. removing 12 . -

Answer 1

1)

Increasing Temperature will shift the reaction in a direction which absorbs heat as per Le chatelier Principle

Forward reaction is endothermic in nature

hence, forward reaction will be favoured

So, Equilibrium moves to product side

So, concentration of H2 will increase

Answer: T

2)

Increasing pressure will shift the reaction in a direction which have lesser 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

So, concentration of H2 will not change

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

So, concentration of H2 will not change

Answer: F

4)

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

So, Equilibrium moves to product side

So, concentration of H2 will increase

Answer: T

5)

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

So, Equilibrium moves to product side

So, concentration of H2 will increase

Answer: T