Using Le-Chatelier's principle predict the effect of
increasing the pressure on following equilibrium :
`N_(2)(g) + 3H_(2)(g) hArr 2NH_(3)(g) +` Heat

Explanation

The given equilibirum is
`N_(2)(g) + 3H_(2)(g) underset("Endothermic")overset("Exothermic")hArr 2NH_(3)(g)` + Heat
(a) Effect of temperature : Since the reaction is exothermic in forward direction. Therefore, according to Le-Chatelier.s principle, decrease in temperature will shift the equilibrium in forward direction. Thus, it favours the formation of ammonia.
(b) Effect of pressure : We know that with the increase in pressure the number of gaseous moles per unit volume increase. Therefore, according to Le-Chatelier.s principle equilibrium will shift towards the direction of lesser number of gaseous moles. Thus, in the above reaction in pressure will favour the formation of ammonia.