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30 January, 02:31

What mass of KNO3 would be needed to produce 18.4 liters of oxygen gas, measured at 1.50 x 10^3 kPa and 15 degrees Celsius?

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  1. 30 January, 04:20
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    Answer:-

    2328.454 grams

    Explanation:-

    Volume V = 18.4 litres

    Temperature T = 15 C + 273 = 288 K

    Pressure P = 1.5 x 10^ 3 KPa

    We know universal Gas constant R = 8.314 L KPa K-1 mol-1

    Using the relation PV = nRT

    Number of moles of oxygen gas n = PV / RT

    Plugging in the values

    n = (1.5 x 10^3 KPa) x (18.4 litres) / (8.314 L KPa K-1 mol-1 x 288 K)

    n = 11.527 mol

    Now the balanced chemical equation for this reaction is

    2KNO3 - -> 2KNO2 + O2

    From the equation we can see that

    1 mol of O2 is produced from 2 mol of KNO3.

    ∴ 11.527 mol of O2 is produced from 2 x 11.527 mol of KNO3.

    = 23.054 mol of KNO3

    Molar mass of KNO3 = 39 x 1 + 14 x 1 + 16 x 3 = 101 grams / mol

    Mass of KNO3 = 23.054 mol x 101 gram / mol

    = 2328.454 grams
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