In the reaction CO(g) + 2H2(g) ⇌ CH3OH(g), if the pressure is increased, which d

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

Options:

Correct Answer: To the right

Solution:

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

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

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

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.

Le Chatelier's Principle – When a system at equilibrium is subjected to a change in pressure, the equilibrium will shift in the direction that reduces the pressure, typically towards the side with fewer moles of gas.
Stoichiometry of Gases – Understanding the relationship between the number of moles of gas and the effect of pressure on equilibrium.