If the density of lead is 11.34 g/cm³,how many atoms are in a piece of lead that is 2.00 cm wide,1.00 m long,and 2.00 mm thick? A)1.32 × 10²⁴ atoms B)1.16 × 10²³ atoms C)1.32 × 10²³ atoms D)1.16 × 10²² atoms E)6.60 × 10²³ atoms

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Quizplus · Accepted Answer

First, calculate the volume of the lead piece in cubic centimeters (cm³): 2.00 cm * 100 cm (1.00 m = 100 cm) * 0.2 cm (2.00 mm = 0.2 cm) = 40 cm³. The mass of the lead piece is then volume * density = 40 cm³ * 11.34 g/cm³ = 453.6 g. The molar mass of lead (Pb) is approximately 207.2 g/mol, so the number of moles of lead = 453.6 g / 207.2 g/mol ≈ 2.19 mol. Avogadro's number is 6.022 × 10²³ atoms/mol, so the total number of atoms = 2.19 mol * 6.022 × 10²³ atoms/mol ≈ 1.32 × 10²⁴ atoms.

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