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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FREE Expert Solution

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:

Molarity (M)=moles of soluteL of solution



MPCl5=0.250 mol2.50 L

MPCl5 = 0.1


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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.

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What professor is this problem relevant for?

Based on our data, we think this problem is relevant for Professor Orgill's class at UNLV.