For the reaction, PCl5 (g) <--> PCl3 (g) + Cl2 (g), Kc=33.3 at 760.0 C. In a container at equilibrium, there are 1.29 x 10-3 mol/L of PCl5 and 1.87 x 10-1 mol/L of Cl2.
Calculate the [PCl3] in the container.
Kc = [Cl2][PCl3] / [PCl5]
[Cl2] = 1.87 x 10-1 M
[PCl5] = 1.29 x 10-3 M
[PCl3] = ?
Kc = 33.3
33.3 = [0.187][PCl3] / [0.00129]
0.0429 = [PCl3] x 0.187
[PCl3] = 0.229 M = 2.29 x 10-1 M
For the reaction, PCl5 (g) <--> PCl3 (g) + Cl2 (g), Kc=33.3 at 760.0 C. In...
The equilibrium constant Kc for the reaction: PCl3(g) + Cl2(g) PCl5(g) is 490 at 230°C. If 0.70 mol of PCl3 is added to 0.70 mol of Cl2 in a 1.00-L reaction vessel at 230°C, what is the concentration of PCl3 when equilibrium has been established? (show work)
The equilibrium constant, Kc, for the following reaction is 1.20×10-2 at 500K. PCl5(g) to PCl3(g) + Cl2(g) If an equilibrium mixture of the three gases in a 15.2 L container at 500K contains 0.214 mol of PCl5(g) and 0.202 mol of PCl3, the equilibrium concentration of Cl2 is ___M.
Phosphorus pentachloride decomposes according to the chemical equation PCl5(g)↽−−⇀PCl3(g)+Cl2(g)?c=1.80 at 250 ∘CPCl5(g)↽−−⇀PCl3(g)+Cl2(g)Kc=1.80 at 250 ∘C A 0.252 mol0.252 mol sample of PCl5(g)PCl5(g) is injected into an empty 3.40 L3.40 L reaction vessel held at 250 ∘C.250 ∘C. Calculate the concentrations of PCl5(g)PCl5(g) and PCl3(g)PCl3(g) at equilibrium.
Phosphorus pentachloride decomposes according to the chemical equation PCl5(g) <=> PCl3 (g) + Cl2 (g) Kc = 1.80 at 250 C A 0.3391 mol sample of PCl5 (g) is injected into an empty 3.60 L reaction vessel held at 250 ∘ C. Calculate the concentrations of PCl5 ( g ) and PCl3 ( g ) at equilibrium. [PCl5] = __________M. [PCl3]=___________M.
For the equilibrium PCl5(g) PCl3(g) + Cl2(g), Kc = 2.0 × 101 at 240°C. If pure PCl5 is placed in a 1.00-L container and allowed to come to equilibrium, and the equilibrium concentration of PCl3(g) is 0.27 M, what is the equilibrium concentration of PCl5(g)?
Phosphorus pentachloride decomposes according to the chemical equation PCl5(g) <---> PCl3(g) + Cl2(g) Kc= 1.80 at 250°C A 0.314 mol sample of PCl5(g) is injected into an empty 3.45 L reaction vessel held at 250 °C. Calculate the concentrations of PCl5(g) and PCl3(g) at equilibrium. [PCl5]= ? M [PCl3]= ? M
Phosphorus pentachloride decomposes according to the chemical equation PCl5(g)−⇀↽−PCl3(g)+Cl2(g)Kc=1.80 at 250 ∘C A 0.3907 mol sample of PCl5(g) is injected into an empty 3.95 L reaction vessel held at 250 ∘C. Calculate the concentrations of PCl5(g) and PCl3(g) at equilibrium.
An analysis of a chemical reaction system at 340 °C shows that PCl5, PCl3, and Cl2 are present at equal concentrations of 0.120 mol/L. Determine the equilibrium concentrations (in M) of PCl5, PCl3 and Cl2 at 340 °C, given that Kc = 0.800. Show all calculations and report your answer to the correct number of sig figs. PCl5(g) ⟺ PCl3(g) + Cl2(g)
For this reaction: PCl3(g) + Cl2(g) <==> PCl5(g) Kc = 26 at 275K Initially, you have 0.10 mol PCl3, 0.10 mol Cl2, and 0.010mol PCl5 all in a 6.40L flask. Assuming ideal gas conditions, calculate: Kp, Qp, and state which direction the reaction will shift.
Phosphorus pentachloride decomposes according to the chemical equation PCl5(g)−⇀↽−PCl3(g)+Cl2(g) Kc=1.80 at 250 A 0.1414 mol sample of PCl5(g) is injected into an empty 2.00 L reaction vessel held at 250 ∘C. Calculate the concentrations of PCl5(g) and PCl3(g) at equilibrium.