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20 April, 16:16

Given the chemical equation, 2Mg + O2 - > 2MgO, when 2.2 g Mg react with 3.6 g of O2, 2.7 g MgO were obtained. What is the percent yield in the reaction?

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  1. 20 April, 20:05
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    Always convert to moles when comparing compounds.

    Molar mass of a compound is the sum of it's atomic molar mass units.

    Mg = 24.3 g/mol Mg

    O2 = 16 + 16 = 32 g/mol O2

    MgO = 24.3 + 16 = 40.3 g/mol MgO

    Determine the moles of each reactant/product.

    2.2 g Mg * (1 mol/24.3 g Mg) = 0.09 mol Mg

    3.6 O2 * (1 mol/32 g O2) = 0.1125 mol O2

    2.7 g MgO * (1 mol/40.3 g MgO) = 0.067 mol MgO

    Check if there's a limiting reagent. For every 1 O2 we need 2 Mg

    0.1125 mol O2 * 2 = 0.225 mol Mg needed.

    So Mg is a limiting reagent. We have plenty of O2 which is typically the case when oxygen is a reactant.

    Figure out how much product should form based on the moles of limiting reagent. For every 2 Mg 2 MgO are formed. So it's a 1:1 ratio.

    0.09 mol Mg - - - > 0.09 mol MgO

    compare the expected 0.09 mol MgO to the actual 0.067 mol MgO obtained. Calculate the percent obtained.

    (0.067 mol MgO obtained) / (0.09 mol MgO expected) * 100 = 74.44 % yield
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