?Phosphorus trichloride gas and chlorine gas react to form phosphorus pentachloride gas

Chapter 15, Problem 15.34

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Phosphorus trichloride gas and chlorine gas react to form phosphorus pentachloride gas: \(\mathrm{PCl}_{3}(g)+\mathrm{Cl}_{2}(g) \rightleftharpoons \mathrm{PCl}_{5}(\mathrm{~g})\). A 7.5-L gas vessel is charged with a mixture of \(\mathrm{PCl}_{3}(g)\) and \(\mathrm{Cl}_{2}(g)\), which is allowed to equilibrate at 450 K. At equilibrium the partial pressures of the three gases are \(P_{\mathrm{PCl}_{3}}=0.124 \mathrm{~atm}, P_{\mathrm{Cl}_{2}}=0.157 \mathrm{~atm}\), and \(P_{\mathrm{PCl}_{5}}=1.30 \mathrm{~atm}\).

(a) What is the value of \(K_{p}\) at this temperature?

(b) Does the equilibrium favor reactants or products?

(c) Calculate \(K_{c}\) for this reaction at 450 K.

Text Transcription:

PCl3(g) + Cl_2(g) \rightleftharpoons PCl_5(g)

PCl_3(g)

Cl_2(g)

P_PCl3 = 0.124 atm, P_Cl2 = 0.157 atm

P_PCl5 = 1.30 atm

K_p

K_c