For the equilibrium reaction A(g) + B(g) ⇌ C(g), if the reaction is endothermic,

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Question: For the equilibrium reaction A(g) + B(g) ⇌ C(g), if the reaction is endothermic, what is the effect of increasing pressure?

Options:

Correct Answer: Shifts equilibrium to the left

Solution:

Increasing pressure favors the side with fewer moles of gas. If A and B have more moles than C, the equilibrium will shift to the left.

For the equilibrium reaction A(g) + B(g) ⇌ C(g), if the reaction is endothermic, what is the effect of increasing pressure?

For the equilibrium reaction A(g) + B(g) ⇌ C(g), if the reaction is endothermic, what is the effect of increasing pressure?

Step 1: Identify the reaction: A(g) + B(g) ⇌ C(g).
Step 2: Determine the number of moles of gas on each side of the reaction.
Step 3: Count the moles: On the left side (reactants), there are 2 moles (1 mole of A and 1 mole of B). On the right side (products), there is 1 mole (1 mole of C).
Step 4: Understand the effect of pressure: Increasing pressure in a gas reaction shifts the equilibrium towards the side with fewer moles of gas.
Step 5: Since the left side has 2 moles and the right side has 1 mole, increasing pressure will favor the right side (C).
Step 6: Conclude that increasing pressure will shift the equilibrium to the right, producing more C.

Le Chatelier's Principle – This principle states that if a system at equilibrium is subjected to a change in pressure, temperature, or concentration, the system will adjust to counteract that change and restore a new equilibrium.
Endothermic Reactions – In endothermic reactions, heat is absorbed, and the reaction shifts to favor the products when temperature is increased.
Mole Count in Gaseous Reactions – The effect of pressure changes on equilibrium depends on the number of moles of gas on each side of the reaction.