Effect of Increasing Concentration of C on Equilibrium Concentration of B

To analyze the effect of increasing the concentration of C on the equilibrium concentration of B in the given system A(s) + 2B(g) ⇌ 3C(g), we need to consider Le Chatelier's principle. According to this principle, a system at equilibrium will adjust to counteract any changes imposed upon it.

Le Chatelier's Principle:
If a system at equilibrium is subjected to a change in temperature, pressure, or concentration, the system will respond in a way that tends to counteract the change and restore the equilibrium.

Increasing Concentration of C:
When the concentration of C is increased by a factor of 2, it means that the concentration of C doubles. This change disrupts the equilibrium of the system and causes a shift to re-establish equilibrium.

Effect on Equilibrium Concentration of B:
Since C is a product in the forward reaction, increasing its concentration will shift the equilibrium to the left according to Le Chatelier's principle. As a result, the concentration of B will decrease.

The stoichiometric coefficient of B in the balanced equation is 2. This means that for every 2 moles of B consumed, 3 moles of C are produced. Therefore, the decrease in the concentration of B will be directly proportional to the increase in the concentration of C.

Mathematical Relationship:
Let's assume the initial concentration of B is [B]₀ and the equilibrium concentration of B is [B]eq. Similarly, the initial concentration of C is [C]₀ and the equilibrium concentration of C is [C]eq.

Since the concentration of C is doubled, we can express the new concentration of C as 2[C]₀.

The decrease in the concentration of B can be calculated using the ratio of stoichiometric coefficients:

Change in [B]eq / Change in [C]eq = Stoichiometric coefficient of B / Stoichiometric coefficient of C

Δ[B]eq / (2[C]₀ - [C]₀) = 2 / 3

Δ[B]eq / [C]₀ = 2 / 3

Δ[B]eq = (2 / 3) * [C]₀

Therefore, increasing the concentration of C by a factor of 2 will cause the equilibrium concentration of B to decrease by (2 / 3) times the initial concentration of C.

Explanation:
By doubling the concentration of C, the equilibrium shifts to the left to consume excess C and restore equilibrium. As a result, the concentration of B decreases by a factor of (2 / 3) times the initial concentration of C. This relationship is based on the stoichiometry of the balanced equation and can be derived using Le Chatelier's principle.

It is A(s)<->B(g)+C(g)