We can solve the problem by using the ideal gas law:
[tex] pV=nRT [/tex]
where
[tex] p=100000 Pa [/tex] is the gas pressure
[tex] V=2 m^3 [/tex] is the gas volume
n is the number of moles
[tex] R=8.314 J/mol K [/tex] is the gas constant
[tex] T=100 K [/tex] is the absolute temperature of the gas
By rearranging the equation and substituting the numbers, we find the number of moles of the gas:
[tex] n=\frac{pV}{RT}= \frac{(100000 Pa)(2 m^3)}{(8.314 J/mol K))(100 K)}=240.5 mol [/tex]
so, the correct answer is
B. 240
