Into an evacuated 100 L flask at 610 K are placed 4.0 mol of argon (inert) and 5.0 mol of PCl5, which decomposes as PCl5(g) PCl3(g) + Cl2(g). At equilibrium the total pressure of the mixture is 6.0 atm. Calculate Kp for the decomposition. [R = 0.082 L atm K⁻¹ mol⁻¹]

Question

Into an evacuated 100 L flask at 610 K are placed 4.0 mol of argon (inert) and 5.0 mol of PCl5, which decomposes as PCl5(g) <-> PCl3(g) + Cl2(g). At equilibrium the total pressure of the mixture is 6.0 atm. Calculate Kp for the decomposition. [R = 0.082 L atm K⁻¹ mol⁻¹]

Accepted Answer

2.25. From PV = nRT the total equilibrium moles are about 12, so x = 3 mol dissociates; using partial pressures the calculation gives Kp approximately 2.25 atm.

Into an evacuated 100 L flask at 610 K are placed 4.0 mol of argon (inert) and 5.0 mol of PCl5, which decomposes as PCl5(g) <-> PCl3(g) + Cl2(g). At equilibrium the total pressure of the mixture is 6.0 atm. Calculate Kp for the decomposition. [R = 0.082 L atm K⁻¹ mol⁻¹]

Solution

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