0.73 g of orgainc compound on oxidation gave 1.32 g of carbon dioxide. The percentage of carbon in the given compound will be

Options

A. 49.32
B. 59.32
C. 29.32
D. 98.64

Answer

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

### Step 1: Calculate the moles of CO2 produced
We are given that 1.32 g of carbon dioxide (CO2) is produced. The molar mass of CO2 can be calculated as follows:
- Molar mass of Carbon (C) = 12 g/mol
- Molar mass of Oxygen (O) = 16 g/mol
- Therefore, molar mass of CO2 = 12 g/mol + (2 × 16 g/mol) = 44 g/mol

Now, we can calculate the moles of CO2:
\[ \text{Moles of CO2} = \frac{\text{mass of CO2}}{\text{molar mass of CO2}} = \frac{1.32 \, \text{g}}{44 \, \text{g/mol}} = 0.03 \, \text{mol} \]

### Step 2: Determine the moles of Carbon in the organic compound
From the reaction, we know that 1 mole of carbon produces 1 mole of CO2. Therefore, the moles of carbon in the organic compound will also be 0.03 mol.

### Step 3: Calculate the mass of Carbon
Now, we can calculate the mass of carbon using its moles and molar mass:
\[ \text{Mass of Carbon} = \text{moles of Carbon} \times \text{molar mass of Carbon} = 0.03 \, \text{mol} \times 12 \, \text{g/mol} = 0.36 \, \text{g} \]

### Step 4: Calculate the percentage of Carbon in the organic compound
To find the percentage of carbon in the organic compound, we use the formula:
\[ \text{Percentage of Carbon} = \left( \frac{\text{mass of Carbon}}{\text{mass of organic compound}} \right) \times 100 \]
Substituting the values:
\[ \text{Percentage of Carbon} = \left( \frac{0.36 \, \text{g}}{0.73 \, \text{g}} \right) \times 100 \approx 49.32\% \]

### Final Result
The percentage of carbon in the given organic compound is approximately **49.32%**.

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