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

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

Solutions

Expert Solution

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".

queen_honey_blossom answered 1 year ago

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