`0.45 g` of an orgainc compound containing only `C, H` and `N` on combustion gave `1.1 g` of `CO_(2)` and `0.3 g` of `H_(2) O`. What is the percentage of `C, H` and `N` in the orgainc compound.

Explanation

To find the percentage of carbon (C), hydrogen (H), and nitrogen (N) in the organic compound, we can follow these steps:

### Step 1: Calculate the percentage of Carbon (C)
1. **Determine the mass of Carbon in CO2**:
- The molar mass of CO2 is 44 g/mol (12 g/mol for C + 32 g/mol for O).
- The mass of carbon in CO2 can be calculated using the formula:
\[ \text{Mass of C} = \left(\frac{\text{Molar mass of C}}{\text{Molar mass of CO2}}\right) \times \text{Mass of CO2} \]
- Substituting the values:
\[ \text{Mass of C} = \left(\frac{12}{44}\right) \times 1.1 \, \text{g} = 0.3 \, \text{g} \]

2. **Calculate the percentage of Carbon**:
- Use the formula:
\[ \text{Percentage of C} = \left(\frac{\text{Mass of C}}{\text{Mass of compound}}\right) \times 100 \]
- Substituting the values:
\[ \text{Percentage of C} = \left(\frac{0.3}{0.45}\right) \times 100 \approx 66.67\% \]

### Step 2: Calculate the percentage of Hydrogen (H)
1. **Determine the mass of Hydrogen in H2O**:
- The molar mass of H2O is 18 g/mol (2 g/mol for H + 16 g/mol for O).
- The mass of hydrogen in H2O can be calculated using the formula:
\[ \text{Mass of H} = \left(\frac{\text{Molar mass of H}}{\text{Molar mass of H2O}}\right) \times \text{Mass of H2O} \]
- Substituting the values:
\[ \text{Mass of H} = \left(\frac{2}{18}\right) \times 0.3 \, \text{g} = 0.0333 \, \text{g} \]

2. **Calculate the percentage of Hydrogen**:
- Use the formula:
\[ \text{Percentage of H} = \left(\frac{\text{Mass of H}}{\text{Mass of compound}}\right) \times 100 \]
- Substituting the values:
\[ \text{Percentage of H} = \left(\frac{0.0333}{0.45}\right) \times 100 \approx 7.41\% \]

### Step 3: Calculate the percentage of Nitrogen (N)
1. **Determine the percentage of Nitrogen**:
- Since the organic compound contains only C, H, and N, we can find the percentage of nitrogen by subtracting the percentages of carbon and hydrogen from 100%:
\[ \text{Percentage of N} = 100 - (\text{Percentage of C} + \text{Percentage of H}) \]
- Substituting the values:
\[ \text{Percentage of N} = 100 - (66.67 + 7.41) \approx 25.92\% \]

### Final Results:
- Percentage of Carbon (C): **66.67%**
- Percentage of Hydrogen (H): **7.41%**
- Percentage of Nitrogen (N): **25.92%**