Question

What is the pressure in `mm*Hg` if a `4.0*g` mass of oxygen gas at `303*K` was confined to a container whose volume of `3000*mL`?

Answer 1

`P=1.04*atm.......`

Explanation:

We use the Ideal Gas Equation, to give.....

`P=(nRT)/V=((4.00*g)/(32.00*g*mol^-1)xx0.0821*(L*atm)/(K*mol)xx303*K)/(3000*mLxx10^-3*L*mL^-1)`

`=1.04*atm`

Now had the pressure been UNDER `1*atm` I could use the relationship `1*atm-=760*mm*Hg`; i.e. an atmosphere will support a column of mercury that is so high. You do not measure a pressure that is greater than `1*atm` in `mm*Hg`. Whoever set this problem was ignorant.........