For the reaction below, describe the temperature and pressure conditions that would produce the highest yield of the forward reaction. Explain your answer in terms of Le Châtelier's principle.

The correct answer for the question that is being presented above is this one: "CO (g) + 2H2 (g) CH3OH (g) and that the reaction is exothermic (the delta H value is negative). The reaction is exothermic, so lowering the temperature will shift the equilibrium toward the right. Since the reaction uses 3 moles of gas to form 1 mole of gas, increasing the pressure will shift the reaction toward the right. So, low temperature and high pressure will produce the highest yield. Le Chatelier's principle states that when a system at equilibrium is disturbed, the system responds in such a way to minimize the disturbance."