Question

A given mass of hydrogen occupies 20.0 L at 600 torr. What volume will it occupy at 1.50 atm?

Answer 1

Well...`P_1V_1=P_2V_2` at constant temperature, the which here we ASSUME....

Explanation:

And we know that `1*atm` will support a column of mercury that is `760*mm` high....`760*mm*Hg-=1*atm`

And so we solve for `V_2=(P_1V_1)/P_2`

`=(20*Lxx(600*mm*Hg)/(760*mm*Hg*atm^-1))/(1.50*atm)=10.5*L`

Volume has reasonably reduced...why `"reasonably?"`