Chemical Equilibria|Le Chatelier's Principle|Factors Affecting Chemical equilibria| The Haber Process|The Contact Process|Equilibrium Constants
Consider the following reaction:
N2 (g) + 3H2(g) <=> 2NH3 (g) ∆H = -ve
State 2 conditions which might be chnaged to increase the yield of ammonia gas.
Condition 1: An increase in pressure; side with less number of moles will be favoured, that is right hand side and thus more ammonia will be produced.
Condition 2: A decrease in temperature; enthalpy chnage for the reaction is exothermic. This means that a decrease in temperature will favour side which will liberate energy, that is forward reaction. Thus more ammonia is produced.