Question

an ore contains 1.34% of the mineral argentite, Ag2S, by weight. How many grams of ts ore would have to be processesin order to obtain 1.00 g of pure solid silver(Ag) -


1) 74.6 g 2) 85.7 g 3) 107.9 4)134.0


ans 85.7. pls answer urgently..

Answer 1

Molar mass of Ag2S = 108x2 + 32  = 248 g/mol

Mass of silver in 1 mole of Ag2S = 108x2 = 216g

216 g of Ag is contained in 248g of Ag2S

1 g of Ag is contained in = (1 x 248)/216 

                                       = 1.148 g of Ag2S

The ore contains 1.34% Ag2S

∴ 1.34% ≡ 1.148 g


What about 100%?


100% ≡ 100/1.34  x 1.148

          = 85.7 g


The second choice

Answer 2

Answer:

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