0.66g of an organic compound containing C, H and O gave on combustion 0.968g of `CO_(2)` and 0.792 g of `H_(2)O`. Calculate the percentage of O in the compound. (C= 12, H= 1, O= 16)

Explanation

To calculate the percentage of oxygen in the organic compound, we will follow these steps:

### Step 1: Determine the moles of CO₂ produced
The mass of CO₂ produced is given as 0.968 g. To find the number of moles of CO₂, we use the molar mass of CO₂, which is 44 g/mol.

\[ \text{Moles of } CO_2 = \frac{\text{mass of } CO_2}{\text{molar mass of } CO_2} = \frac{0.968 \, \text{g}}{44 \, \text{g/mol}} \approx 0.0220 \, \text{mol} \]
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