For the reaction below, describe the temperature and pressure conditions that would produce the highest yield for the forward reaction. explain your answer in terms of le châtelier’s principle. co(g) + 2h2(g) two arrows stacked on top of each other. the top arrow points to the right. the bottom arrow points to the left. ch3oh(g) deltah = -90.7 kj/mol

Le Chatelier's principle suggests that equilibrium will move towards the direction that will counteract the change applied to a system. In this case, wherein the reaction is exothermic, the forward reaction will be favored by decreasing the temperature conditions. The reaction will tend to move forward to produce more heat to counteract the decrease in temperature. Also, to increase the yield, the pressure must be increased. This is because the reactants have more moles of gases and by increasing the pressure, the reaction will tend to move forward as to consume the reactants.