Question

Equal mass of H2, He and CH4 are mixed in empty container at 300K, when total pressure is 2.6 atm. The partial pressure of H2 in the mixture is

Answer 1

The partial pressure of hydrogen in the mixture of 1.22 atm

Explanation:

We know that partial pressure of a gas is the product of the “total pressure” and the concentration or the “mole fraction of a gas” in the mixture.

Partial pressure = Total pressure × Mole fraction

Let the moles of each gas be X.

We know that the atomic masses given below:

$H_2=2$

$He=2$

$CH_4=16$

So, we have the mole fraction of each gas which is given below:

$H_2 = \frac{X}{2}$

$He=\frac{X}{2}$

$CH_4=\frac{X}{16}$

The total moles of the gas mixture $= \frac{17X}{16}$

Now, to calculate the partial pressure of $H_2$:

Partial pressure = Total pressure × Mole fraction

$=\frac{\frac{X}{2}}{\frac{17X}{16}} \times 2.6$

$=\frac{8}{17} \times 2.6$

Partial pressure = 1.22 atm

Answer 2

Answer:

Explanation:take this perfect amswer