Given :
A sample of methane gas (CH₄) with a mass of 58 g is kept in a 1.5 L container at a temperature of 373 K.
To Find :
The pressure of the gas.
Solution :
Moles of methane :
[tex]n = \dfrac{58\ gram}{16\ gram/mol} \\\\n = 3.625\ moles[/tex]
We know, by ideal gas equation :
PV = nRT
Here, R is ideal gas equation, [tex]R = 0.082 \ L \ atm\ mol^{-1} \ K^{-1}[/tex]
So,
[tex]P = \dfrac{nRT}{V}\\\\P = \dfrac{3.625\times 0.082 \times 373}{1.5}\ atm\\\\P = 73.92 \ atm[/tex]
Hence, this is the required solution.
