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28 November, 07:30

How many carbon dioxide (CO2) molecules are produced during the decomposition of 1.25 molecules of carbonic acid (H2CO3) ? Remember to use the balanced equation!

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Answers (2)
  1. 28 November, 09:22
    0
    7.5*10^23 molecules of carbon dioxide

    Explanation:

    H2CO3 → CO2 + H2O

    From the balanced reaction equation, one mole of carbonic acid produces one mole of carbon IV oxide.

    1.25 moles of carbonic acid will produce 1.25 moles of carbon dioxide

    If 1 mole of carbon dioxide contains 6.02*10^23 molecules

    1.25 moles of carbon dioxide contains 1.25*6.02*10^23 = 7.5*10^23 molecules of carbon dioxide
  2. 28 November, 09:28
    0
    1.25 molecules of CO2 will be produced

    Explanation:

    Step 1: data given

    Number of molecules carbonic acid (H2CO3) = 1.25 molecules

    Molar mass carbonic acid (H2CO3) = 62.03 g/mol

    Number of Avogadro = 6.022 * 10^23 / moles

    Step 2: Calculate moles of H2CO3

    Moles H2CO3 = 1.25 molecules / 6.02 * 10^23

    Moles H2CO3 = 2.076 * 10^-24 moles

    Step 3: The equation

    H2CO3 → H2O + CO2

    For 1 mol H2CO3 we'll have 1 mol H2O and 1 mol CO2

    For 2.076 * 10^-24 moles H2CO3 we'll have 2.076 * 10^-24 moles CO2

    Step 4: Calculate molecules CO2

    Molecules CO2 = moles CO2 * number of Avogadro

    Molecules CO2 = 2.076 * 10^-24 moles * 6.02 * 10^23

    Molecules CO2 = 1.25 molecules

    1.25 molecules of CO2 will be produced
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