Partial pressure?

Question

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?

Answer 1

Presumably, you are expected to assume that the gases are behaving as ideal gases. In particular, this means that their partial pressures are additive.

After you open the valve, the H2 has a volume of 5L to spread out into, instead of 2L, so its partial pressure will be only 2/5 (or 40%) of the original 200 Torr. (You'll have to multiply to figure out what that number is.)

So the rest of the 260 Torr is caused by the N2. And that contribution is only 3/5 (or 60%) of what the N2 pressure was before the valve was opened. So you need to subtract the H2 partial pressure (calculated in the preceding paragraph) from 260, and then divide by 60% to get the original N2 pressure.

Answer 2

this is a kinda high lv Q. i dono but probobly goin to be highre than 200.0 torr wish i could help more