O.N. of \(\mathrm{\mathrm{N}}\) changes from +2 to +5 hence it is reduced as well as oxidised.
CHXI08:REDOX REACTIONS
315354
In the reaction \(\mathrm{\mathrm{C}_{2} \mathrm{O}_{4}^{-2}+\mathrm{MnO}_{4}^{-}+\mathrm{H}^{+} \rightarrow \mathrm{Mn}^{+2}+\mathrm{CO}_{2}}\) the reductant is
1 \(\mathrm{\mathrm{C}_{2} \mathrm{O}_{4}^{-2}}\)
2 \(\mathrm{H^{+}}\)
3 \(\mathrm{\mathrm{MnO}_{4}^{-}}\)
4 None of these
Explanation:
In the above reaction \(\mathrm{\mathrm{C}_{2} \mathrm{O}_{4}^{-2}}\) acts as a reductant because it is oxidised to \(\mathrm{\mathrm{CO}_{2}}\) as : \(\mathrm{\mathrm{C}_{2} \mathrm{O}_{4}^{-2} \rightarrow 2 \mathrm{CO}_{2}+2 e}\) (oxidation) \(\mathrm{\mathrm{C}_{2} \mathrm{O}_{4}^{-2}}\) reduces \(\mathrm{\mathrm{MnO}_{4}^{-}}\)to \(\mathrm{\mathrm{Mn}^{+2}}\) ion in solution.
CHXI08:REDOX REACTIONS
315355
Identify the substance which behaves as both oxidising and reducing agent among the following.
The species in which an element has oxidation number lying in between its minimum and maximum values can acts as oxidant and reductant both. \(\rm{\begin{array}{llc} & \text { Min. O.N. } & \text { Max. O.N. } \\N^{3+} \text { in } \mathrm{HNO}_{2} & -3 & +5 \\\mathrm{~S}^{4+} \text { in } \mathrm{SO}_{2} & -2 & +6 \\\mathrm{O}^{1-} \text { in } \mathrm{H}_{2} \mathrm{O}_{2} & -2 & +2\end{array}}\)
O.N. of \(\mathrm{\mathrm{N}}\) changes from +2 to +5 hence it is reduced as well as oxidised.
CHXI08:REDOX REACTIONS
315354
In the reaction \(\mathrm{\mathrm{C}_{2} \mathrm{O}_{4}^{-2}+\mathrm{MnO}_{4}^{-}+\mathrm{H}^{+} \rightarrow \mathrm{Mn}^{+2}+\mathrm{CO}_{2}}\) the reductant is
1 \(\mathrm{\mathrm{C}_{2} \mathrm{O}_{4}^{-2}}\)
2 \(\mathrm{H^{+}}\)
3 \(\mathrm{\mathrm{MnO}_{4}^{-}}\)
4 None of these
Explanation:
In the above reaction \(\mathrm{\mathrm{C}_{2} \mathrm{O}_{4}^{-2}}\) acts as a reductant because it is oxidised to \(\mathrm{\mathrm{CO}_{2}}\) as : \(\mathrm{\mathrm{C}_{2} \mathrm{O}_{4}^{-2} \rightarrow 2 \mathrm{CO}_{2}+2 e}\) (oxidation) \(\mathrm{\mathrm{C}_{2} \mathrm{O}_{4}^{-2}}\) reduces \(\mathrm{\mathrm{MnO}_{4}^{-}}\)to \(\mathrm{\mathrm{Mn}^{+2}}\) ion in solution.
CHXI08:REDOX REACTIONS
315355
Identify the substance which behaves as both oxidising and reducing agent among the following.
The species in which an element has oxidation number lying in between its minimum and maximum values can acts as oxidant and reductant both. \(\rm{\begin{array}{llc} & \text { Min. O.N. } & \text { Max. O.N. } \\N^{3+} \text { in } \mathrm{HNO}_{2} & -3 & +5 \\\mathrm{~S}^{4+} \text { in } \mathrm{SO}_{2} & -2 & +6 \\\mathrm{O}^{1-} \text { in } \mathrm{H}_{2} \mathrm{O}_{2} & -2 & +2\end{array}}\)
O.N. of \(\mathrm{\mathrm{N}}\) changes from +2 to +5 hence it is reduced as well as oxidised.
