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?

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

PCl5(g) ⇌ PCl3(g) + Cl2(g)

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

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