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

Answer

`8.314xx10^(4)pa`

Explanation

It is known that,
`p=m/M(RT)/V`
For methane `(CH_(4)),`
`p_(CH4)=(3.2)/16xx(8.314xx300)/(9xx10^(-3))``{:[("Since "9dm^(3)=9xx10^(-3)m^(3)),(27^(@)C=300K" ")]:}`
`=5.543xx10^(4)Pa`
For carbon dioxide `(CO_(2)),`
`P_(CO_2)=(4.4)/44xx(8.314xx300)/(9xx10^(-3))`
`=2.771xx10^(4)Pa`
Totla pressure exerted by the mixture can be obtained as:
`p=p_(CH_4)+p_(CO_2)`
`=(53543xx10^(4)+2.771xx10^(4))` pa
` = 8.314 xx10^(4)` Pa
Hence, the total pressure exerted by the mixture 8.314 `xx10^(4)` Pa.