Question

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`?

Answer 1

Well, `PV=nRT`.........and so.......`V~=3*L`

Explanation:

You must simply KNOW that `1*atm` pressure will support a column of mercury that is `760*mm` high; and thus `"Torr"-=1*mm*Hg` stands in for a pressure measurement. You must also know the relationship between `"degrees Kelvin"`, and `"degrees centigrade"`: `0` `""^@C-=+273.15*K`

`V=(nRT)/P=(0.1*molxx0.0821*(L*atm)/(K*mol)xx310*K)/((700*"Torr")/(760*"Torr"*atm^-1))`

`=??*L`. The question would have been better proposed had it been specified that `0.1*mol` quantity of gas had been enclosed in a piston at the given temperature and pressure.