Answer:
Increasing the temperature
Step-by-step explanation:
Increasing the temperature would likely increase the yield of products in an exothermic reaction with more moles of gas on the product side due to Le Chatelier's Principle. According to Le Chatelier's Principle, when a system in equilibrium is stressed, it tends to shift in the direction that minimizes the stress. In this case, increasing the temperature is a stress that can be countered by shifting the reaction to the right to consume some of the excess heat. As a result, the system would produce more products to restore equilibrium and reduce the temperature increase. This is because the forward reaction is exothermic and releasing heat helps to offset the temperature rise. Additionally, increasing the temperature can also increase the kinetic energy of the reactant molecules, leading to more frequent and energetic collisions, which can promote the formation of products. Overall, increasing the temperature can help to shift the equilibrium of the exothermic reaction with more moles of gas on the product side to the right, leading to a higher yield of products.