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18 April, 14:03

How many grams of nitric acid are needed to produce 30.0 g of water?

4Zn+10HNO3=4Zn (NO3) 2+NH4NO3+3H2O

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  1. 18 April, 14:19
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    Mass = 32.13 g

    Explanation:

    Given dа ta:

    Mass of water produced = 30 g

    Mass of nitric acid needed = ?

    Solution:

    Chemical equation:

    4Zn + 10HNO₃ → 4Zn (NO₃) ₂ + NH₄NO₃ + 3H₂O

    Number of moles of water:

    Number of moles = mass/molar mass

    Number of moles = 30 g / 18 g/mol

    Number of moles = 1.7 mol

    Now we will compare the moles of water with nitric acid.

    HNO₃ : H₂O

    10 : 3

    1.7 : 3/10*1.7 = 0.51 mol

    Mass of nitric acid:

    Mass = number of moles * molar mass

    Mass = 0.51 mol * 63.01 g/mol

    Mass = 32.13 g
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