A mixture of 2.00 moles of H 2 , 3.00 moles of NH 3 , 4.00 moles of CO 2 and 5.0
ID: 1048356 • Letter: A
Question
A mixture of 2.00 moles of H2, 3.00 moles of NH3, 4.00 moles of CO2 and 5.00 moles of N2 in a 15.0L container at 180C What is the total pressure and the partial pressure of each gas?
PV=nRT is the equation i'm using
R=0.08206
I need to convert C to K, find the moIes in grams of each, the use formula for each compund, the total masses and do the same, correct?
I think I have this figured out, but I would like to check my answers. Please post work so I can compare, thank you
This is what I came up with, I don't think my answer is correct, total = 429, H2 = 6.42, NH3 = 81.4, CO2 = 280, N2 = 223. These don't add up to my total pressure. Welp, back to the books...
Explanation / Answer
At the same pressure and temperature, all gases exert the same pressure if moles are the same.
Total moles = 2.00 + 3.00 + 4.00 + 5.00 = 14.0 moles
Volume = 15.0 L
Temperature = 180 C = 453 K
Total pressure = moles * R * temperature / volume
= 15.0 mole * 0.0821 L-atm/mol. K * 453 K / 15.0 L = 37.2 atm
Mole fraction of each gas = moles/ total moles
MF of H2 = 2.00 mol / 15.0 mol = 0.133
MF of NH3 = 3.00/ 15.0 = 0.200
MF of CO2 = 4.00 / 15.0 = 0.27
MF of N2 = 5.00 / 15.0 = 0.33
Partial pressure of each gas = MF * total pressure
Pressure of H2 = 0.133 * 37.2 = 4.95 atm
Pressure of NH3 = 0.200 * 37.2 = 7.44 atm
Pressure of CO2 = 0.27 * 37.2 = 10.0 atm
Pressure of N2 = 0.33 * 37.2 = 12.3 atm
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