Odisha Board Solutions for Chapter: Redox Reaction, Exercise 1: QUESTIONS

In the following reaction,  

${\mathrm{MnO}}_4^{-}+{\mathrm{H}}^{+}+\mathrm{X} \to {\mathrm{Mn}}^{2+}+4{\mathrm{H}}_2\mathrm{O}$,     $\mathrm{X}$ is

In the following equation : 

${\mathrm{Cr}}_2{\mathrm{O}}_7^{2-}+{\mathrm{H}}^{+}+\mathrm{X} \to 2{\mathrm{Cr}}^{3+}+7{\mathrm{H}}_2\mathrm{O}$,   $\mathrm{X}$ is

Balance the following equations by oxidation number method.

${\mathrm{K}}_2{\mathrm{MnO}}_4+\mathrm{HCl} \to {\mathrm{KMnO}}_4+{\mathrm{MnO}}_2+\mathrm{KCl}+{\mathrm{H}}_2\mathrm{O}$

Balance the following equation by oxidation number method

${\mathrm{MnO}}_4^{-}+{\mathrm{SO}}_2 \to {\mathrm{Mn}}^{2+}+{\mathrm{H}}_2{\mathrm{SO}}_4$

Consider the reactions : 

$$\begin{gathered} 2{\mathrm{S}}_2{\mathrm{O}}_{3\left(\mathrm{aq}\right)}^{2-}+{\mathrm{I}}_{2\left(\mathrm{s}\right)} \to {\mathrm{S}}_4{\mathrm{O}}_{6\left(\mathrm{aq}\right)}^{2-}+2{\mathrm{I}}_{\left(\mathrm{aq}\right)}^{-} \\ {\mathrm{S}}_2{\mathrm{O}}_{3\left(\mathrm{aq}\right)}^{2-}+2{\mathrm{Br}}_{2\left(\mathrm{l}\right)}+5{\mathrm{H}}_2{\mathrm{O}}_{\left(\mathrm{l}\right)} \to 2{\mathrm{SO}}_{4\left(\mathrm{aq}\right)}^{2-}+4{\mathrm{Br}}_{\left(\mathrm{aq}\right)}^{-}+10{\mathrm{H}}_{\left(\mathrm{aq}\right)}^{+} \end{gathered}$$

Why does the same reductant, thiosulphate reacts differently with iodine and bromine?

Sulphur dioxide and hydrogen peroxide can act as oxidising as well as reducing agents in their reactions. Why?

Determine the volume of $\frac{\mathrm{M}}{8}{\mathrm{KMnO}}_4$ solution required to react completely with $20 {\mathrm{Cm}}^3$ of $\frac{\mathrm{M}}{4}{\mathrm{FeSO}}_4$ solution in acidic medium.

Which of the following species, do not show disproportionation reaction and why?

${\mathrm{ClO}}^{-}, {\mathrm{ClO}}_2^{-}, {\mathrm{ClO}}_3^{-}$ and ${\mathrm{ClO}}_4^{-}$

Also write reaction for each of the species that disproportionates.