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12 April, 11:23

What is the total mass of copper consumed when 16.0 moles of water are produced?

3Cu + 8HNO3 → 3Cu (NO3) 2 + 2NO + 4H2O

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  1. 12 April, 11:38
    0
    762.55 g.

    Explanation:

    For the balanced reaction:

    3Cu + 8HNO₃ → 3Cu (NO₃) ₂ + 2NO + 4H₂O.

    It is clear that 3 mol of Cu reacts with 8 mol of HNO₃ to produce 3 mol of Cu (NO₃) ₂, 2 mol of NO, and 4 mol of H₂O.

    We need to calculate the no. of moles of copper consumed when 16.0 moles of water are produced:

    Using cross multiplication:

    3 mol of Cu produce → 4 mol of H₂O, from stichiometry.

    ? mol of Cu produce → 16 mol of H₂O.

    ∴ no. of moles of Cu needed = (3 mol) (16 mol) / (4 mol) = 12 mol.

    Now, we can get the mass of Cu needed:

    ∴ mass of Cu = (no. of moles) (atomic mass of Cu) = (12 mol) (63.546 g/mol) = 762.55 g.
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