2.746 g of a compound gave on analysis 1.94 g of silver, 0.268 g of sulphur and 0.538 g of oxygen. Calculate the empirical formula of the compound (At. Masses : Ag = 108, S = 32, O = 16)

Explanation

To find the empirical formula of the compound based on the given masses of silver, sulfur, and oxygen, we will follow these steps:

### Step 1: Calculate the number of moles of each element.

1. **Moles of Silver (Ag)**:
\[ \text{Moles of Ag} = \frac{\text{mass of Ag}}{\text{molar mass of Ag}} = \frac{1.94 \, \text{g}}{108 \, \text{g/mol}} \approx 0.0180 \, \text{mol} \]
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