A gas mixture contains CO, Ar and H2. What is the total pressure of the mixture, if
the mole fraction of H2 is 0.35 and the pressure of H2 is 0.58 atm?

Considering the Dalton's partial pressure, the total pressure in the mixture of gases is 1.657 atm.

The pressure exerted by a particular gas in a mixture is known as its partial pressure.

So, Dalton's law states that the total pressure of a gas mixture is equal to the sum of the pressures that each gas would exert if it were alone:

where n is the amount of gases in the mixture.

Dalton's partial pressure law can also be expressed in terms of the mole fraction of the gas in the mixture.  So in a mixture of two or more gases, the partial pressure of gas A can be expressed as:

In this case, the partial pressure of gas H₂ can be expressed as:

You know:

Replacing in the definition of partial pressure of gas H₂:

Solving:

= 1.657 atm

In summary, the total pressure in the mixture of gases is 1.657 atm.

Learn more:

The total pressure of the mixture is 1.657 atm

Explanation:

Step 1: Data given

Mol fraction of H2 = 0.35

Pressure of H2 = 0.58 atm

Partial pressure gas = total pressure gas * mol fraction gas

Step 2: Calculate the total pressure

Partial pressure H2 = total pressure * mol fraction

0.58 atm = total pressure * 0.35

Total pressure = 0.58 atm / 0.35

Total pressure = 1.657 atm

The total pressure of the mixture is 1.657 atm