Chemistry related question

Question

The reaction for the formation of ammonia by direct combination is

N2 + 3H2 →← 2NH3 ∆H = –92 kJ

(A) doubling the concentration of hydrogen

(B) reducing the total pressure

(C) raising the temperature

(D) increasing the reaction time

(E) adding a catalyst

Could you explain which answer/option is correct

Answer 1

N₂ + 3H₂ <==> 2NH₃ .. ∆H = –92 kJ

Which operation will increase the yield of ammonia in the equilibrium mixture?

(A) doubling the concentration of hydrogen

This will shift equilibrium to the right making more NH₃

(B) reducing the total pressure

This will shift equilibrium to the left making more N₂ and H₂ and less NH₃

(C) raising the temperature

This will shift equilibrium to the left making less NH₃ because -kJ means exothermic rxn

(D) increasing the reaction time

This will not have an effect on equilibrium position

(E) adding a catalyst

This will not have an effect on equilibrium position