Question

An ore contains 1.34%of the mineral Argentine, Ag2S, by mass. How many gram of this ore would have to be processed in order to obtain 1.00 g of pure solid silver,Ag?

Answer 1

Answer:

Explanation:

Gram molar mass of Ag₂S = 108 x 2 + 32 = 248 g/mol

Now, 1 mole of Ag₂S has 2 moles of Ag.

⇒ 216g ---> 248g

   1g ---> x

x = 248/216 = 1.148g

So, we need 1.148g of Ag₂S to get 1g of Ag.

Now, if 1.148g of Ag₂S makes up 1.34% of mass, then-

(1.148 x 100)/1.34 = 85.7 g of mineral ore is the total mass that needs to be processed.

Hope it helps!!! ^_^