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28 March, 16:29

Chamber 1 and Chamber 2 have equal volumes of 1.0L and are assumed to be rigid containers. The chambers are connected by a valve that is initially closed. Chamber 1 contains 2.00 moles of helium and Chamber 2 contains 1.00 mol of helium. Both chambers are at a temperature of 27°C. Part 3. When the valve is opened, what happens to the pressure in Chamber 1? Choose the best answer.

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  1. 28 March, 16:59
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    1) At tne same temperature and with the same volume, initially the chamber 1 has the dobule of moles of gas than the chamber 2, so the pressure in the chamber 1 (call it p1) is the double of the pressure of chamber 2 (p2)

    => p1 = 2 p2

    Which is easy to demonstrate using ideal gas equation:

    p1 = nRT/V = 2.0 mol * RT / 1 liter

    p2 = nRT/V = 1.0 mol * RT / 1 liter

    => p1 / p2 = 2.0 / 1.0 = 2 = > p1 = 2 * p2

    2) Assuming that when the valve is opened there is not change in temperature, there will be 1.00 + 2.00 moles of gas in a volumen of 2 liters.

    So, the pressure in both chambers (which form one same vessel) is:

    p = nRT/V = 3.0 mol * RT / 2liter

    which compared to the initial pressure in chamber 1, p1, is:

    p / p1 = (3/2) / 2 = 3/4 = > p = (3/4) p1

    So, the answer is that the pressure in the chamber 1 decreases to 3/4 its original pressure.

    You can also see how the pressure in chamber 2 changes:

    p / p2 = (3/2) / 1 = 3/2, which means that the pressure in the chamber 2 decreases to 3/2 of its original pressure.
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