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17 September, 09:19

At what temperature celsius will 19.4g of molecular oxygen, o2, exert a pressure of 1820mm hg in a 5.12th cylinder?

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  1. 17 September, 11:07
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    T = - 28.2 °C

    Solution:

    Data Given;

    P = 1820 mmHg = 2.39 atm

    V = 5.12 L

    m = 19.4 g

    R = 0.0821 atm. L. mol⁻¹. K⁻¹

    Calculating moles,

    n = 19.4 g : 32 g. mol⁻¹

    n = 0.606 mol

    Assuming that the oxygen gas is acting perfectly, then according to Ideal Gas Equation,

    P V = n R T

    Solving for T,

    T = P V / n R

    Putting values,

    T = (2.39 atm * 5.12 L) : (0.606 mol * 0.0821 atm. L. mol⁻¹. K⁻¹)

    T = 244.7 K

    Or,

    T = - 28.2 °C
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