Consider the following reaction, equilibrium concentrations, and equilibrium constant at a particular temperature. Determine the equilibrium concentration of H₂O(g) . C₂H₄(g) + H₂O(g) ⇌ C₂H₅OH(g) K_c = 9.0 × 10³M^-1
[C₂H₄]_eq = 0.015 mol L^-1 [C₂H₅OH]_eq = 1.69 mol L^-1

Question

Quizplus · Accepted Answer

From the given equilibrium equation and equilibrium concentrations, we can set up an ICE table: C₂H₄(g) + H₂O(g) ⇌ C₂H₅OH(g) I: 0.015 mol, 0.015 mol, 0 mol C: -x, -x, +x E: 0.015 - x, 0.015 - x, x where x is the change in concentration at equilibrium. Using the equilibrium constant expression, we have: K_c = [C₂H₅OH]/([C₂H₄][H₂O]) 9.0 × 10³M^-1 = (1.69 - x)/([0.015 - x][x]) Assuming that x is much smaller than 0.015, we can simplify the expression to: 9.0 × 10³M^-1 = (1.69)/([0.015][x]) Solving for x, we get x = 0.013 mol/L. Therefore, the equilibrium concentration of H₂O is 0.013 mol/L, which corresponds to answer choice E.

Consider the Following Reaction, Equilibrium Concentrations, and Equilibrium Constant at a Particular