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4 September, 17:46

A 1.50 mol sample of He occupies a volume of 2.50 L at a pressure of 14.7 atm. What will be the pressure of a 1.50 mol sample of H2 gas under the same conditions

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  1. 4 September, 20:53
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    Answer: 14.7 atm

    Explanation:

    Using the ideal gas law also called the general gas equation;

    PV = nRT

    Where,

    P = pressure

    V = Volume

    n = amount of substance

    R = ideal gas constant

    T = temperature

    For the He sample;

    V = 2.5 L

    n = 1.5 mol

    R = 8.314 J/mol/K or 0.0821 L atm/mol/K

    T = ?

    T = PV/nR

    T = 14.7*2.5 / (1.5*0.0821)

    T = 298.42K

    For the H2 sample, since both are under the same condition:

    P = nRT/V

    P = (1.5*0.0821*298.42) : 2.5

    P = 14.7 atm.
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