Question

$0.245 \text{ gm}$ of an unknown organic compound gave $0.5453 \text{ gm}$ of $\text{AgCl}$ through Carious method. Calculate $%$ of $\text{Cl}$ in unknown compound.

• A. $55.06$
• B. $45.12$
• C. $35.50$
• D. $25.25$

Hint:

Carious method calculates the percentage of halogens by converting the halogen present in the organic sample into a silver halide ($\text{AgX}$). The relationship relies on the mole ratio of the halogen to the silver halide (1:1).

Answer 1

The Correct Option is A

Step 1: Given mass of organic compound = $0.245\,g$. Step 2: Given mass of $AgCl$ formed = $0.5453\,g$. Step 3: In Carius method, halogen is converted completely into silver halide. Step 4: Molar masses: \[ AgCl = 143.5\,g/mol,\quad Cl = 35.5\,g/mol \] Step 5: Mass of chlorine present: \[ 0.5453 \times \frac{35.5}{143.5} \] Step 6: Percentage of chlorine: \[ %\;Cl=\frac{0.5453}{0.245}\times\frac{35.5}{143.5}\times100 \approx 55.06% \] Hence, correct answer is 55.06%.