# What volume would be occupied by a 0.1*mol quantity of gas at a temperature of 310*K, and a pressure of 700*mm*Hg?

Well, $P V = n R T$.........and so.......$V \cong 3 \cdot L$
You must simply KNOW that $1 \cdot a t m$ pressure will support a column of mercury that is $760 \cdot m m$ high; and thus $\text{Torr} \equiv 1 \cdot m m \cdot H g$ stands in for a pressure measurement. You must also know the relationship between $\text{degrees Kelvin}$, and $\text{degrees centigrade}$: $0$ ""^@C-=+273.15*K
$V = \frac{n R T}{P} = \frac{0.1 \cdot m o l \times 0.0821 \cdot \frac{L \cdot a t m}{K \cdot m o l} \times 310 \cdot K}{\left(700 \cdot \text{Torr")/(760*"Torr} \cdot a t {m}^{-} 1\right)}$
=??*L. The question would have been better proposed had it been specified that $0.1 \cdot m o l$ quantity of gas had been enclosed in a piston at the given temperature and pressure.