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.

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

FREE Expert Solution

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

We’re given the following equilibrium reaction:

PCl_5(g) ⇌ PCl_3(g) + Cl_2(g);    K_c = 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:

$\boxed{\mathbf{Molarity}\mathbf{ }\mathbf{\left(}\mathbf{M}\mathbf{\right)}\mathbf{=}\frac{\mathbf{moles}\mathbf{ }\mathbf{of}\mathbf{ }\mathbf{solute}}{\mathbf{L}\mathbf{ }\mathbf{of}\mathbf{ }\mathbf{solution}}}$

${\mathbf{M}}_{{\mathbf{PCl}}_{\mathbf{5}}}\mathbf{=}\frac{\mathbf{0}\mathbf{.}\mathbf{250}\mathbf{ }\mathbf{mol}}{\mathbf{2}\mathbf{.}\mathbf{50}\mathbf{ }\mathbf{L}}$

M_PCl5 = 0.1