Question

The reaction PCl3(g)+Cl2(g)???PCl5(g)

has Kp=0.0870 at 300 ?C. A flask is charged with 0.50atmPCl3, 0.50atmCl2, and 0.20atmPCl5 at this temperature.

1.Calculate the equilibrium partial pressures of PCl3.Express your answer using two significant figures.

2.Calculate the equilibrium partial pressures of Cl2. .Express your answer using two significant figures.

3.Calculate the equilibrium partial pressures of PCl5.Express your answer using two significant figures.

Answer 1

Just study the thing don't expect others to just answer the homework for you

Step-by-step explanation:

If you truly are a good student then you should have asked your teacher in person or through email instead of asking on here. Not trying to be mean but you also have to understand that people on here have a life. :)

Answer 2

1) p(PCl3) = 0.66 atm

2) p(Cl2) = 0.66 atm

3) p(PCl5) = 0.038 atm

Step-by-step explanation:

Step 1: Data given

Kp = 0.0870

Temperature = 300 °C

Pressure of PCl3 = 0.50 atm

Pressure of Cl2 = 0.50 atm

Pressure of PCl5 = 0.20 atm

Step 2: The balanced equation

PCl3(g) + Cl2(g) ⇆ PCl5(g)

Step 3: The pressure at equilibrium

p = [PCl5] / [PCl3] [Cl2]

Q = [0.20] / [0.50] [0.50] = 0.8

Q >> Kp

The reaction will shift to the left to decrease the numerator PCl5

p(PCl3) = (0.50 + x) atm

p(Cl2) = (0.50 + x) atm

p(PCl5) = (0.20 - x) atm

Kp = (pPCl5) / (pPCl3) (pCl2)

0.0870 = (0.20-x) / (0.50+x) (0.50+x)

0.0870 (0.50+x)(0.50+x) = (0.20-x)

0.0870 (0.25 + 1.0x + x²)= (0.20-x)

0.02175 + 0.087x + 0.087x² = 0.2 -x

0.087x² + 1.087x -0.17825 = 0

x= 0.1619

Step 4: The equilibrium partial pressures

p(PCl3) = (0.50 + x) atm = 0.50 + 0.1619 = 0.6619 atm

p(Cl2) = (0.50 + x) atm = 0.50 + 0.1619 = 0.6619 atm

p(PCl5) = (0.20 - x) atm = 0.20 - 0.1619 = 0.0381 atm