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21 July, 08:14

How many milliliters of nitrogen, N2, would have to be collected at 99.19 kPa and 28oC to have a sample containing 0.015 moles of N2

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  1. 21 July, 08:39
    0
    378mL

    Explanation:

    The following data were obtained from the question:

    Pressure (P) = 99.19 kPa

    Temperature (T) = 28°C

    Number of mole (n) = 0.015 mole

    Volume (V) = ... ?

    Next, we shall convert the pressure and temperature to appropriate units. This is illustrated below:

    For Pressure:

    101.325 KPa = 1 atm

    Therefore, 99.19 kPa = 99.19/101.325 = 0.98 atm

    For Temperature:

    T (K) = T (°C) + 273

    T (°C) = 28°C

    T (K) = 28°C + 273 = 301K.

    Next we shall determine the volume of N2. The volume of N2 can be obtained by using the ideal gas equation as shown below:

    PV = nRT

    Pressure (P) = 0.98 atm

    Temperature (T) = 301K

    Number of mole (n) = 0.015 mole

    Gas constant (R) = 0.0821atm. L/Kmol.

    Volume (V) = ... ?

    0.98 x V = 0.015 x 0.0821 x 301

    Divide both side by 0.98

    V = (0.015 x 0.0821 x 301) / 0.98

    V = 0.378 L

    Finally, we shall convert 0.378 L to millilitres (mL). This is illustrated below:

    1L = 1000mL

    Therefore, 0.378L = 0.378 x 1000 = 378mL

    Therefore, the volume of N2 collected is 378mL
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