🤓 Based on our data, we think this question is relevant for Professor Bwambok's class at CSUSM.

Solution: Phosphorus pentachloride decomposes to phosphorus trichloride at high temperatures according to the equation: PCl5(g) ⇌ PCl3(g) + Cl2(g) At 250° 0.125 M PCl5 is added to the flask. If Kc = 1.80, what are the equilibrium concentrations of each gas?

Problem

Phosphorus pentachloride decomposes to phosphorus trichloride at high temperatures according to the equation:

PCl5(g) ⇌ PCl3(g) + Cl2(g)

At 250° 0.125 M PCl5 is added to the flask. If Kc = 1.80, what are the equilibrium concentrations of each gas?