Final Pressure of Mixed Gases at 25°C

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To determine the final pressure of mixed gases at 25°C, the initial pressures and volumes of F2 and N2 are used in the formula P=(P1V1+P2V2)/(V1+V2). The initial conditions are F2 at 271.78 torr in a 2 L flask and N2 at 372.79 torr in a 1 L flask. After applying the formula, the calculated final pressure is approximately 458.17 torr. The approach emphasizes that the total number of moles remains constant at constant temperature. This method effectively combines the contributions of both gases to find the final pressure after mixing.
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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.
 
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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
 
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