What is the effect of increasing pressure and temperature on the equilibrium concentration of ammonia in Haber's process

Question

2N2+3H2=2NH3

Enthalpy=+93.6

 

Answer 1

Since ∆H is positive, this is an endothermic reaction and can be written as 

2N₂ + 3H₂ + HEAT ==> 2NH₃

Increasing temperature will push the reaction toward the product side (to the right) because heat is a reactant.

Increasing pressure will push the reaction toward the product side (to the right) because there are fewer moles of gas on the right than on the left (2 v. 5).  This will thus counteract the increase in pressure, which is what Le Chatelier predicts.