Question

A mixture of hydrogen gas and oxygen gas exerts a total pressure of
3.0 atm on the walls of its containee. If the partial pressure of
hydrogen is 1.65 atm, find the mole fraction of oxygen in the mixture.

Accepted Answer

Q262118

A mixture of hydrogen gas and oxygen gas exerts a total pressure of
3.0 atm on the walls of its container. If the partial pressure of
hydrogen is 1.65 atm, find the mole fraction of oxygen in the mixture.

SOLUTION :

First, we will find the partial pressure of the Oxygen gas.

There is only hydrogen and oxygen gas in the mixture, so

TOTAL PRESSURE = PARTIAL PRESSURE OF H2 + PARTIAL PRESSURE OF O2.

Total pressure = 3.0 atm, Partial pressure = 1.65 atm.

plug this information in the formula and find the Partial pressure of
O2.

3.0 atm = 1.65 atm + Partial pressure of O2.

Partial pressure of O2 = 3.0 atm - 1.65 atm = 1.35 atm.

Next, using the partial pressure of O2 and Total pressure, we can find
the mole fraction of O2 in the mixture.

mole \ fraction \ of \ O_2 = \frac{Partial \ pressure \ of \
O_2}{Total Pressure }

Partial pressure of O2 = 1.35 atm.

Total pressure = 3.0 atm

plug this in the equation we have

mole \ fraction \ of \ O_2 = \frac{1.35 \ atm }{3.0 \ atm } = 0.45

Mole fraction is a unitless quantity.

HENCE THE MOLE FRACTION OF O2 IN THE MIXTURE IS 0.45.

Question #262118

Expert's answer

Total Pressure = Partial pressure of H₂ + Partial pressure of O₂.

Hence the mole fraction of O₂ in the mixture is 0.45.

Question #262118

Expert's answer

Total Pressure = Partial pressure of H2 + Partial pressure of O2.

Hence the mole fraction of O2 in the mixture is 0.45.

Total Pressure = Partial pressure of H₂ + Partial pressure of O₂.

Hence the mole fraction of O₂ in the mixture is 0.45.