Q1. For the exothermic equilibrium 2SO2(g) + O2(g) reversible 2SO3(g), which combination favours the maximum equilibrium yield of SO3?
Explanation
Le Chatelier's principle predicts that lowering temperature favours the exothermic direction, here formation of SO3. Increasing pressure favours the side with fewer gas molecules; the forward side has 2 mol gas compared with 3 mol gas on the reactant side. Therefore low temperature and high pressure give the greater equilibrium yield, apart from kinetic-rate considerations.
