A gas cylinder having a volume of 25.0 L contains a mixtue of butane `CH_(3)(CH_(2))_(2) CH_(3)` and isobutane `(CH_(3))_(3) CH` in the ratio of 3 : 1 by moles. If the pressure inside the cylinder is `6.78 xx 10^(6)` pa and the temperature is 298 K, calculate the number of molecular of each gas assuming ideal gas behaviour. (1 atm = 101325 Pa)

Explanation

Total moles `(n)=(6.78x10^(6)xx25)/(101325xx0.082xx298)=68.37mo`
`N_("butane")=(1)/(4)xx68.37xx6.02xx10^(23)=3.07xx10^(25)`
`N_("Isobutane")=(1)/(4)xx68.37xx6.02xx10^(23)=1.02xx10^(25)`