The equilibrium concentration of X, Y and YX2 are 4, 2 and 2 moles respectively for the equilibrium — Chemical Equilibrium Chemistry Question

💡 Solution & Explanation

# Solution: Finding Kc for the Equilibrium 2X + Y ⇌ YX₂ **Step 1: Write the equilibrium expression** For the reaction: $2X + Y \rightleftharpoons YX_2$ $$K_c = \frac{[YX_2]}{[X]^2[Y]}$$ **Step 2: Identify equilibrium concentrations** From the problem: - $[X]_{eq} = 4$ mol - $[Y]_{eq} = 2$ mol - $[YX_2]_{eq} = 2$ mol **Step 3: Substitute into the expression** $$K_c = \frac{2}{(4)^2 \times 2}$$ $$K_c = \frac{2}{16 \times 2} = \frac{2}{32}$$ $$K_c = \frac{1}{16} = 0.0625$$ **Answer: B** (assuming option B = 1/16 or 0.0625) The equilibrium constant depends only on equilibrium concentrations raised to their stoichiometric coefficients, making this a straightforward substitution problem.