# What is the volume occupied by 30.7 g Cl_2(g) at 35°C and 745 torr?

Jun 10, 2017

We use the old Ideal Gas Law, and get $V \cong 11 \cdot L$

#### Explanation:

We must first express the pressure exerted by the gas. We know that $1 \cdot a t m$ of pressure will support a column of mercury that is $760 \cdot m m$ high. And thus a mercury column, even if you face an awful problem if the column breaks and the mercury spills, is a good visual representation of pressure.

And thus $1 \cdot a t m \equiv 760 \cdot m m \cdot H g$.......

And then we fill in the variables for $V = \frac{n R T}{P}$, i.e.

V=((30.7*g)/(70.9*g*mol^-1)xx0.0821*(L*atm)/(K*mol)xx308.2*K)/((745*mm*Hg)/(760*mm*Hg*atm^-1))=??*L

Is this expression dimensionally consistent? That is when I cancel out the units in the numerator and the denominator, I SHOULD get an answer in $L$...........All care taken but no responsibility admitted.