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4 June, 07:36

Consider the following balanced equation for the following reaction:

15O2 (g) + 2C6H5COOH (aq) → 14CO2 (g) + 6H2O (l)

Determine the amount of CO2 (g) formed in the reaction if the percent yield of CO2 (g) is 83.0% and the theoretical yield of CO2 (g) is 1.30 moles.

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  1. 4 June, 08:27
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    The actual yield of CO2 is 1.079 moles or 47.5 grams formed

    Explanation:

    Step 1: Data given

    Number of CO2 = 1.30 moles

    Percent yield = 83.0 %

    Step 2: The balanced equation

    15O2 (g) + 2C6H5COOH (aq) → 14CO2 (g) + 6H2O (l)

    Step 3: Calculate the number moles of CO2 formed

    1.30 moles CO2 = 100 %

    The actual amount of moles = 0.83 * 1.30 = 1.079 moles

    Step 4: Calculate the percent yield of the reaction

    We can control this by calculating the percent yield of the reaction

    % yield = (actual yield / theoretical yield) * 100 %

    % yield = (1.079 moles / 1.30 moles) * 100 %

    % yield = 83.0 %

    Step 5: Calculate thr mass of CO2 produced

    Mass CO2 = moles * molar mass CO2

    Mass CO2 = 1.079 moles * 44.01 g/mol

    Mass CO2 = 47.5 grams

    The actual yield of CO2 is 1.079 moles or 47.5 grams formed
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