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 $104.28g$ 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)

$C{l}_2$ is limiting reagent and $104.28g$ of $HCl$ are formed

Balanced reaction is:

$H_2+C{l}_2\to 2HCl$

According to the reaction, one mole or 70 g chlorine reacts with 1 mole (or 2 g) hydrogen to produce 2 moles or $2\times 36.5=73gHCl$

100 g of chlorine will react with $=\frac{2}{70}\times 100=2.86$ g hydrogen.

But here, hydrogen is 100 g.

$\therefore$ chlorine is the limiting reagent and hydrogen is in excess by:

=$100-2.86=97.14g$

70 g of chlorine produces 73 g HCl

100 g of chlorine produces $=\frac{73}{70}\times 100=104.28$ g HCl

Hence, option $B$ is correct.