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2 January, 21:36

When carbon is burned in air, it reacts with oxygen to form carbon dioxide. When 20.4 g of carbon were burned in the presence of 66.2 g of oxygen, 11.8 g of oxygen remained unreacted. What mass of carbon dioxide was produced?

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  1. 2 January, 21:43
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    74.77 g

    Explanation:

    The equation for the reaction between carbon and Oxygen is given by;

    C (s) + O₂ (g) → CO₂ (g)

    We are given;

    Mass of carbon 20.4 g

    Mass of Oxygen is 66.2 g

    Remaining mass of Oxygen after the reaction is 11.8 g

    Therefore, Carbon is the rate limiting reagent since Oxygen was in excess.

    We are required to calculate the mass of carbon dioxide produced.

    Step 1: Moles of Carbon produced

    Moles = Mass : Molar mass

    Molar mass of carbon = 12.01 g/mol

    Therefore;

    Moles of Carbon = 20.4 g : 12.01 g/mol

    = 1.699 moles

    Step 2: Moles of carbon dioxide produced

    From the equation, 1 mole of carbon reacts to produce 1 mole of carbon dioxide.

    Therefore, the mole ratio of Carbon to carbon dioxide is 1 : 1

    Thus, moles of carbon dioxide = Moles of carbon

    = 1.699 moles

    Step 3: Mass of carbon dioxide produced

    Mass = Moles * Molar mass

    Molar mass of carbon dioxide = 44.01 g/mol

    Therefore;

    Mass = 1.699 moles * 44.01 g/mol

    = 74.77 g

    Therefore, the mass of carbon dioxide gas produced is 74.77 g
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