Tag: oxidation- reduction reactions

Write balanced half reactions for the following redox reaction:
$Cr _2O _7^{2-} + Fe^{2+}\rightarrow  Cr^{3+} + Fe^{3+}$

Which particles are gained and lost during a redox reaction?

Two half reactions are given as follows:
$2e^{-} + H^{+} + H _5IO _6 \rightarrow IO^{3-} + 3H _2O $
$Cr \rightarrow Cr^{3+} + 3e^{-}$
Final balanced reaction is:

In the reaction, $FeS {2} + KMnO _{4} + H^{+} \rightarrow Fe^{3+} + SO _{2} + Mn^{2+} + H _{2}O$, the equivalent mass of $FeS _{2}$ would be equal to__________.

How much volume of $0.1M$ $Zn{ \left( Mn{ O } _{ 4 } \right)  } _{ 2 }$ is required to react with $50ml$ of $0.2M$ ferrous oxalate. Given ${ MnO } _{ 4 }^{ - }$ reduces into ${ Mn }^{ 2+ }$ in acidic medium.

For the redox reaction $MnO^- _4+C _2O^{3+} _4+H^+\rightarrow Mn^{2+}+CO _2+H _2O$. The correct whole number stoichiometric coefficients of $MnO^- _4, C _2O^{3+} _4$ and $H^+$ are respectively.

0.2 g of a sample of $
{\text{H}} _{\text{2}} {\text{O}} _{\text{2}}
$ required 10 mL of 1 N $
{\text{KMnO}} _{\text{4}}
$ in a titration in the presence of $
{\text{H}} _{\text{2}} {\text{SO}} _{\text{4}}
$. Purity of $
{\text{H}} _{\text{2}} {\text{O}} _{\text{2}}
$ is:

In alkaline medium, $ClO _2$ oxidizes $H _2O _2$ to $O _2$ and is itself reduced to ${ClO} _2^{\displaystyle-}$. Number of moles of $H _2O _2$ oxidized by 1 mole of $ClO _2$ is :

Give the products available on the cathode and the anode respectively during the electrolysis of an aqueous solution of $MgSO _4$ between inert electrodes.

For the reaction of $MnO _2\,+\,C _2O _{4}^{2-}\,+\,H^+\,\rightarrow\,Mn^{2+}\,+\,CO _2\,+\,H _2O$ the correct whole number stoichiometric coefficients of $MnO _4$ , $C _2$$O _4$ and $H^+$ are respectively :