## Chemistry: Molecular Approach (4th Edition)

$$V = 3.0 \space L$$ The volume would not be different if the gas was argon if we consider that both helium and argon are Ideal Gases, which is appropriate for these conditions.
1. According to the Ideal Gas Law: $$V = \frac{nRT}{P} = \frac{( 0.118 \space mol)( 0.08206 \space atm \space L \space mol^{-1} \space K^{-1} )( 305 \space K)}{ 0.97 \space atm }$$ $$V = 3.0 \space L$$ The volume would not be different if the gas was argon if we consider that both helium and argon are Ideal Gases, which is appropriate for these conditions.