A sample of gaseous PCl5 was introduced into an evacuated flask so the pressure of pure PCl5 would be 0.50 atm at 523 K. However, PCl5​ decomposes to gaseous PCl3​ and Cl2, and the equilibrium partial pressure of PCL5 in the flask was found to be 0.16 atm. Calculate the Kp​ for the decomposition reaction PCl5(g) ⇌ PCl3(g) + Cl2(g)

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