In the reaction CO(g) + 2H2(g) ⇌ CH3OH(g), if the pressure is increased, which direction will the equilibrium shift?

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Q: In the reaction CO(g) + 2H2(g) ⇌ CH3OH(g), if the pressure is increased, which direction will the equilibrium shift?

Solution: Increasing pressure shifts the equilibrium towards the side with fewer moles of gas, which is the right side in this case.

Steps: 7

Step 1: Identify the reaction: CO(g) + 2H2(g) ⇌ CH3OH(g).
Step 2: Count the number of gas moles on each side of the reaction.
Step 3: On the left side (reactants), there is 1 mole of CO and 2 moles of H2, totaling 3 moles of gas.
Step 4: On the right side (products), there is 1 mole of CH3OH.
Step 5: Compare the total moles of gas: 3 moles on the left vs. 1 mole on the right.
Step 6: Understand that increasing pressure favors the side with fewer moles of gas.
Step 7: Since the right side has fewer moles (1 mole), the equilibrium will shift to the right.