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28 June, 02:17

A sample of He gas (V = 3.0 L) at 5.6 atm and 25 °C was combined with 4.5 L of Ne gas at 3.6 atm and 25 °C in a 9.0 L flask (which was initially evacuated). What is the total pressure in the 9.0 L flask after mixing? Assume the temperature remains at 25 °C.

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  1. 28 June, 02:45
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    3.67 atm

    Explanation:

    Because the gases are not reacting and the temperature remaining the same, we can apply Boyle's Law:

    P1V1 = P2V2

    Where P is the pressure, V is the volume, 1 is the initial state, and 2 the final state.

    For a mixture of gases, from Dalton's law, the total pressure is the sum of the partial pressures of the components, so:

    P1V1 = PHe*Ve + PNe*VNe

    PHe*Ve + PNe*VNe = P2*V2

    5.6*3.0 + 3.6*4.5 = P2*9

    9P2 = 33

    P2 = 3.67 atm
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