Question

Partial Pressure:

a) Calculate the partial pressure of oxygen and hydrogen in a mixture of 35.0 g of oxygen gas and 11.5 g of hydrogen gas in a 2.0 L container at 35F?

b) Within a balloon, there are 3 types of gasses. The first gas is 6 moles in amount, the 2nd is 4 moles and the 3rd is 3.5. If a total pressure of 10 atm was felt by the balloon and labeled the 1st, 2nd, 3rd gas X, Y, Z, what is the partial pressure of each gas?

Pls show the steps. Thanks!

Answer 1

moles of O2 = 35 / 32 = 1.09

moles of H2 = 11.5 / 2 = 5.75

total moles = 6.84

mole fraction of O2 = 1.09 / 6.84 = 0.159

mole fraction of H2 = 0.841

V = 2.0 L

T = 35 F = 274.8 K

P V = n R T

P x 2.0 = 6.84 x 0.0821 x 274.8

P = 77.16 atm

partial pressure = mole fraction x total pressure

partial pressure of O2 = 0.159 x 77.16

                                   = 12.27 atm

partial pressure of H2 = 0.841 x 77.16

                                    = 64.89 atm

b)

total moles = 6 + 4 + 3.5 = 13.5

mole fractions of each :

X = 6 / 13 .5 = 0.444

Y = 4/ 13.5 = 0.296

Z = 3.5 /13.5 = 0.259

partial pressure = mole fraction x total pressure

Xp   = 0.444 x 10 = 4.44 atm

Yp = 0.296 x 10 = 2.96 atm

Zp = 0.259 x 10 = 2.59 atm