Question

In a reaction container, $100\,g$ of hydrogen and $100 \,g$ of $Cl_2$ 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 $36.5\, g$ of $HCl$ are formed
• B. $Cl_2$ is limiting reagent and $102.8 \,g$ of $HCl$ are formed
• C. $H_2$ is limiting reagent and $142\, g$ of $HCl$ are formed
• D. $Cl_2$ is limiting reagent and $73\, g$ of $HCl$ are formed

Answer 1

Answer: (B)

$\underset{\text{2$\,$g}}{H_2}$+$\underset{\text{71$\,$g}}{Cl_2} \to \underset{\text{73$\,$g}}{2HCl}$
$2\, g$ of $H_2$ reacts with $71\, g$ of $Cl_2$
$ 100 \,g$ of $H_2$ will react with $\frac {71}{2} \times 100=3550\,g $ of $Cl_2$
Hence, $Cl_2$ is the limiting reagent.
$71\,g$ of $Cl_2$ produces $73\,g$ of $HCl$
$100\,g$ of $CL_2$ will produce $\frac{73}{71} \times 100 = 102.8\,g$ of $HCl$