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Posted about 1 month ago

When exposed to sulfur in the air, silver forms a dark layer of silver sulfide (Ag2 S)\left(\mathrm{Ag}_{2} \mathrm{~S}\right) known as "tarnish." To remove this tarnish, an aluminum-based cleaning solution may be used. The aluminum reacts with the silver sulfide and converts it back to pure silver:
3Ag2 S+2Al6Ag+Al2 S3
3 \mathrm{Ag}_{2} \mathrm{~S}+2 \mathrm{Al} \rightarrow 6 \mathrm{Ag}+\mathrm{Al}_{2} \mathrm{~S}_{3}

Removing silver tarnish with aluminum foil
What is the minimum mass of Al\mathrm{Al} needed to completely react with 1.45 grams of Ag2 S\mathrm{Ag}_{2} \mathrm{~S} ?

Show molar masses of reactants and products
Choose 1 answer:
(A) 0.105 g0.105 \mathrm{~g}
(B) 0.237 g0.237 \mathrm{~g}
(c) 0.695 g0.695 \mathrm{~g}
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Answer from Sia
Posted about 1 month ago
Key Concept
To find the minimum mass of aluminum needed, we use stoichiometry. First, calculate the moles of Ag2SAg_2S using its molar mass, then use the balanced chemical equation to find the moles of AlAl required, and finally convert this to grams using the molar mass of AlAl.

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