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4 August, 05:34

For a pressure of 1.00 atm and a temperature of 24.0 ∘C, use the ideal-gas law to estimate the number of air molecules in the room. Assume all the air is N2. Express your answer to three significant figures and include the appropriate units

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  1. 4 August, 08:19
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    mass of air = 324 kg

    Explanation:

    mass of air = moles of air * molecular weight (N₂)

    moles of air = PV / RT

    Given that

    P = 1 atm

    Volume of room = 282 m³

    R = 0.082L atm mol⁻¹k⁻¹

    = (1 * 282 * 10³) / (0.0821 * 297)

    = 11.565 * 10³mol

    molecular weight of N₂ = 28g/mol

    mass of air = (11.565 * 10³) mol * 0.028kg/mol

    = 323.8kg

    to three significant figures = 324 kg
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