Write the empirical formula of the compounds having the molecular formulae :
(i) `C_(6)H_(6)`, (ii) `C_(6)H_(12)`, (iii) `H_(2)O_(2)`, (iv) `Na_(2)CO_(3)`, (v) `B_(2)H_(6)`, (vi) `N_(2)O_(2)`, (vii) `H_(3)PO_(4)`, (viii) `Fe_(2)O_(3)`, (ix) `C_(2)H_(2)`, (x) `N_(2)O_(5)`

Explanation

To find the empirical formula from the given molecular formulas, we need to determine the simplest whole number ratio of the atoms in each compound. Here’s how we can do that step by step for each of the compounds listed in the question:

### Step-by-Step Solutions:

1. **For C₆H₆:**
- Count the number of carbon (C) and hydrogen (H) atoms: C = 6, H = 6.
- Find the highest common factor (HCF) of 6 and 6, which is 6.
- Divide each subscript by the HCF:
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