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