N_(2(g)) + 3H_(2(g)) hArr 2NH_(3(g)), DeltaH=-92.38 "kJ mol"^(-1) the reaction is exothermic. So at lowertemperature more product is obtained still why the reaction is carried out at high temperature ?

N_(2(g)) + 3H_(2(g)) hArr 2NH_(3(g)), DeltaH=-92.38 "kJ mol"^(-1) the

1.	N_(2(g)) + 3H_(2(g)) hArr 2NH_(3(g)), DeltaH=-92.38 "kJ mol"^(-1) the reaction is exothermic. So at lowertemperature more product is obtained still why the reaction is carried out at high temperature ?
Answer» SOLUTION :If the temperature kept LOW than the rate of reaction decreases so equilibrium state is not obtained. Hence the temp must be kept (HIGH) `500^@C` for this reaction.