Phosphorus pentachloride decomposes at higher temperatures.
PCl5(g) ⇄ PCl3(g) + Cl2(g)
An equilibrium mixture at some temperature consists of
5.93 g PCl5, 208.23 g/mol
4.86 g PCl3, 137.33 g/mol
3.59 g Cl2, 70.91 g/mol
in a 1.00-L flask.
If you add 1.31 g of Cl2, how will the equilibrium be affected and what will the concentration of PCl5 be when equilibrium is reestablished?
_shift left
_shift right
_no shift will occur
[PCl5] =? mol/L
Phosphorus pentachloride decomposes at higher temperatures. PCl5(g) ⇄ PCl3(g) + Cl2(g) An equilibrium mixture at some...
Phosphorus pentachloride decomposes at high temperatures. PCl5(g) ⇆ PCl3(g) + Cl2(g) An equilibrium mixture at some temperature consists of 3.51 g PCl5 4.86 g PCl3 3.59 g Cl2 in a 1.00-L flask. If you add 1.31 g of Cl2, how will the equilibrium be affected? (Shift left, shift right, or no change) What is the new equilibrium of PCl5?
Phosphorus pentachloride decomposes to phosphorus trichloride at high temperatures according to the equation: PCl5(g) ⇌ PCl3(g) + Cl2(g) At 250° 0.250 M PCl 5 is added to the flask. If K c = 1.80, what are the equilibrium concentrations of each gas? [PCl5] = 2.27 M, [PCl3] = 2.02 M, and [Cl2] = 2.02 M [PCl5] = 1.80 M, [PCl3] = 1.80 M, and [Cl2] = 1.80 M [PCl5] = 0.0280 M, [PCl3] = 0.222 M, and [Cl2] = 0.222 M...
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) 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 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.
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)?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.
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 ∘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 is formed when phosphorus trichloride and chlorine react. PCl3(g) + Cl2(g) ⇌ PCl5(g) The equilibrium constant for the reaction is KC = 38.0 at 233 °C. If 0.510 mol of phosphorus trichloride is added to 0.238 mol of chlorine in a 1.11-L reaction vessel at this temperature, what is the equilibrium concentration (in mol/L) of phosphorus pentachloride? Report your answer to THREE significant figures.