When phosphorus pentachloride, PCl₅, is heated at a constant pressure of exactly 1 bar to a temperature of 1400 K, the amount of phosphorus pentachloride decreases by 20.7% because of dissociation to phosphorus trichloride, PCl₃, and chlorine, Cl₂. Determine the equilibrium constant at this temperature.

Question

Quizplus · Accepted Answer

The equilibrium constant (K) can be calculated using the degree of dissociation and the initial concentration of PCl5. Given that 20.7% of PCl5 dissociates, we can set up an equilibrium expression involving the concentrations of PCl5, PCl3, and Cl2 at equilibrium. The calculation involves using the stoichiometry of the reaction and the given percentage of dissociation to find the equilibrium concentrations of the reactants and products, and then applying these to the formula for the equilibrium constant. The correct answer involves detailed calculations that account for the change in concentration due to the dissociation and the stoichiometry of the reaction.

When Phosphorus Pentachloride, PCl5, Is Heated at a Constant Pressure

When Phosphorus Pentachloride, PCl₅, Is Heated at a Constant Pressure