What will be the pressure exerted by a mixture of 3.2 g of methane and 4.4 g of carbon dioxide contained in a `9 dm^3` flask at `27^@C`?

Explanation

Moles of Methane =`W/M=3.2/16=0.2`
Moles of `H_2=W/M=4.4/44=0.1`
Total moles of `CH_4` and `H_2`=0.2+0.1=0.3
Ideal gas equation, `p=(nRt)/V`
Pressure of the gaseous mixture
`p=(0.3mol es times0.083L b ar K^-1mol^-1times300k)/(9L)`
p=0.83 bar
1 bar `=1.013 times 10^5` pascal
`0.83=0.83 times 1.013 times10^5=8.31 times 10^4` Pascal.