Warren Ford
05/21/2024 · Junior High School
Phosphorus pentachloride can dissociate into phosphorus trichloride and chlorine: \[ \mathrm{PCl}_{5}(\mathrm{~g}) \rightleftharpoons \mathrm{PCl}_{3}(\mathrm{~g})+\mathrm{Cl}_{2}(\mathrm{~g}) \] At \( 250^{\circ} \mathrm{C} \), the equilibrium constant in terms of pressures, Kp , for this dissociation reaction is 2.15 . (a) If 19.66 g of phosphorus pentachloride is placed in a \( 15.21-\mathrm{L} \) vessel and heated to \( 250^{\circ} \mathrm{C} \), what is the partial pressure of phosphorus trichloride when equilibrium is attained? (b) What fraction of phosphorus pentachloride is dissociated at equilibrium?
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(a) The partial pressure of phosphorus trichloride at equilibrium is approximately 0.267 atm.
(b) Approximately 88.1% of phosphorus pentachloride is dissociated at equilibrium.
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