`0.2 g` of an organic compound containing `C,H` and `O` on combustion yielded `0.147 g CO_(2)` and `0.12 g` water. The percentage of oxygen in it is `:`

Options

A. `76.67%`
B. `15.45%`
C. `83.23%`
D. `89.50%`

Explanation

To find the percentage of oxygen in the organic compound, we can follow these steps:

### Step 1: Calculate the mass of carbon in the compound.
- The mass of carbon can be derived from the mass of carbon dioxide (CO₂) produced during combustion.
- The molecular weight of CO₂ is 44 g/mol, and the molecular weight of carbon (C) is 12 g/mol.
- From the combustion, we know that 0.147 g of CO₂ was produced.

Using the formula:
\[ \text{Mass of C} = \left( \frac{\text{Molar mass of C}}{\text{Molar mass of CO}_2} \right) \times \text{mass of CO}_2 \]
\[ \text{Mass of C} = \left( \frac{12}{44} \right) \times 0.147 \, \text{g} = 0.0401 \, \text{g} \]

### Step 2: Calculate the mass of hydrogen in the compound.
- The mass of hydrogen can be derived from the mass of water (H₂O) produced during combustion.
- The molecular weight of water is 18 g/mol, and the molecular weight of hydrogen (H) is 1 g/mol.
- From the combustion, we know that 0.12 g of water was produced.

Using the formula:
\[ \text{Mass of H} = \left( \frac{2 \times \text{Molar mass of H}}{\text{Molar mass of H}_2\text{O}} \right) \times \text{mass of H}_2\text{O} \]
\[ \text{Mass of H} = \left( \frac{2 \times 1}{18} \right) \times 0.12 \, \text{g} = 0.0133 \, \text{g} \]

### Step 3: Calculate the mass of oxygen in the compound.
- The total mass of the organic compound is given as 0.2 g.
- The mass of oxygen can be calculated by subtracting the mass of carbon and hydrogen from the total mass of the compound.

Using the formula:
\[ \text{Mass of O} = \text{Total mass} - (\text{Mass of C} + \text{Mass of H}) \]
\[ \text{Mass of O} = 0.2 \, \text{g} - (0.0401 \, \text{g} + 0.0133 \, \text{g}) = 0.1466 \, \text{g} \]

### Step 4: Calculate the percentage of oxygen in the compound.
- To find the percentage of oxygen, we use the formula:
\[ \text{Percentage of O} = \left( \frac{\text{Mass of O}}{\text{Total mass}} \right) \times 100 \]
\[ \text{Percentage of O} = \left( \frac{0.1466 \, \text{g}}{0.2 \, \text{g}} \right) \times 100 \approx 73.3\% \]

### Final Answer:
The percentage of oxygen in the organic compound is approximately **73.3%**.

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