For the reaction CO(g) + 2H2(g) ⇌ CH3OH(g), if the pressure is increased, what w

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Question: For the reaction CO(g) + 2H2(g) ⇌ CH3OH(g), if the pressure is increased, what will be the effect on the equilibrium position?

Options:

Correct Answer: Shift to the right

Solution:

Increasing pressure shifts the equilibrium towards the side with fewer moles of gas, which is the right side (1 mole of CH3OH).

For the reaction CO(g) + 2H2(g) ⇌ CH3OH(g), if the pressure is increased, what will be the effect on the equilibrium position?

For the reaction CO(g) + 2H2(g) ⇌ CH3OH(g), if the pressure is increased, what will be the effect on the equilibrium position?

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 are 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 in a reaction favors the side with fewer moles of gas.
Step 7: Conclude that increasing pressure will shift the equilibrium position to the right side (towards CH3OH).

Le Chatelier's Principle – When the pressure of a system at equilibrium is increased, the equilibrium shifts towards the side with fewer moles of gas.
Stoichiometry of Gases – Understanding the relationship between the number of moles of reactants and products in a gas-phase reaction.