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)
An analysis of a chemical reaction system at 340 °C shows that PCl5, PCl3, and Cl2...
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.
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 0.314 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.
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.
Consider the reaction. PCl5(g)↽−−⇀PCl3(g)+Cl2(g)?c=0.0420 The concentrations of the products at equilibrium are [PCl3]=0.120 M and [Cl2]=0.150 M. What is the concentration of the reactant, PCl5, at equilibrium?
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.
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)
Phosphorus pentachloride decomposes according to the chemical equation PCl5(g)↽−−⇀PCl3(g)+Cl2(g)?c=1.80 at 250° C A 0.162 mol sample of PCl5(g) is injected into an empty 2.65 L reaction vessel held at 250° C. Calculate the concentrations of PCl5(g) and PCl3(g) at equilibrium. [PCl5]= ? M
Phosphorus pentachloride decomposes according to the chemical equation PCl5(g)↽−−⇀PCl3(g)+Cl2(g)?c=1.80 at 250° C A 0.268 mol sample of PCl5(g) is injected into an empty 3.70 L reaction vessel held at 250° C. Calculate the concentrations of PCl5(g) and PCl3(g) at equilibrium.