Question

Pennies minted after 1982 are mostly zinc (97.5%) with a copper cover. If a post-1982 penny is dissolved in a small amount of nitric acid, the copper coating reacts as in Problem 3.90 and the exposed zinc reacts according to the following equation: $$\mathrm{Zn}(\mathrm{s})+2 \mathrm{HNO}_{3}(a q) \longrightarrow \mathrm{Zn}\left(\mathrm{NO}_{3}\right)_{2}(a q)+\mathrm{H}_{2}(g)$$ For a penny that weighs $2.482 \mathrm{g},$ what is the molarity of the $\mathrm{Zn}\left(\mathrm{NO}_{3}\right)_{2}$ if the resultant solution is diluted to 250.0 $\mathrm{mL}$ with water?

          Pennies minted after 1982 are mostly zinc (97.5%) with a copper cover. If a post-1982 penny is dissolved in a small amount of nitric acid, the copper coating reacts as in Problem 3.90 and the exposed zinc reacts according to the following equation:
$$\mathrm{Zn}(\mathrm{s})+2 \mathrm{HNO}_{3}(a q) \longrightarrow \mathrm{Zn}\left(\mathrm{NO}_{3}\right)_{2}(a q)+\mathrm{H}_{2}(g)$$
For a penny that weighs $2.482 \mathrm{g},$ what is the molarity of the
$\mathrm{Zn}\left(\mathrm{NO}_{3}\right)_{2}$ if the resultant solution is diluted to 250.0 $\mathrm{mL}$ with water?

Added by Andrea A.

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