What is the effect of decreasing the volume of the container on the equilibrium

What is the effect of decreasing the volume of the container on the equilibrium of the reaction 2N2O(g) ⇌ 2N2(g) + O2(g)?

What is the effect of decreasing the volume of the container on the equilibrium of the reaction 2N2O(g) ⇌ 2N2(g) + O2(g)?

Step 1: Understand that the reaction involves gases: 2N2O(g) ⇌ 2N2(g) + O2(g).
Step 2: Identify the number of gas moles on each side of the reaction.
Step 3: Count the moles: The left side (2N2O) has 2 moles, and the right side (2N2 + O2) has 3 moles.
Step 4: Know that decreasing the volume of the container increases the pressure of the gases inside.
Step 5: Remember that according to Le Chatelier's principle, the equilibrium will shift to reduce the pressure.
Step 6: Since the left side has fewer moles (2 moles) compared to the right side (3 moles), the equilibrium will shift to the left.

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