Question

For the balanced redox reaction:

$2KMn{O}_4+16HCl\to 2KCl+2MnC{l}_2+5C{l}_2+8H_{2}O$
Calculate the number of gram equivalents of $HCl$ if $58.4g$ of $HCl$ is taken.

• A. 0.25
• B. 0.5
• C. 0.75
• D. 1

Answer 1

The correct option is D 1

As only 10 moles of $C{l}^{-}$ ions undergoes oxidation,
n - factor of HCl will be $=\frac{10}{16}=\frac{5}{8}$
$\text{Equivalent weight of HCl}=\frac{\text{Molar Mass}}{\text{n - factor}}$

$\text{Equivalent weight of HCl}=\frac{36.5}{\left(\frac{5}{8}\right)}=\frac{8\times 36.5}{5}=58.4$
$\text{Equivalents}=\frac{\text{Given weight}}{\text{Equivalent weight}}\text{Equivalents}=\frac{58.4}{58.4}=1$