Question

How wil the following changes affect the equilibrium listed below?

4NH3 (g) + 3O2 (g) <---> 2N2 (g) + 6H20 (g) delta H = -1531 kJ

A) Increasing the size of the reactions vessel

B) Adding a catalyst

C) Adding extra ammonia

D) Lowering the temperature

Answer 1

A)

We are increasing volume here

In other words we are trying to decrease pressure

so, according to Le Chatelier's principle,

Reaction will try to increase the pressure

Hence it will move in a direction which have more gaseous molecules

Here product has more gaseous molecule

So equilibrium will move to right

Answer: Equilibrium moves to product side

B)

Catalyst doesn't affect equilibrium

Answer: No effect on equilibrium

C)

we are adding a reactant

According to Le Chatelier's Principle,

Adding reactant will shift reaction towards product side

Answer: Equilibrium moves to product side

D)

Forward reaction is exothermic in nature

we are decreasing temperature or removing heat here

so, according to Le Chatelier's principle,

equilibrium will move in direction which release heat

hence, forward reaction will be favoured

Answer: Equilibrium moves to product side