# Problem: Phosphorus pentachloride decomposes according to the chemical equation.PCl5(g) ⇌ PCI3(g) + Cl2(g)             Kc = 1.80 at 250 °CA 0.250 mol sample of PCl5(g) is injected into an empty 2.50 L reaction vessel held at 250 °C. Calculate the concentrations of PCl5(g) and PCl3(g) at equilibrium.

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We are asked to calculate the equilibrium concentration of PCl5(g) and PCl3(g)

We’re given the following equilibrium reaction:

PCl5(g)  PCl3(g) + Cl2(g);    Kc = 1.80 at 250°C

We know that the initial amount of PCl5 is 0.250 mol. In a 2.50 L container, the concentration of each is:

MPCl5 = 0.1 ###### Problem Details

Phosphorus pentachloride decomposes according to the chemical equation.

PCl5(g) ⇌ PCI3(g) + Cl2(g)             Kc = 1.80 at 250 °C

A 0.250 mol sample of PCl5(g) is injected into an empty 2.50 L reaction vessel held at 250 °C. Calculate the concentrations of PCl5(g) and PCl3(g) at equilibrium.