315453
\(\mathrm{\mathrm{H}_{2} \mathrm{O}_{2}+\mathrm{H}_{2} \mathrm{O}_{2} \longrightarrow 2 \mathrm{H}_{2} \mathrm{O}+\mathrm{O}_{2}}\) is an example of disproportionation because
1 O.N. of oxygen only decreases
2 O.N. of oxygen only increases
3 O.N. of oxygen decreases as well as increases
4 O.N. of oxygen neither decreases nor increases
Explanation:
Conceptual Questions
CHXI08:REDOX REACTIONS
315454
In the reaction, \(\mathrm{3 \mathrm{Br}_{2}+6 \mathrm{CO}_{3}^{2-}+3 \mathrm{H}_{2} \mathrm{O} \rightarrow 5 \mathrm{Br}^{-}+\mathrm{BrO}_{3}^{-}+6 \mathrm{HCO}_{3}^{-}}\)
1 Bromine is oxidised and carbonate is reduced
2 Bromine is oxidised as well as reduced
3 Bromine is reduced and water is oxidised
4 \(\mathrm{\mathrm{Br}_{2}}\) is neither oxidised nor reduced
Explanation:
O.N. of \(\mathrm{\mathrm{Br}}\) in \(\mathrm{\mathrm{Br}_{2}=0}\) \(\mathrm{\mathrm{Br}^{-}=-1}\) \(\mathrm{\mathrm{BrO}_{3}^{-}=+5}\) \(\mathrm{\mathrm{Br}}\) is oxidised as well as reduced.
CHXI08:REDOX REACTIONS
315455
Which reaction does not represent auto redox or disproportionation?
In auto redox or disproportionation, same element is oxidized as well as reduced. In (1) \(\mathrm{\mathrm{Cl}_{2}}\); (2), \(\mathrm{\mathrm{H}_{2} \mathrm{O}_{2}}\) and (3), \(\mathrm{\mathrm{Cu}^{+}}\)is oxidized as well as reduced. In (4), \(\mathrm{\mathrm{N}}\) is oxidized and \(\mathrm{\mathrm{Cr}}\) is reduced in one molecule of \(\mathrm{\left(\mathrm{NH}_{4}\right)_{2} \mathrm{Cr}_{2} \mathrm{O}_{7}}\) and thus it is intramolecular redox.
315457
During the disproportionation of iodine to iodide and iodate ions, the ratio of iodate and iodide ions formed in alkaline medium is
1 \(1: 5\)
2 \(5: 1\)
3 \(3: 1\)
4 \(1: 3\)
Explanation:
\(3 \mathrm{I}_{2}+\underline{6} \mathrm{OH}^{-} \rightarrow \mathrm{IO}_{3}^{-}+5 \mathrm{I}^{-}+3 \mathrm{H}_{2} \mathrm{O}\) So, ratio of iodate to iodide ion is \(1: 5\).
315453
\(\mathrm{\mathrm{H}_{2} \mathrm{O}_{2}+\mathrm{H}_{2} \mathrm{O}_{2} \longrightarrow 2 \mathrm{H}_{2} \mathrm{O}+\mathrm{O}_{2}}\) is an example of disproportionation because
1 O.N. of oxygen only decreases
2 O.N. of oxygen only increases
3 O.N. of oxygen decreases as well as increases
4 O.N. of oxygen neither decreases nor increases
Explanation:
Conceptual Questions
CHXI08:REDOX REACTIONS
315454
In the reaction, \(\mathrm{3 \mathrm{Br}_{2}+6 \mathrm{CO}_{3}^{2-}+3 \mathrm{H}_{2} \mathrm{O} \rightarrow 5 \mathrm{Br}^{-}+\mathrm{BrO}_{3}^{-}+6 \mathrm{HCO}_{3}^{-}}\)
1 Bromine is oxidised and carbonate is reduced
2 Bromine is oxidised as well as reduced
3 Bromine is reduced and water is oxidised
4 \(\mathrm{\mathrm{Br}_{2}}\) is neither oxidised nor reduced
Explanation:
O.N. of \(\mathrm{\mathrm{Br}}\) in \(\mathrm{\mathrm{Br}_{2}=0}\) \(\mathrm{\mathrm{Br}^{-}=-1}\) \(\mathrm{\mathrm{BrO}_{3}^{-}=+5}\) \(\mathrm{\mathrm{Br}}\) is oxidised as well as reduced.
