In Carius method, `0.099 g ` organic compound gave `0.287 g AgCl.` The percentage of chlorine in the compound will be

Options

A. 28.6
B. 71.71
C. 35.4
D. 64.2

Answer

To find the percentage of chlorine in the organic compound using the Carius method, we can follow these steps:

### Step 1: Identify the masses
- Mass of the organic compound = 0.099 g
- Mass of AgCl produced = 0.287 g

### Step 2: Determine the molar masses
- Molar mass of AgCl = Molar mass of Ag + Molar mass of Cl
- Molar mass of Ag (Silver) = 107.87 g/mol
- Molar mass of Cl (Chlorine) = 35.45 g/mol
- Therefore, Molar mass of AgCl = 107.87 + 35.45 = 143.32 g/mol

### Step 3: Calculate the moles of AgCl produced
To find the moles of AgCl produced, use the formula:
\[ \text{Moles of AgCl} = \frac{\text{mass of AgCl}}{\text{molar mass of AgCl}} \]
\[ \text{Moles of AgCl} = \frac{0.287 \, \text{g}}{143.32 \, \text{g/mol}} \approx 0.00200 \, \text{mol} \]

### Step 4: Calculate the moles of Cl in the compound
Since one mole of AgCl contains one mole of Cl, the moles of Cl will also be 0.00200 mol.

### Step 5: Calculate the mass of Cl
To find the mass of chlorine in the organic compound, use the formula:
\[ \text{Mass of Cl} = \text{moles of Cl} \times \text{molar mass of Cl} \]
\[ \text{Mass of Cl} = 0.00200 \, \text{mol} \times 35.45 \, \text{g/mol} \approx 0.0709 \, \text{g} \]

### Step 6: Calculate the percentage of chlorine in the organic compound
To find the percentage of chlorine in the organic compound, use the formula:
\[ \text{Percentage of Cl} = \left( \frac{\text{mass of Cl}}{\text{mass of organic compound}} \right) \times 100 \]
\[ \text{Percentage of Cl} = \left( \frac{0.0709 \, \text{g}}{0.099 \, \text{g}} \right) \times 100 \approx 71.71\% \]

### Final Answer
The percentage of chlorine in the organic compound is approximately **71.71%**.

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