Question

In a reaction container, $100g$ of hydrogen and $100g$ of $C{l}_2$ are mixed for the formation of $HCl$ gas. What is the limiting reagent and how much $HCl$ is formed in the reaction?

• A. $H_2$ is limiting reagent and $36.5g$ of $HCl$ are formed
• B. $C{l}_2$ is limiting reagent and $102.8g$ of $HCl$ are formed
• C. $H_2$ is limiting reagent and $142g$ of $HCl$ are formed
• D. $C{l}_2$ is limiting reagent and $73g$ of $HCl$ are formed

Answer 1

Answer: (B)

$\underset{\text{2g}}{H_2}$+$\underset{\text{71g}}{C{l}_2}\to \underset{\text{73g}}{2HCl}$
$2g$ of $H_2$ reacts with $71g$ of $C{l}_2$
$100g$ of $H_2$ will react with $\frac{71}{2}\times 100=3550g$ of $C{l}_2$
Hence, $C{l}_2$ is the limiting reagent.
$71g$ of $C{l}_2$ produces $73g$ of $HCl$
$100g$ of $C{L}_2$ will produce $\frac{73}{71}\times 100=102.8g$ of $HCl$