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6 December, 16:01

Common brass is a copper and zinc alloy containing 37.0% zinc by mass and having a density of 8.48 g/cm3. A fitting composed of common brass has a total volume of 112.5cm^3. How many atoms of copper and zinc does the fitting contain?

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  1. 6 December, 18:18
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    First, determine the mass of the alloy by multiplying the density and volume.

    m = (8.48 g/cm³) (112.5 cm³) = 954 g

    The mass of zinc in this alloy is,

    (954 g) (0.37) = 352.98 g

    mass of copper,

    954 g - 352.98 g = 601.02 g

    Then, calculate the number of moles of zinc and copper present by dividing its mass with the molar mass. The molar mass of zinc is 65.38 g/mol and that of copper is 63.55 g/mol

    n (zinc) = 352.98 g / (65.38 g/mol) = 5.40 moles

    n (copper) = 601.02 g / (63.55 g/mol) = 9.46 moles

    The number of atoms of copper and zinc are determined by multiplying the number of moles with the Avogadro's number and the answers are,

    atoms (zinc) = 3.25 x 10^24 atoms

    atoms (copper) = 5.70 x 10^24 atoms
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