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29 September, 04:16

A hot-air balloon is filled with air to a volume of 4.00 3 103 m3 at 745 torr and 218C. The air in the balloon is then heated to 628C, causing the balloon to expand to a volume of 4.20 3 103 m3. What is the ratio of the number of moles of air in the heated balloon to the original number of moles of air in the balloon?

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  1. 29 September, 06:52
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    The ratio of number of moles is 0.572

    Explanation:

    Step 1: Given data

    A hot-air balloon has a volume of 4*10³ m³

    The pressure is 745 torr = 0.98 atm

    The temperature in the ballon is 218 °C = 491.15 Kelvin

    The temperature is raised to 628 °C (901.15 Kelvin) which makes to volume expand to 4.20 * 10³ m³

    Step 2: Calculate the ratio of number of moles

    In this situation we will use the ideal gas law

    PV = nRT

    We can rearrange this formula to

    P1V1 / (n1T1) = P2V2 / (n2T2)

    To find the ratio of the number of moles we should rearrange this into:

    (n2 / n1) = (P2 / P1) * (V2 / V1) * (T1 / T2)

    The P is constant so P1 = P2

    This gives us:

    (n2 / n1) = (V2 / V1) x (T1 / T2)

    (n2 / n1) = (4.20 * 10³L / 4.00*10³L) * (491.15K / 901.15K) =

    The ratio of number of moles is 0.572
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