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

To solve the problem, we will use the Ideal Gas Law, which is given by the equation:

\[ PV = nRT \]

Where:
- \( P \) = pressure (in Pascals)
- \( V \) = volume (in liters)
- \( n \) = number of moles
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