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14 October, 20:02

A 3.24-gram sample of NaHCO3 was completely decomposed in an experiment.

2NaHCO3 → Na2CO3 + H2CO3

In this experiment, carbon dioxide and water vapors combine to form H2CO3. After decomposition, the Na2CO3 had a mass of 2.19 grams.

Determine the mass of the H2CO3 produced.

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  1. 14 October, 23:34
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    Theoretical mass/yield of H2CO3 produced = 1.196 g

    Actual mass/yield of H2CO3 produced = 1.05 g

    Explanation:

    NaHCO3 sample was decomposed to Na2CO3 + H2CO3. The balanced chemical equation for the reaction is represented below:

    2NaHCO3 → Na2CO3 + H2CO3

    The mass of NaHCO3 = 3.24 g

    Molar mass of NaHCO3 = 23 + 1 + 12 + 48 = 84 g

    From the chemical equation 2 moles of NaHCO3 was used. Therefore the mass will be 2 * 84 = 168 g

    Molar mass of H2CO3 = 2 + 12 + 48 = 62 g

    168 g of NaHCO3 produces 62 g of H2CO3

    3.24 g of NaHCO3 will produce? g of H2CO3

    cross multiply

    theoretical mass of H2CO3 produced = (3.24 * 62) / 168

    theoretical mass of H2CO3 produced = 200.88/168

    theoretical mass of H2CO3 produced = 1.1957142857 g

    Theoretical mass of H2CO3 produced = 1.196 g

    Actual mass of H2CO3

    Actual mass of H2CO3 produced = mass of NaHCO3 - mass of Na2CO3

    Actual mass of H2CO3 produced = 3.24 - 2.19

    Actual mass of H2CO3 produced = 1.05 g

    The question didn't indicate whether you want the actual mass or theoretical mass but i calculated for both mass.
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