Given the equation: PCl3(g) + Cl2(g) ⇌ PCl5(g) kp = 1.05 at 70.5 °C If one...

Given the equation:

PCl3(g) + Cl2(g) ⇌ PCl5(g) kp = 1.05 at 70.5 °C

If one starts with 1,7 atm of PCl5(g), what is the partial pressure of PCl5(g) at equilibrium?

Expert Solution

PCl3(g) + Cl2(g) ⇌ PCl5(g)

I 0 0 1.7

C +x +x -x

E +x +x 1.7-x

Kp = P_PCl5/P_PCl3 P_Cl2

1.05 = 1.7-x/x*x

1.05x^2 = 1.7-x

x = 0.88

P_PCl5 = 1.7-x = 1.7-0.88 = 0.82atm>>>>answer

queen_honey_blossom answered 2 years ago

For the equilibrium PCl5(g) PCl3(g) + Cl2(g), Kc = 4.0 at 228°C. If pure PCl5 is...

For the equilibrium PCl5(g) PCl3(g) + Cl2(g), Kc = 4.0 at 228°C. If pure PCl5 is placed in a 1.00-L container and allowed to come to equilibrium, and the equilibrium concentration of PCl5(g) is 0.26 M, what is the equilibrium concentration of PCl3?

For the exothermic reaction PCl3(g)+Cl2(g)⇌PCl5(g) Kp = 0.140 at a certain temperature. A flask is charged...

For the exothermic reaction PCl3(g)+Cl2(g)⇌PCl5(g) Kp = 0.140 at a certain temperature. A flask is charged with 0.500 atm PCl3 , 0.500 atm Cl2, and 0.300 atm PCl5 at this temperature. What are the equilibrium partial pressures of PCl3 , Cl2, and PCl5, respectively? Express your answers numerically in atmospheres with three digits after the decimal point, separated by commas.

For the exothermic reaction PCl3(g)+Cl2(g)⇌PCl5(g) Kp = 0.160 at a certain temperature. A flask is charged...

For the exothermic reaction PCl3(g)+Cl2(g)⇌PCl5(g) Kp = 0.160 at a certain temperature. A flask is charged with 0.500 atm PCl3 , 0.500 atm Cl2, and 0.300 atm PCl5 at this temperature. What are the equilibrium partial pressures of PCl3, Cl2, and PCl5? How will the following changes affect the mole fraction of chlorine gas, X Cl2, in the equilibrium mixture. X Cl2 increases when __________ X Cl2 decreases when _________ X Cl2 stays the same __________ Fill in the blanks...

For the exothermic reaction PCl3(g)+Cl2(g)?PCl5(g) Kp = 0.200 at a certain temperature. A flask is charged...

For the exothermic reaction PCl3(g)+Cl2(g)?PCl5(g) Kp = 0.200 at a certain temperature. A flask is charged with 0.500 atm PCl3 , 0.500 atm Cl2, and 0.300 atm PCl5 at this temperature. What are the equilibrium partial pressures of PCl3 , Cl2, and PCl5, respectively? Express your answers numerically in atmospheres with three digits after the decimal point, separated by commas.

1.For the reaction, PCl5(g) <-----> PCl3(g) + Cl2(g) Kp = 24.6 at 500 K calculate the equilibrium...

1.For the reaction, PCl5(g) <-----> PCl3(g) + Cl2(g) Kp = 24.6 at 500 K calculate the equilibrium partial pressures of the reactants and products if the initial pressures are PPCl5 = 0.610 atm, PPCl3 = 0.400 atm and PCl2 = 0.000 atm. PPCl5 = PPCl3 = PCl2 = 2. H2O(g) + Cl2O(g) <-----> 2HClO(g) Kc = 0.14 at 298.15 K calculate the equilibrium concentrations of the reactants and products if the initial concentrations are [H2O(g)] = 0.00482 mol L-1, [Cl2O(g)] = 0.00482...

The equilibrium constant K=0.36 for the reaction PCl5 (g)  PCl3 (g) +Cl2 (g). (a) Given...

The equilibrium constant K=0.36 for the reaction PCl5 (g)  PCl3 (g) +Cl2 (g). (a) Given that 2.0 g of PCl5 was initially placed in the reaction chamber of volume 250 cm3, determine the molar concentration in the mixture at equilibrium. (b) What is the percentage of PCl5 decomposed.

Q2. For the exothermic reaction PCl3(g)+Cl2(g) <======>PCl5(gas) Kp=0.160 at a certian temperature. A flask is charged...

Q2. For the exothermic reaction PCl3(g)+Cl2(g) <======>PCl5(gas) Kp=0.160 at a certian temperature. A flask is charged with 0.500 atm PCl3, 0.500 atm Cl2, and .300 atm PCl5 at this temperature. True or False __________The net reaction proceeds to the left to attain equlibrium __________Q is less than k. __________Q is equal to k. __________The reaction is at equlibrium __________Q is greater than k. ___________ No net reaction will occur ____________ The net reaction proceeds to the right to attain equlibrium....

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 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)<--->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.

Question