A sample of gaseous PCl5 was introduced into an evacuated flask so that the pressure of pure
A sample of gaseous PCl5 was introduced into an evacuated flask so that the pressure of pure PCl5 would be 0.50 atm at 523 K. However, PCl5 decomposes to gaseous PCl3 and Cl2, and the actual pressure in the flask was found to be 0.84 atm. Calculate Kp for the decomposition reaction PCl5(g) ⇌ PCl3(g) + Cl2(g) at 523 K. Also calculate K at this temperature.
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PCl 5 g PCl 3 g Cl 2 g K p To determine K p we must determine the equilibrium partial pr…View the full answer
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