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28 April, 15:51

The chemical equation below shows the decomposition of ammonium nitrate (NH4NO3).

NH4NO3 → N2O + 2H20

A chemist who is performing this reaction starts with 160.1 g of NH4NO3. The molar mass of NH4NO3 is 80.03 g/mol; the molar

mass of water (H2O) is 18.01 g/mol. What mass, in grams, of H2O is produced?

9.01

18.01

36.03

7206

+2
Answers (1)
  1. 28 April, 17:33
    0
    72.04 g of H₂O

    Explanation:

    The balance chemical equation is as follow;

    NH₄NO₃ → 2 H₂O + N₂O

    To solve this problem we will first find the number of Moles of NH₄NO₃ as;

    Moles = Mass / M. Mass

    Moles = 160.1 g / 80.03 g/mol

    Moles = 2.00 Moles

    Secondly, we will find the number of moles of H₂O produced as,

    According to equation,

    1 mole of NH₄NO₃ produced = 2.0 moles of H₂O

    So,

    2.00 moles of NH₄NO₃ will produce = X moles of H₂O

    Solving for X,

    X = 2.0 moles * 2.0 mole / 1 mole

    X = 4.0 moles of H₂O

    Atlast, we will convert moles of water to mass as,

    Moles = Mass / M. Mass

    Or,

    Mass = Moles * M. Mass

    Mass = 4.0 mol * 18.01 g/mol

    Mass = 72.04 g of H₂O
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