0.465g of an organic compound upon combustion produced 1.32g of `CO_(2)` and 0.315g of `H_(2)O`. 0.2325g of the same compound gave 27.8 mL of dry `N_(2)` at NTP. If the compound contained C, H and N find its formula

Explanation

To find the empirical formula of the organic compound containing carbon (C), hydrogen (H), and nitrogen (N), we will follow these steps:

### Step 1: Calculate the moles of Carbon from CO₂ produced
Given that 1.32 g of CO₂ was produced, we can calculate the moles of carbon in the compound.

1. **Find the molar mass of CO₂**:
- Molar mass of CO₂ = 12.01 g/mol (C) + 2 × 16.00 g/mol (O) = 44.01 g/mol

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