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15 July, 16:56

If 25 grams of HNCO react, how many grams of CO2 are formed?

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  1. 15 July, 17:42
    0
    25.570 g

    Explanation:

    Assuming the chemical reaction in question;

    4HNCO + 6NO → 5N₂ + 2H₂O + 4CO₂

    We are given;

    Mass HNCO as 25 grams

    We are required to calculate the mass of CO₂ formed

    Step 1: Number of moles of HNCO

    To calculate the number of moles we divide mass by the molar mass

    Number of moles = Mass : molar mass

    Molar mass of HNCO = 43.03 g/mol

    Therefore,

    Moles of HNCO = 25 g : 43.03 g/mol

    = 0.581 moles

    Step 2: Moles of CO₂ formed

    From the equation 4 moles of HNCO reacts to produce 4 moles of CO₂

    Therefore, the mole ratio of HNCO to CO₂ is 1 : 1

    Thus, moles of CO₂ is equal to moles of HNCO

    Moles of CO₂ = 0.581 moles

    Step 3: Mass of CO₂

    Mass is calculated by multiplying number of moles by molar mass

    Molar mass of CO₂ is 44.01 g/mol

    Therefore;

    Mass = 0.581 moles * 44.01 g/mol

    = 25.570 g

    Therefore, the mass of CO₂ formed is 25.570 g
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