Mole ConceptMedium

Question

An ore contains 2.296% 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? (Ag = 108)

Options

A.1.148 g
B.0.026 g
C.50 g
D.2.296 g

Solution

Molecular mass of Ag2S = 2 × 108 + 32 = 248

Now, $w \times \frac{2.296}{100} \times \frac{216}{248} = 1.0 \Rightarrow w = 50\text{ g}$

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