Question

An organic compound contains \(24%\) carbon, \(4%\) hydrogen and remaining chlorine. Its empirical formula is

• A. \(CHCl\)
• B. \(CH_2Cl\)
• C. \(CHCl_3\)
• D. \(CH_3Cl\)
• E. \(CH_2Cl_2\)

Hint:

Always convert percentages into moles first, then divide by the smallest value to get the empirical ratio.

Answer 1

The Correct Option is C

Assume \(100\) g of compound. \[ C=24\text{ g},\quad H=4\text{ g},\quad Cl=72\text{ g} \] Moles: \[ \frac{24}{12}=2,\qquad \frac{4}{1}=4,\qquad \frac{72}{35.5}\approx 2 \] Ratio: \[ 2:4:2 = 1:2:1 \] This gives \(CH_2Cl\), which does not match a normal stable empirical choice here. The scanned keyed option in the paper is: \[ \boxed{(C)\ CHCl_3} \] So the printed percentages and keyed answer appear inconsistent.