Start with the ideal gas equation, PV=nRT PV=nRT
and rearrange for pressure to get p=nRTV p=nRTV
. You have all the necessary variables in their proper units, so plug em' into the equation to solve for pressure in units of atmospheres.
P=(2.5 mol)(300 K)(0.08206 L atm K −1 mol −1 50.0 L =1.23 atm P=(2.5 mol)(300 K)(0.08206 L atm K−1 mol−150.0 L=1.23 atm
All that needs to be done now is converting atmospheres to mm Hg Hg
.
1.23 atm∗760 mm Hg1 atm =935 mm Hg 1.23 atm∗760 mm Hg1 atm=935 mm Hg
.
That value makes sense, since the original pressure in atmospheres was above 1, the pressure in mm Hg Hg
will be above 760.
