An equation to find FINAL PRESSURE.?

Question

Two gas tanks are linked by a connecting tube of negligible volume with a valve. One contains 15.0 L of nitrogen at 7.0 atm pressure. The other contains 8.4 L of neon at un unkown pressure. When the valve is opened, the final pressure of the two tanks combined is 10.0 atm. What was the original pressure of neon in the one tank?


My other question is finding the final pressure.


Two gas tanks are linked by a connecting tube of negligible volume with a valve. One contains 15.0 L of nitrogen at 7.2 atm of pressure. The other contains 8.3 L of helium at 4.1 atm of pressure. If the valve is opened, what is the final pressure of the two tanks combined?

Answer 1

These are GAS LAW problems, so you need to use PV=nRT. However, for these problems, nRT will be constant so you only need to use P(pressure) and V(volume). Therefore, for both of these questions, use the equation:
P1V1 + P2V2 = PtVt where P1 is the pressure in the first vessel, P2 is the pressure in the second vessel, and Pt is the total pressure of the connected system.

Problem #1
P1V1 + P2V2 = PtVt
(7.0atm)(15.0L) + (P2)(8.4L) = (10.0atm)(23.3L)
P2 = 15.4 atm

Problem#2
(7.2atm)(15.0L) + (4.1atm)(8.3L) = (Pt)(23.3L)
Pt = 6.1 atm

Answer 2

Final Pressure Calculator

Answer 3

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at 300K, the flasks are at equilibrium, the total number of moles of H2 in the apparatus is 1.4moles, with 0.7moles in each flask and with a total pressure of 50.6625kPa. when the temperature of 1 flask is raised to 400K, the H2 in this portion will move faster than those on the cooler side and, due to the more rapid movement, will be able to move through the tube at a faster rate than colder H2 molecules. the cooler flask will have the majority of H2 molecules. the pressure in the hotter flask will increase because there is no change in volume. the increased pressure, due to the increased heat, will move the hotter molecules to the other side. eventually the equilibrium will be reached agan and the molecules will be equally distributed at the new temperature. n is constant, v is constant and R is constant. we are really dealing with charles's law P1/T1 = P2 / T2 50.6625kPa / 300K = P2 / 400K new pressure = 67.55kPa before heating, each flask contains 0.7moles H2. after heating the H2 molecules will be unequally distributed due to the increased heat of the second flask. P1/n1 = P2/n2 50.6625kPa / 0.7moles= 67.55kPa / n2 n will still be 0.7moles H2 moles in first flask will be 0.933moles and 0.467moles in the second flask

Answer 4

for the first part you know Pa + Pb =10.0 atm (pressure of each tank after valve is opened)

for tank a(nitrogen) you do:
P1V1=P2V2

P1=7.0 atm
V1=15.0 L
P2=?
V2=(15.0 L + 8.4 L)

solve for P2 and get 4.49 atm

10.0 atm - 4.49 atm = 5.51 for P2 of tank 2

P1=?
V1=8.4 L
P2=5.51 atm
V2=(15.0 + 8.4)

solve for P1 (using P1V1=P2V2) and get 15.3 atm

ok, and for the 2nd problem...
solve for P2 of both tanks using P1V1=P2V2 (where V2 is 15.0 + 8.3)

you should get 4.64 + 1.46 = 6.10 atm for final pressure