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31 March, 16:51

Calculate the pressure of 2.78 g of Ne in a 5.00 L flask at - 10°C

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  1. 31 March, 17:54
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    0.60 atm

    Explanation:

    Step 1.

    Data obtained from the question.

    This includes the following:

    Mass of Ne = 2.78g

    Volume (V) = 5L

    Temperature (T) = - 10°C

    Pressure (P) = ?

    Step 2:

    Determination of the number of mole of Ne.

    The number of mole of Ne can be obtained as follow:

    Mass of Ne = 2.78g

    Molar Mass of Ne = 20g/mol

    Number of mole Ne = ?

    Number of mole = Mass/Molar Mass

    Number of mole of Ne = 2.78/20

    Number of mole of Ne = 0.139 mol

    Step 3:

    Conversion of celsius temperature to Kelvin temperature. This can be achieved by as shown below:

    Temperature (Kelvin) = temperature (celsius) + 273

    Temperature (celsius) = - 10°C

    Temperature (Kelvin) = - 10°C + 273

    Temperature (Kelvin) = 263K

    Step 4:

    Determination of the pressure. The pressure can be obtained by using the ideal gas equation as follow:

    PV = nRT

    Volume (V) = 5L

    Temperature (T) = 263K

    Number of mole (n) of Ne = 0.139mol

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

    Pressure (P) = ?

    PV = nRT

    P x 5 = 0.139 x 0.082 x 263

    Divide both side by 5

    P = (0.139 x 0.082 x 263) / 5

    P = 0.60 atm

    Therefore the pressure is 0.60 atm
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