Question

$10g$ of carbon is reacted with $100g$ of $C{l}_2$ to form $CC{l}_4$. The incorrect statements are:

• A. Carbon is the limiting reagent
• B. Chlorine is the excess reagent
• C. $108.4g$ of $CC{l}_4$ is formed
• D. $0.833$ moles of $CC{l}_4$ are formed

Answer 1

Answer: (A), (B), (D)

$0.833$ moles of $CC{l}_4$ are formed

$C+2C{l}_2\to CC{l}_4$
$\text{Moles of carbon =}\frac{10}{12}=0.833moles$
$\text{Moles of chlorine}=\frac{100}{71}=1.408moles$
Finding the limiting reagent:
$C=\frac{\text{given moles}}{\text{stoichiometric coefficient}}=\frac{0.833}{1}=0.833C{l}_2=\frac{\text{given moles}}{\text{stoichiometric coefficient}}=\frac{1.408}{2}=0.704$
Hence, the limiting reagent will be chlorine.
$2\text{moles of}C{l}_2\text{produce 1 mole of}CC{l}_4$
$1.408\text{moles produce}\frac{1}{2}\times 1.408=0.704\text{moles of}CC{l}_4$
$\text{Mass of}CC{l}_4\text{produced}=0.704\times 154=108.42g$