According to TPR (from hyperlearning science workbook, Chemistry Passage 50, #3),
It states that for equal volume of inert gases A and B, the Final Total pressure is equal to the average of the pressure of each component, so: Final Total Pressure= (P flask A +P flask B)/2.
Specifically, the problem stated that Flask A has pressure of 450 torr, and B was 620 torr, so the inert mixture of the two gases would yield Final Total Pressure of (450 + 620)/2 = 535 torr.
If the gases were not inert and reacted with one another, you would have a different Final Total Pressure.
What I don't understand is (1) why are we allowed to take the average of these individual gases to get the final pressure? In other words, does equal volume of each imply equal moles of gas for each flask- but I thought this would only be in the case if there is constant pressure (which clearly isn't the case- flasks A and B have different pressures!), volume, and temperature.
2 Which gas law applies here? I thought perhaps Raoult's Law which says Pi=(X)(Pvapor) or Dalton's law which states Pi=(X)(Ptotal). Even if the Mole fraction is X=1/2 for each gas, I'm not sure how we get TPR's "Average formula" above.
This problem/concept has confused me, and I would really be grateful for any help I can get. Thanks!
It states that for equal volume of inert gases A and B, the Final Total pressure is equal to the average of the pressure of each component, so: Final Total Pressure= (P flask A +P flask B)/2.
Specifically, the problem stated that Flask A has pressure of 450 torr, and B was 620 torr, so the inert mixture of the two gases would yield Final Total Pressure of (450 + 620)/2 = 535 torr.
If the gases were not inert and reacted with one another, you would have a different Final Total Pressure.
What I don't understand is (1) why are we allowed to take the average of these individual gases to get the final pressure? In other words, does equal volume of each imply equal moles of gas for each flask- but I thought this would only be in the case if there is constant pressure (which clearly isn't the case- flasks A and B have different pressures!), volume, and temperature.
2 Which gas law applies here? I thought perhaps Raoult's Law which says Pi=(X)(Pvapor) or Dalton's law which states Pi=(X)(Ptotal). Even if the Mole fraction is X=1/2 for each gas, I'm not sure how we get TPR's "Average formula" above.
This problem/concept has confused me, and I would really be grateful for any help I can get. Thanks!
