Final Pressure of Mixed Gases at 25°C

[stacker]

Two separate flasks are each filled with a gas at 25 degrees Celsius; the valve between them is opened and the gases are allowed to mix. What would be the final pressure in torr after mixing, if initially F2 is in the first flask (Volume = 2 L) at 271.78 torr and N2 is in the second flask (Volume = 1 L) at 372.79 torr?
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Here's my approach. I will determine the moles of F2 and N2 using the PV = nRT equation. This equation will give me the two mole values. Then I will use the fact that Xa = (na/ntotal) = Pa/Ptotal

Doing this, I got the answer to be 0.6028618419 in atm and 458.1749998 torrs.

Could someone confirm or correct me please.

 

[omkar13]

sorry i didnt understood you my way of approach will be total no of moles are constant at const. temp
Hence P=(P1V1+P2V2)/(V1+V2) where P is final pressure after mixing

 

[Blueshift5]

Your approach is correct. To determine the final pressure after mixing, we can use the ideal gas law equation:

PV = nRT

Where:
P is pressure (in atm)
V is volume (in L)
n is moles
R is the ideal gas constant (0.0821 L*atm/mol*K)
T is temperature (in K)

First, we need to convert the initial pressures from torr to atm:

271.78 torr = 0.359 atm
372.79 torr = 0.490 atm

Next, we can use the ideal gas law to calculate the moles of F2 and N2 in each flask:

nF2 = (0.359 atm * 2 L) / (0.0821 L*atm/mol*K * 298 K) = 0.00885 moles
nN2 = (0.490 atm * 1 L) / (0.0821 L*atm/mol*K * 298 K) = 0.00607 moles

Now that we have the moles of each gas, we can calculate the total moles and the mole fraction of each gas:

ntotal = 0.00885 moles + 0.00607 moles = 0.01492 moles
Xa = (0.00885 moles / 0.01492 moles) = 0.593
Xb = (0.00607 moles / 0.01492 moles) = 0.407

Finally, we can use the mole fractions to calculate the final pressure:

Pfinal = Xa * Ptotal
Pfinal = (0.593 * 0.359 atm) + (0.407 * 0.490 atm) = 0.214 atm

Converting back to torr, the final pressure is 0.214 atm * 760 torr/atm = 162.7 torr.

Therefore, the final pressure after mixing would be 162.7 torr. Your answer of 458.1749998 torr seems to have a calculation error.