# Problem: Modern pennies are composed of zinc coated with copper. A student determines the mass of a penny to be 2.483 g and then makes several scratches in the copper coating (to expose the underlying zinc). The student puts the scratched penny in hydrochloric acid, where the following reaction occurs between the zinc and the HCl (the copper remains undissolved):Zn(s) + 2HCl(aq) → H2(g) + ZnCl2(aq)The student collects the hydrogen produced over water at 25 oC. The collected gas occupies a volume of 0.899 L at a total pressure of 791 mm Hg .Calculate the percent zinc in the penny. (Assume that all the Zn in the penny dissolves.)

###### FREE Expert Solution

Dalton’s Law:
at 25°C, water has a vapor pressure of 23.78 mmHg

${\mathbit{P}}_{{\mathbf{H}}_{\mathbf{2}}}\mathbf{=}$767.22 mmHg

Calculate no. of moles of H2 gas:

n = 0.0371 mol H2

Balanced equation: Zn(s) + 2HCl(aq) → H2(g) + ZnCl2(aq)

• Mole to mole comparison: 1 mole Zn forms 1 mole H2

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###### Problem Details

Modern pennies are composed of zinc coated with copper. A student determines the mass of a penny to be 2.483 g and then makes several scratches in the copper coating (to expose the underlying zinc). The student puts the scratched penny in hydrochloric acid, where the following reaction occurs between the zinc and the HCl (the copper remains undissolved):
Zn(s) + 2HCl(aq) → H2(g) + ZnCl2(aq)

The student collects the hydrogen produced over water at 25 oC. The collected gas occupies a volume of 0.899 L at a total pressure of 791 mm Hg .

Calculate the percent zinc in the penny. (Assume that all the Zn in the penny dissolves.)