0.290 g of an organic compound containing C, H and O gave on combustion 0.270 g of water and 0.66 g of `CO_(2)`. What is empirical formula of the compound.

Explanation

To find the empirical formula of the organic compound, we will follow these steps:

### Step 1: Determine the mass of carbon and hydrogen in the compound.

1. **Mass of CO2 produced**: 0.66 g
- The molar mass of CO2 = 12 (C) + 16*2 (O) = 44 g/mol
- Moles of CO2 = mass / molar mass = 0.66 g / 44 g/mol = 0.0150 mol
- Since each mole of CO2 contains 1 mole of carbon, moles of C = 0.0150 mol
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