Question

the molar fraction of h2 when solution contain equall masses of h2 and he

Answer 1

Answer:

I hope it's helpfull

Explanation :

Equal mass of H 2

, He and CH 4are mixed in an empty container at 300 K when total pressure is 2.6 atm. The partial pressure of H 2

1.6 atm

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 given mass of each gas be x.

We know that the atomic masses given below:

H 2 =2He=4CH 4=16

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

H 2=x/2

He=x/4

CH 4 =x/16

The total moles of the gas mixture =0.8125x

Now, to calculate the partial pressure of :H

2Partial pressure = Total pressure × Mole fraction

= 0.8125x2x

×2.6Partial pressure of H 2=1.6 atm