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5 December, 10:24

The air in a hot-air balloon at 735 torr is heated from 22.0°C to 46.0°C. Assuming that the moles of air and the pressure remain constant, what is the density of the air at each temperature? (The average molar mass of air is 29.0 g/mol.)

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  1. 5 December, 10:47
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    D1 = 1.16 g/L

    D2 = 1.07 g/L

    Explanation:

    PV = mRT/M

    PVM = mRT

    PM/RT = m/V = D - density

    D = PM/RT

    P = 735 torr

    T1 = 22.0°C + 273.15 = 295.15 K

    T2 = 46.0°C + 273.15 = 319.15 K

    M = 29.0 g/mol

    R = 62.363 torr*L/mol*K

    D1 = PM/RT1

    D1 = (735 torr*29.0 g/mol) / (62.363 torr*L/mol*K * 295.15 K) = 1.16 g/L

    D1 = 1.16 g/L

    D2 = PM/RT2

    D2 = (735 torr*29.0 g/mol) / (62.363 torr*L/mol*K * 319.15 K) = 1.07 g/L

    D2 = 1.07 g/L
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