For the reaction: 2A(g) + B(g) ⇌ 3C(g), if the volume of the container is decrea

For the reaction: 2A(g) + B(g) ⇌ 3C(g), if the volume of the container is decreased, what will be the effect on the equilibrium? (2022)

For the reaction: 2A(g) + B(g) ⇌ 3C(g), if the volume of the container is decreased, what will be the effect on the equilibrium? (2022)

Step 1: Understand that the reaction involves gases: 2A(g) + B(g) ⇌ 3C(g).
Step 2: Identify the number of gas moles on each side of the reaction.
Step 3: Count the moles: On the left side (reactants), there are 2 moles of A and 1 mole of B, totaling 3 moles. On the right side (products), there are 3 moles of C.
Step 4: Recognize that decreasing the volume of the container increases the pressure of the gases inside.
Step 5: Apply Le Chatelier's principle, which states that if a system at equilibrium is disturbed, it will shift to counteract the disturbance.
Step 6: Since increasing pressure favors the side with fewer moles of gas, determine which side has fewer moles.
Step 7: Compare the moles: The left side has 3 moles and the right side has 3 moles, so they are equal.
Step 8: Since both sides have the same number of moles, the equilibrium will not shift significantly in either direction.

Le Chatelier's Principle – This principle states that if a system at equilibrium is subjected to a change in conditions (such as pressure or volume), the equilibrium will shift in a direction that counteracts the change.
Mole Ratio in Gaseous Reactions – Understanding the relationship between the number of moles of gas on each side of the equilibrium equation is crucial for predicting the direction of the shift.