Question

In: Chemistry

Gaseous phosphorus pentachloride decomposes according to the reaction PCl5 (g) ⇌ PCl3 (g) + Cl2 (g)...

Gaseous phosphorus pentachloride decomposes according to the reaction

PCl5 (g) ⇌ PCl3 (g) + Cl2 (g)

The equilibrium system was analyzed at a particular temperature, and the concentration of the substances present were determined to be [PCl5] = 1.1 x10-2 M, [PCl3] = 0.325 M, and [Cl2] = 3.9 x 10-3 M. Calculate the value of K for the reaction.

Solutions

Expert Solution

Step 1: Explanation

Kp is the equilibrium constant calculated from the partial pressures of a reaction equation. It is used to express the relationship between product pressures and reactant pressures

Step 2: Write the balanced the chemical equation

PCl5 (g) <-----> PCl3 (g) + Cl2 (g)

All value at equilibrium is

[PCl5] = 1.1 × 10-2 M

[PCl3] = 0.325 M

[Cl2] = 3.9 × 10-3 M

Step 3: Calculation of Kc

PCl5 (g) <-----> PCl3 (g) + Cl2 (g)

we know, the Kc expression can be written as

Kc = [PCl3] × [ Cl2] / [PCl5]

on substituting the values

=> Kc = [PCl3] × [ Cl2] / [PCl5] = ( 0.325) × ( 3.9 × 10-3 ) / ( 1.1 × 10-2 ) = 0.11523

[ exact value of Kc= 0.1152272727 ]


Related Solutions

Phosphorus pentachloride decomposes according to this equation. PCl5(g) equilibrium reaction arrow PCl3(g) + Cl2(g) An equilibrium...
Phosphorus pentachloride decomposes according to this equation. PCl5(g) equilibrium reaction arrow PCl3(g) + Cl2(g) An equilibrium mixture in a 5.00 L flask at 245°C contains 4.01 g of PCl5, 8.71 g of PCl3, and 2.87 g of Cl2. How many grams of each will be found if the mixture is transferred into a 2.00 L flask at the same temperature? (Enter unrounded values.) I'm pretty sure I did this problem right but my final answers were only 3 decimal places...
Phosphorus pentachloride decomposes according to the chemical equation PCl5(g) - PCl3(g) + Cl2(g) A 0.213 mol...
Phosphorus pentachloride decomposes according to the chemical equation PCl5(g) - PCl3(g) + Cl2(g) A 0.213 mol sample of PCl5(g) is injected into an empty 3.40 L reaction vessel held at 250 degrees C. Calculate the concentrations of PCl5(g) and PCl3(g) at equilibrium.
Phosphorus pentachloride decomposes according to the chemical equation: PCl5(g) forward and reverse arrows PCl3(g) + Cl2(g)                      
Phosphorus pentachloride decomposes according to the chemical equation: PCl5(g) forward and reverse arrows PCl3(g) + Cl2(g)                          Kc=1.80M at 250 degrees celcius. A 0.293 mol sample of PCl5(g) is injected into an empty 4.35L reaction vessel held at 250 degrees celcius. Calculate the concentrations of PCl5(g) and PCl3(g) at equilibrium.
Phosphorus pentachloride decomposes according to the chemical equation PCl5 <-----> PCl3 + Cl2 Kc=1.80 at 250...
Phosphorus pentachloride decomposes according to the chemical equation PCl5 <-----> PCl3 + Cl2 Kc=1.80 at 250 °C A 0.135 mol sample of PCl5(g) is injected into an empty 2.15 L reaction vessel held at 250 °C. Calculate the concentrations of PCl5(g) and PCl3(g) at equilibrium.
Phosphorus pentachloride decomposes at higher temperatures. PCl5(g) ⇄ PCl3(g) + Cl2(g) An equilibrium mixture at some...
Phosphorus pentachloride decomposes at higher temperatures. PCl5(g) ⇄ PCl3(g) + Cl2(g) An equilibrium mixture at some temperature consists of 3.03 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 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 according to the chemical equation PCL5(g)<--->PCl3(g)+Cl2(g). Kc=1.80 at 250 C. A 0.244 mol...
Phosphorus pentachloride decomposes according to the chemical equation PCL5(g)<--->PCl3(g)+Cl2(g). Kc=1.80 at 250 C. A 0.244 mol sample of PCl5(g) is injected into an empty 2.80 L reaction vessel held at 250 Celsius. 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 PCl 5 ( g...
Phosphorus pentachloride decomposes according to the chemical equation PCl5(g)↽−−⇀PCl3(g)+Cl2(g)?c=1.80 at 250 ∘C PCl 5 ( g ) ↽ − − ⇀ PCl 3 ( g ) + Cl 2 ( g ) K c = 1.80 at 250 ∘ C A 0.3295 mol 0.3295 mol sample of PCl5(g) PCl 5 ( g ) is injected into an empty 3.80 L 3.80 L reaction vessel held at 250 ∘C. 250 ∘ C. Calculate the concentrations of PCl5(g) PCl 5 ( g...
Phosphorus pentachloride is formed when phosphorus trichloride and chlorine react. PCl3(g) + Cl2(g) ⇌ PCl5(g) The...
Phosphorus pentachloride is formed when phosphorus trichloride and chlorine react. PCl3(g) + Cl2(g) ⇌ PCl5(g) The equilibrium constant for the reaction is KC = 37.8 at 110 °C. If 0.887 mol of phosphorus trichloride is added to 0.550 mol of chlorine in a 1.02-L reaction vessel at this temperature, what is the equilibrium concentration (in mol/L) of phosphorus pentachloride? Report your answer to THREE significant figures.
Phosphorus pentachloride decomposes according to the chemical equation. PCl5(g) ightleftharpoons PCI3(g) + Cl2(g) Kc = 1.80...
Phosphorus pentachloride decomposes according to the chemical equation. PCl5(g) ightleftharpoons PCI3(g) + Cl2(g) Kc = 1.80 at 250 �C A 0.318 mol sample of PCl5(g) is injected into an empty 3.35 L reaction vessel held at 250 �C. Calculate the concentrations of PCl5(g) and PCl3(g) at equilibrium.
ADVERTISEMENT
ADVERTISEMENT
ADVERTISEMENT