Suppose two 100.0 L tanks are to be filled separately with the gases helium and hydrogen. What mass of each gas is needed to produce a pressure of 155 atm in its respective tank at 22°C?
5 answers
Use PV = nRT and solve for n in each tank. Then n = grams/molar mass. You know molar mass and n, solve for grams in each tank.
DrBob222, I still don't understand
You have a 100 L tank and you want to fill it with He to a pressure of 155 atm at 22 C.
This problem is two problems in one. One for He and the other for H2. Here is the He one done for you. It's just a matter of substituting into PV = nRT and using n for solve for grams.
PV = nRT or
n = PV/RT =
P = 155 atm
V = 100 L
R = 0.08205
T = 273C + 22C = 295K
n = (155*100)/(0.08205*295)=640 more or less. You can do it more accurately.
Then grams = mols x molar mass
g He = mols He x molar mass He
g He = 640 x 4 = about 2.6 kg.
This problem is two problems in one. One for He and the other for H2. Here is the He one done for you. It's just a matter of substituting into PV = nRT and using n for solve for grams.
PV = nRT or
n = PV/RT =
P = 155 atm
V = 100 L
R = 0.08205
T = 273C + 22C = 295K
n = (155*100)/(0.08205*295)=640 more or less. You can do it more accurately.
Then grams = mols x molar mass
g He = mols He x molar mass He
g He = 640 x 4 = about 2.6 kg.
Thank!
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