Dear student

Assume that 100 g each of hydrogen, oxygen and methane are present.

The volume of gases is directly proportional to the number of moles of gases.

The molar mass of hydrogen, oxygen and methane are 2 g/mol, 32 g/mol and 16 g/mol respectively.

The number of moles of hydrogen, oxygen and methane are

2/ 100 ,

32/ 100

and

16 1/100

respectively.

The ratio of the volumes of hydrogen, oxygen and methane will be

2 1/100 : 32 /100 : 16 1/100 =

1

1

:

16

1

:

8

1

=16:1:2

Hello There,

First of all calculate the total number of moles using the ideal gas law. Here as you have not mentioned temperature I have assumed it as room temperature.

BY formula n = PV/RT you'll get total moles = 0.5

Now calculate the total mass by the formula total moles = moles of ch4 + moles of SO

I.e 0.5 = x/16 + x/48

By this, you'll get x = 0.5 g

Now calculate number of moles of individual component by formula n = 0.5 g / 16 for CH4 and 0.5/48 for SO.

From the obtained values of moles of CH4 and SO, calculate the Mole fraction

which is obtained as 0.75 for CH4 and 0.25 for SO.

After this,

We have for gases, Pressure fraction = Mole Fraction

i.e p1/12 = 0.75 for CH4 and 12-p1 for SO

The obtained values for partial pressure for CH4 is 9 atm and for SO is 3 atm

Good Luck!!!!