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5 February, 11:13

A flashbulb of volume 2.70 mL contains O2 (g) at a pressure of 2.30 atm and a temperature of 30.0 °C. How many grams of O2 (g) does the flashbulb contain?

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  1. 5 February, 11:21
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    P = 2.30 atm

    Volume in liter = 2.70 mL / 1000 = > 0.0027 L

    Temperature in K = 30.0 + 273 = > 303 K

    R = 0.082 atm

    molar mass O2 = 31.9988 g/mol

    number of moles O2:

    P * V = n * R * T

    2.30 * 0.0027 = n * 0.082 * 303

    0.00621 = n * 24.846

    n = 0.00621 / 24.846

    n = 0.0002499 moles of O2

    Mass of O2:

    n = m / mm

    0.0002499 = m / 31.9988

    m = 0.0002499 * 31.9988

    m = 0.008 g
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