Calculate the partial pressures and total pressure (in atm) exerted by 0.838 mol of methane, 0.184 mol of ethane and 0.755 mol of neon contained in a 4.00 L container at 27 C.

Question

Calculate the partial pressures and total pressure (in atm) exerted by 0.838 mol of methane, 0.184 mol of ethane and 0.755 mol of neon contained in a 4.00 L container at 27 C.

PV=nRT for methane
(4.00L) X = (0.838 mol)(0.08206 L-atm/mol-K)(300.15 K)
X = 5.160 atm

PV=nRT for ethane
(4.00L) X = (0.184 mol)(0.08206 L-atm/mol-K)(300.15 K)
X = 1.133 atm

PV=nRT for neon
(4.00L) X = (0.755 mol)(0.08206 L-atm/mol-K)(300.15 K)
X = 4.649 atm

Total Pressure: 5.160atm + 1.133atm + 4.649atm = 10.942 atm

Correct?

Answer 1

The numbers are ok and the method is correct; however, you have too many significant figures in the answer (for each and for the total).

Answer 2

So, for methane, would it be 5.16 atm; ethane 1.13 atm; neon 4.65 atm; giving a total pressure of 10.94 atm?

Answer 3

That's right.

Answer 4

Great, thanks

Answer 5

Yes, your calculations are correct. The partial pressures for methane, ethane, and neon are 5.160 atm, 1.133 atm, and 4.649 atm respectively. The total pressure exerted by the gases in the container is the sum of the partial pressures, which is equal to 10.942 atm.