Consider two flasks that are connected by a valve.
One flask has a volume of 2.00L and contains H2 at a pressure of 200.0 Torr. The other flask has a volume of 3.00L and contains N2 at an unknown pressure. If the total pressure in the flasks is 260.0 Torr after the valve is opened, what was the initial pressure of the N2 in the 3.00L flask?
2006-10-17 12:11:20 · 2 answers · asked by Anonymous in Science & Mathematics ➔ Chemistry
OK...Gases basically behave like another gas isn't there. So, if you just think about the hydrogen for a minute, it went from 2 L at 200 torr into a total volume of 5 L. So, the pressure of the hydrogen would be 2/5(200) or 80.0 Torr. Now, you have to work the same problem basically backward for the nitrogen. Since the final total pressure is 260 torr, you know that 80 torr of that is the hydrogen. So, the pressure of nitrogen in the final state is 180 Torr. With that and the ratios of the 2 volumes, you can calculate the initial pressure of the nitrogen (P1V1=P2V2).
2006-10-17 12:21:12 · answer #1 · answered by hcbiochem 7 · 0⤊ 0⤋
PV(H2) + PV(N2) = PV(TOTAL)
Therefore P(N2) = [PV(TOTAL) - PV(H2)]/V(N2)
The answer is 300, but see if you can get it yourself.
2006-10-17 19:27:00 · answer #2 · answered by Buzlite 2 · 0⤊ 0⤋