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) + 2 H2 (g)Two arrows stacked on top of each other. The top arrow points to the right. The bottom arrow points to the left.
CO (g) + 2 H2 (g) -- CH3OH (g) delta H = -90.7 kj/mol

Question

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) + 2 H2 (g)Two arrows stacked on top of each other. The top arrow points to the right. The bottom arrow points to the left. 
CO (g) + 2 H2 (g) --> CH3OH (g) delta H = -90.7 kj/mol

anonymous · Answer

@Abmon98 :) :)

abmon98 · Answer

Delta H is negative so decreasing the temperature will decrease the rate and the rate too.
increasing the pressure where there are fewer no of moles will allow equilbrium to shift towards the products and increase the rate