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

Formula :
Given 3.2 gms of `CH_4`
no.of moles of ` CH_4 = (w t)/( GMW)= ( 3.2 )/(16 ) = 0.2`
no. of moles of `CO_2 = ( 4.4 )/(44) = 0.1`
` therefore n = n_(CH_4)+n_(CO_2)`
`= 0.2 +0.1 = 0.3`
` R= 8.314 `
` T= 27 ^@ C = 300 K`
` V= 9 dm^3`
` PV =nRT `
` P=(nRT)/( V ) `
` = ( 0.3 xx 8.314 xx 300 )/( 9 ) = 83.14`
` = 83.14 xx 10^(3) p a`
` = 8.314 xx 10^4 Pa`
` therefore P= 8.3314 xx 10^4 Pa`