In the reaction CO(g) + 2H2(g) ⇌ CH3OH(g), what will happen if the volume of the

₹0.0

Question: In the reaction CO(g) + 2H2(g) ⇌ CH3OH(g), what will happen if the volume of the container is decreased?

Options:

Correct Answer: Shift to the right

Solution:

Decreasing the volume increases the pressure, which shifts the equilibrium to the side with fewer moles of gas, favoring the production of CH3OH.

In the reaction CO(g) + 2H2(g) ⇌ CH3OH(g), what will happen if the volume of the container is decreased?

In the reaction CO(g) + 2H2(g) ⇌ CH3OH(g), what will happen if the volume of the container is decreased?

Step 1: Understand the reaction: CO(g) + 2H2(g) ⇌ CH3OH(g). This means carbon monoxide and hydrogen gas react to form methanol gas.
Step 2: Recognize that gases occupy space in a container. If we decrease the volume of the container, the gases inside are compressed.
Step 3: Know that compressing the gases increases the pressure inside the container.
Step 4: According to Le Chatelier's principle, if the pressure changes, the equilibrium will shift to counteract that change.
Step 5: Identify the number of moles of gas on each side of the reaction: the left side has 3 moles (1 CO + 2 H2) and the right side has 1 mole (1 CH3OH).
Step 6: Since the right side has fewer moles of gas, the equilibrium will shift to the right to reduce the pressure.
Step 7: Therefore, decreasing the volume will favor the production of CH3OH.

Le Chatelier's Principle – When a system at equilibrium is subjected to a change in pressure, temperature, or concentration, the equilibrium will shift to counteract that change.
Mole Count in Gaseous Reactions – Understanding the relationship between the number of moles of gas on each side of a chemical equation is crucial for predicting the direction of equilibrium shifts.