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If your favorite silver jewelry ever tarnishes and you happen to have some aluminum foil on...

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Chemistry

If your favorite silver jewelry ever tarnishes and you happen tohave some aluminum foil on hand, you can actually get rid of someof that tarnish. The tarnish here is actually silver sulfide. Ifyou put the jewelry and aluminum into a dish with enough water tocover them both, the following reaction will occur:3Ag2S + 2Al --> 6Ag + Al2S3. Ifyou have a total of 5.0 g of Al foil accessible to you, how manygrams of Ag2S (thus, loosely speaking, how much jewelry)could you theoretically \"clean\"? You must show all work clearly andin detail to receive credit. All numbers immediately followingelemental symbols should be understood as subscripts. (NOTE: If youtry this at home, you may want to dissolve some baking soda in yoursolution to help neutralize the smell, because some of the sulfurhere will escape as a gaseous product and not smell verypleasant!)

Answer & Explanation Solved by verified expert
3.7 Ratings (438 Votes)

    Molar mass of Ag2S = 247.8 g/mol

    Molar mass of Al = 27 g/mol

   

    3Ag2S        + 2Al       ------------>   6Ag +   Al2S3

      3 mol    2 mol

3 x 247.8 g      2 x 27 g

     ?                     5 g

                  ? = 3 x 247.8 g of Ag2S x ( 5g/ 2 x 27 g)

                   = 68.83 g of Ag2S

         Therefore,

       68.83 grams of Ag2S could be theoretically \"clean\".
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