Question

The equivalent weight of $Fe{S}_2$ in the following reaction is $Fe{S}_2+O_2\to F{e}^{+3}+S{O}_2$

• A. $\frac{Mol.wt}{1}$
• B. $\frac{Mol.wt}{7}$
• C. $\frac{Mol.wt}{11}$
• D. $\frac{Mol.wt}{9}$

Answer 1

The correct option is A $\frac{Mol.wt}{1}$

The equivalent weight of $Fe{S}_2$ in the following reaction is $\frac{Mol.wt}{1}$

$Fe{S}_2+O_2\to F{e}^{+3}+S{O}_2$.

Becuase in the above equation the oxidation state of $Fe$ is changed from $+2$ to $+3$.So the no of electrons lost is 1.

$\left(Equivalentweight\right)=\frac{Mol.wt}{(No.Of.eletronslostorgained)}$.