Answer:
[tex]0.384\ \text{L}[/tex]
Explanation:
[tex]P_1[/tex] = Initial pressure = 931 torr = [tex]931\times \dfrac{101.325}{760}=124.12\ \text{kPa}[/tex]
[tex]P_2[/tex] = Final pressure = 113 kPa
[tex]V_1[/tex] = Initial volume = 350 mL
[tex]V_2[/tex] = Final volume
From the Boyle's law we have
[tex]P_1V_1=P_2V_2\\\Rightarrow V_2=\dfrac{P_1V_1}{P_2}\\\Rightarrow V_2=\dfrac{124.12\times 350}{113}\\\Rightarrow V_2=384.44\ \text{mL}=0.384\ \text{L}[/tex]
The volume the gas would occupy is [tex]0.384\ \text{L}[/tex].
