A certain reaction is exothermic in the forward direction and has fewer molecules of gas on the product side. Which set of actions should be used to increase the yield of the products? Decrease the temperature and decrease the pressure. Increase the temperature and decrease the pressure. Decrease the temperature and increase the pressure. Increase the temperature and increase the pressure.

Answer: Option (c) is the correct answer.

Explanation:

According to Le Chatelier's principle, when a system is in equilibrium for a long time then it will change its concentration, temperature, volume or pressure to attain a new equilibrium that partly counteracts the applied change.

Since it is given that reaction is exothermic therefore, according to Le Chatelier's principle increase in temperature will be opposed so that reaction can proceed in the forward direction. Therefore, temperature has to be decreased to carry the reaction in forward direction.

Whereas pressure has to be increased so that reaction will shift to the forward side where there are less number of molecules.

Thus, we can conclude that to increase the yield of the products for the given reaction decrease the temperature and increase the pressure.