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1 November, 10:16

When carbon is burned in air, it reacts with oxygen to form carbon dioxide. When 19.2 g of carbon were burned in the presence of 61.2 g of oxygen, 10.0 g of oxygen remained unreacted. What mass of carbon dioxide was produced

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  1. 1 November, 10:39
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    We will produce 70.4 grams of CO2

    Explanation:

    Step 1: Data given

    Mass of carbon = 19.2 grams

    Mass of oxygen = 61.2 grams

    Mass of oxygen remaining = 10.0 grams

    Molar mass carbon = 12.01 g/mol

    Molar mass Oxygen = 32.0 g/mol

    Step 2: The balanced equation

    C + O2 → CO2

    Step 3: Calculate moles

    Moles = mass / molar mass

    Moles Carbon = 19.2 grams / 12.01 g/mol = 1.60 moles

    For 1 mol carbon we need 1 mol oxygen to produce 1 mol carbon dioxide

    For 1.6 moles carbon we have 1.6 moles oxygen

    Step 4: Calculate mass oxygen reacted

    Mass oxygen = 1.6 moles * 32.0 g/mol

    Mass oxygen = 51.2 grams oxygen reacted

    Remaining mass oxygen = 61.2 grams - 51.2 grams = 10.0 grams

    Step 5: Calculate moles CO2

    For 1 mol carbon we need 1 mol oxygen to produce 1 mol carbon dioxide

    For 1.6 moles carbon we'll have 1.6 moles CO2

    Step 6: Calculate mass CO2

    Mass CO2 = moles * molar mass

    Mass CO2 = 1.6 moles * 44.01 g/mol

    Mass CO2 = 70.4 grams

    We will produce 70.4 grams of CO2

    O2 = 1.6 moles
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