CHXI08:REDOX REACTIONS
315354
In the reaction \(\mathrm{\mathrm{C}_{2} \mathrm{O}_{4}^{-2}+\mathrm{MnO}_{4}^{-}+\mathrm{H}^{+} \rightarrow \mathrm{Mn}^{+2}+\mathrm{CO}_{2}}\) the reductant is
1 \(\mathrm{\mathrm{C}_{2} \mathrm{O}_{4}^{-2}}\)
2 \(\mathrm{H^{+}}\)
3 \(\mathrm{\mathrm{MnO}_{4}^{-}}\)
4 None of these
Explanation:
In the above reaction \(\mathrm{\mathrm{C}_{2} \mathrm{O}_{4}^{-2}}\) acts as a reductant because it is oxidised to \(\mathrm{\mathrm{CO}_{2}}\) as : \(\mathrm{\mathrm{C}_{2} \mathrm{O}_{4}^{-2} \rightarrow 2 \mathrm{CO}_{2}+2 e}\) (oxidation) \(\mathrm{\mathrm{C}_{2} \mathrm{O}_{4}^{-2}}\) reduces \(\mathrm{\mathrm{MnO}_{4}^{-}}\)to \(\mathrm{\mathrm{Mn}^{+2}}\) ion in solution.
CHXI08:REDOX REACTIONS
315355
Identify the substance which behaves as both oxidising and reducing agent among the following.
The species in which an element has oxidation number lying in between its minimum and maximum values can acts as oxidant and reductant both. \(\rm{\begin{array}{llc} & \text { Min. O.N. } & \text { Max. O.N. } \\N^{3+} \text { in } \mathrm{HNO}_{2} & -3 & +5 \\\mathrm{~S}^{4+} \text { in } \mathrm{SO}_{2} & -2 & +6 \\\mathrm{O}^{1-} \text { in } \mathrm{H}_{2} \mathrm{O}_{2} & -2 & +2\end{array}}\)
O.N. of \(\mathrm{\mathrm{N}}\) changes from +2 to +5 hence it is reduced as well as oxidised.
CHXI08:REDOX REACTIONS
315354
In the reaction \(\mathrm{\mathrm{C}_{2} \mathrm{O}_{4}^{-2}+\mathrm{MnO}_{4}^{-}+\mathrm{H}^{+} \rightarrow \mathrm{Mn}^{+2}+\mathrm{CO}_{2}}\) the reductant is
1 \(\mathrm{\mathrm{C}_{2} \mathrm{O}_{4}^{-2}}\)
2 \(\mathrm{H^{+}}\)
3 \(\mathrm{\mathrm{MnO}_{4}^{-}}\)
4 None of these
Explanation:
In the above reaction \(\mathrm{\mathrm{C}_{2} \mathrm{O}_{4}^{-2}}\) acts as a reductant because it is oxidised to \(\mathrm{\mathrm{CO}_{2}}\) as : \(\mathrm{\mathrm{C}_{2} \mathrm{O}_{4}^{-2} \rightarrow 2 \mathrm{CO}_{2}+2 e}\) (oxidation) \(\mathrm{\mathrm{C}_{2} \mathrm{O}_{4}^{-2}}\) reduces \(\mathrm{\mathrm{MnO}_{4}^{-}}\)to \(\mathrm{\mathrm{Mn}^{+2}}\) ion in solution.
CHXI08:REDOX REACTIONS
315355
Identify the substance which behaves as both oxidising and reducing agent among the following.
The species in which an element has oxidation number lying in between its minimum and maximum values can acts as oxidant and reductant both. \(\rm{\begin{array}{llc} & \text { Min. O.N. } & \text { Max. O.N. } \\N^{3+} \text { in } \mathrm{HNO}_{2} & -3 & +5 \\\mathrm{~S}^{4+} \text { in } \mathrm{SO}_{2} & -2 & +6 \\\mathrm{O}^{1-} \text { in } \mathrm{H}_{2} \mathrm{O}_{2} & -2 & +2\end{array}}\)
