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10 December, 05:56

What is the volume, in liters, occupied by 2.79 moles of N2 gas at 439 mmHg pressure and a

temperature of 64°C?

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Answers (1)
  1. 10 December, 06:05
    0
    132.93 L

    Explanation:

    Step 1:

    Data obtained from the question:

    Volume (V) = ?

    Number of mole (n) = 2.79 moles

    Pressure (P) = 439 mmHg

    Temperature (T) = 64°C

    Step 2:

    Conversion to appropriate unit

    For pressure:

    760mmHg = 1atm

    Therefore, 439 mmHg = 439/760 = 0.58 atm

    For temperature:

    Temperature (Kelvin) = temperature (celsius) + 273

    temperature (celsius) = 64°C

    Temperature (Kelvin) = 64°C + 273 = 337 K

    Step 3:

    Determination of the volume.

    The volume occupied by N2 can be obtained by using the ideal gas equation as follow:

    Volume (V) = ?

    Number of mole (n) = 2.79 moles

    Pressure (P) = 0.58 atm

    Temperature (T) = 337 K

    Gas constant (R) = 0.082atm. L/Kmol

    PV = nRT

    0.58 x V = 2.79 x 0.082 x 337

    Divide both side by 0.58

    V = (2.79 x 0.082 x 337) / 0.58

    V = 132.93 L

    Therefore, the volume occupied by N2 is 132.93 L
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