Two moles of an ideal gas initially at 224K and 0.55 atm are compressed to 1.55 atm. I have to find the final volume of the gas so first I found initial volume 67.72 then I found the final volume which was 0.024 but it's not right and I don't know what I'm doing wrong.
2007-11-30 12:30:41 · 2 answers · asked by Shane 1 in Science & Mathematics ➔ Chemistry
I used PV = nRT and got 66.84 where you got 67.72.
(0.55) (x) = (2) (0.08206) (224)
I then used P1V1 = P2V2 and got 23.7 where you got 0.024 (some decimal places messed up??)
(0.55) (66.84) = (1.55) (x)
2007-11-30 12:44:13 · answer #1 · answered by ChemTeam 7 · 0⤊ 0⤋
PV = nRT V = nRT/P
V = (2mol)(0.082L-atm/K-mol)(224K)/(0.55atm) = 66.8L
P1V1 = P2V2 V2 = P1V1/P2
V2 = 0.55atm)(66.8L)/(1.55atm) = 23.7L
2007-11-30 12:51:33 · answer #2 · answered by steve_geo1 7 · 0⤊ 0⤋