For the reaction A(g) + B(g) ⇌ C(g), if the pressure is decreased, what will hap

For the reaction A(g) + B(g) ⇌ C(g), if the pressure is decreased, what will happen to the equilibrium?

For the reaction A(g) + B(g) ⇌ C(g), if the pressure is decreased, what will happen to the equilibrium?

Step 1: Identify the reaction: A(g) + B(g) ⇌ C(g).
Step 2: Count the number of gas moles on each side of the reaction.
Step 3: On the left side (reactants), there are 2 moles of gas (1 mole of A and 1 mole of B).
Step 4: On the right side (products), there is 1 mole of gas (1 mole of C).
Step 5: Determine which side has more moles of gas. The left side has 2 moles, and the right side has 1 mole.
Step 6: Understand that decreasing the pressure will shift the equilibrium towards the side with more moles of gas.
Step 7: Since the left side has more moles of gas, the equilibrium will shift to the left side (A and B) when pressure is decreased.

Le Chatelier's Principle – This principle states that if an external change is applied to a system at equilibrium, the system will adjust to counteract that change and restore a new equilibrium.
Gas Molar Volume and Pressure – Understanding how changes in pressure affect the position of equilibrium based on the number of moles of gas on each side of the reaction.