Question

Phosphorus pentachloride decomposes according to the chemical equation PCl5(g) ? PCl3(g) + Cl2(g) Kc = 1.80 at 250 °C A 0.2815 mol sample of PCl5(g) is injected into an empty 3.60 L reaction vessel held at 250 °C. Calculate the concentration of PCl3 at equilibrium. R = 8.3144598 J mol^-1 K^-1; PV = nRT; Kp = Kc(RT)^?n x = (-b ± ?(b^2 - 4ac)) / 2a when ax^2 + bx + c = 0

          Phosphorus pentachloride decomposes according to the chemical equation

PCl5(g) ? PCl3(g) + Cl2(g)   Kc = 1.80 at 250 °C

A 0.2815 mol sample of PCl5(g) is injected into an empty 3.60 L reaction vessel held at 250 °C.
Calculate the concentration of PCl3 at equilibrium.

R = 8.3144598 J mol^-1 K^-1; PV = nRT; Kp = Kc(RT)^?n  x = (-b ± ?(b^2 - 4ac)) / 2a
when ax^2 + bx + c = 0

Phosphorus pentachloride decomposes according to the chemical equation

PCl5(g) ? PCl3(g) + Cl2(g) Kc = 1.80 at 250 °C

A 0.2815 mol sample of PCl5(g) is injected into an empty 3.60 L reaction vessel held at 250 °C.
Calculate the concentration of PCl3 at equilibrium.

R = 8.3144598 J mol^-1 K^-1; PV = nRT; Kp = Kc(RT)^?n x = (-b ± ?(b^2 - 4ac)) / 2a
when ax^2 + bx + c = 0

Added by Tiffany C.

Chemistry: Structure and Properties

Nivaldo Tro 2nd Edition

Instant Answer

Solved by Expert Sri K

03/14/2023

Step 1

We can do this using the formula: Initial concentration of PCl5 = moles of PCl5 / volume of the container Initial concentration of PCl5 = 0.2815 mol / 3.60 L = 0.078194 mol/L Now, let's set up an ICE table (Initial, Change, Equilibrium) to find the equilibrium Show more…

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Phosphorus pentachloride decomposes according to the chemical equation PCl5(g) ⇌ PCl3(g) + Cl2(g) Kc = 1.80 at 250 °C A 0.2815 mol sample of PCl5(g) is injected into an empty 3.60 L reaction vessel held at 250 °C. Calculate the concentration of PCl3 at equilibrium. R = 8.3144598 J mol^-1 K^-1; PV = nRT; Kp = Kc(RT)^Δn x = (-b ± √(b^2 - 4ac)) / 2a when ax^2 + bx + c = 0