Question

Given the reaction below, which of the following would cause an increase in the concentration of products? 4NH3(g) + 3O2(g) <=> 2N2(g) + 6H2O(g)

A. addition of water

B. removal of ammonia

C. adding a catalyst

D. decreasing the volume of the container

E. There is no way to increase the concentration of products in the equilibrium reaction.

Answer 1

A)

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

So, Equilibrium moves to reactant side

b)

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

So, Equilibrium moves to reactant side

c)

Catalyst doesn't affect equilibrium

So, No effect on equilibrium

d)

Decreasing volume will increase the pressure which in turn shift the reaction in a direction which have lesser gaseous molecules as per Le chatelier Principle

Here reactant has less gaseous molecule

So equilibrium will move to left

So, Equilibrium moves to reactant side

Answer: E