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20 August, 04:16

1. When using the equation P1/T1 = P2/T2to relate temperature and pressure of a gas, what must be held constant?2. A sample of gas is held in a capped flask. At 25 °C the pressure is 693 mmHg. What is the pressure of the gas at 37 °C?3. If the heat of vaporization of water is 40.7 kJ/mol, how much energy is required to vaporize 5.0 g of liquid water at 100 °C?4. Would you expect most of the components in a perfume to have a low or high vapor pressure? Explain

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  1. 20 August, 05:07
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    1.

    P1/T1 = P2/T2

    Charles' law states that the pressure of a gas on its containing vessel must be directly proportional to the absolute temperature at constant volume STP.

    2.

    Using P1/T1 = P2/T2

    T1 = 25 °C

    = 273 + 25

    = 298 K

    P1 = 693 mmHg

    T2 = 37 °C

    = 273 + 37

    = 310 K

    P2 = (693 * 310) / 298

    = 720.9 mmHg.

    3.

    q = n * Hvap

    Where,

    q = heat required

    n = number of moles

    Hvap = heat of vapourisation

    Molar mass of H2O = (1*2) + 16

    = 18 g/mol

    Number of moles = mass/molar mass

    = 5/18

    = 0.28 mol.

    q = 0.28 * 40.7

    = 11.3 kJ.

    4.

    Volatility is defined as a property of a substance which describes how readily a substance vaporizes. At a particular temperature and pressure, a substance with high volatility (high vapour pressure) is more likely to exist as a vapor, while a substance with low volatility (low vapour pressure) is more likely to be a liquid or solid.

    Most perfume components exist individually as gas so they have high vapour pressure.
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