An organic compound contains 80 % (by wt.) carbon and the remaining percentage of hydrogen. The empirical form

Question

An organic compound contains 80 % (by wt.) carbon and the remaining percentage of hydrogen. The empirical formula of this compound is: [Atomic wt. of C is 12, H is 1]

Accepted Answer

1. **Determine the percentage of Hydrogen:**
   $$ \% 	ext{ Hydrogen} = 100\% - \% 	ext{ Carbon} = 100 - 80 = 20\% $$
2. **Calculate Moles of each element (assuming 100 g sample):**
   - Moles of Carbon ($C$) = $\frac{	ext{Mass}}{	ext{Atomic Mass}} = \frac{80}{12} \approx 6.67 	ext{ mol}$
   - Moles of Hydrogen ($H$) = $\frac{20}{1} = 20 	ext{ mol}$
3. **Determine the simplest molar ratio:**
   Divide both values by the smallest number of moles ($6.67$):
   - Ratio for $C = \frac{6.67}{6.67} = 1$
   - Ratio for $H = \frac{20}{6.67} \approx 3$
4. **Conclusion:**
   The simplest whole number ratio of $C:H$ is $1:3$. Therefore, the empirical formula is $CH_3$.

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