1.

An ore contains 1.24% of the mineral argentite, Ag_(2)S by mass. How many grams of this ore would have to be processed in order to obtain 1.0 g of pure solid silver?

Answer»

46.3 g
92.6 g
69.45 g
23.15 g

Solution :1 g AG `=(1)/(108)" mole"`
To get 1 mole of Ag, PURE `Ag_(2)S` required
`=(1)/(2)"mole"`
`therefore" To get 1/108 mole of Ag, pure "Ag_(2)s` required
`=(1)/(216)"mole"=(1)/(216)xx(2xx108+32)g=(248)/(216)g`
`therefore" ORE required "=(100)/(1.24)xx(248)/(216)g=92.6g`


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