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Q.

An ore contains 2.48% of the mineral argentite, Ag2S, by mass. How many grams of this ore would have to be processed in order to obtain 1.00 g of pure solid silver? (Atomic masses: Ag = 108, S = 32)

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a

36.3 g

b

40 g

c

50 g

d

46.3 g

answer is B.

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Detailed Solution

 Ag2S→ 2Ag
 Let mass of ore to be processed = x g
 Mass of mineral argentite,  Question Image
 Moles of  Question Image
 Moles of Ag formed =  =x×2.48100×2248=2x10000
 Mass of Ag formed  =2x10000×108=1
   x=46.3g

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