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Ch.15 - Chemical Equilibrium
All textbooksMcMurry 8th EditionCh.15 - Chemical EquilibriumProblem 98
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Chapter 15, Problem 98

At 700 K, Kp = 0.140 for the reaction ClF₃(g) ⇌ ClF(g) + F₂(g). Calculate the equilibrium partial pressures of ClF₃, ClF, and F₂ if only ClF₃ is present initially, at a partial pressure of 1.47 atm.

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Identify the initial conditions: Only ClF₃ is present initially with a partial pressure of 1.47 atm, and the partial pressures of ClF and F₂ are 0 atm.
Write the expression for the equilibrium constant Kp for the reaction: Kp = (P_{ClF} * P_{F2}) / P_{ClF3}.
Define the change in partial pressures: Let the change in partial pressure of ClF₃ be -x atm, then the change for ClF and F₂ will be +x atm each, due to the stoichiometry of the reaction.
Express the equilibrium partial pressures in terms of x: P_{ClF3} = 1.47 - x, P_{ClF} = x, and P_{F2} = x.
Substitute the equilibrium partial pressures into the Kp expression and solve for x: 0.140 = (x * x) / (1.47 - x).
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