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

1 Answer
Jun 10, 2017

Answer:

We use the old Ideal Gas Law, and get #V~=11*L#

Explanation:

We must first express the pressure exerted by the gas. We know that #1*atm# of pressure will support a column of mercury that is #760*mm# 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*atm-=760*mm*Hg#.......

And then we fill in the variables for #V=(nRT)/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.