CHXI08:REDOX REACTIONS
315455
Which reaction does not represent auto redox or disproportionation?
In auto redox or disproportionation, same element is oxidized as well as reduced. In (1) \(\mathrm{\mathrm{Cl}_{2}}\); (2), \(\mathrm{\mathrm{H}_{2} \mathrm{O}_{2}}\) and (3), \(\mathrm{\mathrm{Cu}^{+}}\)is oxidized as well as reduced. In (4), \(\mathrm{\mathrm{N}}\) is oxidized and \(\mathrm{\mathrm{Cr}}\) is reduced in one molecule of \(\mathrm{\left(\mathrm{NH}_{4}\right)_{2} \mathrm{Cr}_{2} \mathrm{O}_{7}}\) and thus it is intramolecular redox.
315457
During the disproportionation of iodine to iodide and iodate ions, the ratio of iodate and iodide ions formed in alkaline medium is
1 \(1: 5\)
2 \(5: 1\)
3 \(3: 1\)
4 \(1: 3\)
Explanation:
\(3 \mathrm{I}_{2}+\underline{6} \mathrm{OH}^{-} \rightarrow \mathrm{IO}_{3}^{-}+5 \mathrm{I}^{-}+3 \mathrm{H}_{2} \mathrm{O}\) So, ratio of iodate to iodide ion is \(1: 5\).
315453
\(\mathrm{\mathrm{H}_{2} \mathrm{O}_{2}+\mathrm{H}_{2} \mathrm{O}_{2} \longrightarrow 2 \mathrm{H}_{2} \mathrm{O}+\mathrm{O}_{2}}\) is an example of disproportionation because
1 O.N. of oxygen only decreases
2 O.N. of oxygen only increases
3 O.N. of oxygen decreases as well as increases
4 O.N. of oxygen neither decreases nor increases
Explanation:
Conceptual Questions
CHXI08:REDOX REACTIONS
315454
In the reaction, \(\mathrm{3 \mathrm{Br}_{2}+6 \mathrm{CO}_{3}^{2-}+3 \mathrm{H}_{2} \mathrm{O} \rightarrow 5 \mathrm{Br}^{-}+\mathrm{BrO}_{3}^{-}+6 \mathrm{HCO}_{3}^{-}}\)
1 Bromine is oxidised and carbonate is reduced
2 Bromine is oxidised as well as reduced
3 Bromine is reduced and water is oxidised
4 \(\mathrm{\mathrm{Br}_{2}}\) is neither oxidised nor reduced
Explanation:
O.N. of \(\mathrm{\mathrm{Br}}\) in \(\mathrm{\mathrm{Br}_{2}=0}\) \(\mathrm{\mathrm{Br}^{-}=-1}\) \(\mathrm{\mathrm{BrO}_{3}^{-}=+5}\) \(\mathrm{\mathrm{Br}}\) is oxidised as well as reduced.
CHXI08:REDOX REACTIONS
315455
Which reaction does not represent auto redox or disproportionation?
In auto redox or disproportionation, same element is oxidized as well as reduced. In (1) \(\mathrm{\mathrm{Cl}_{2}}\); (2), \(\mathrm{\mathrm{H}_{2} \mathrm{O}_{2}}\) and (3), \(\mathrm{\mathrm{Cu}^{+}}\)is oxidized as well as reduced. In (4), \(\mathrm{\mathrm{N}}\) is oxidized and \(\mathrm{\mathrm{Cr}}\) is reduced in one molecule of \(\mathrm{\left(\mathrm{NH}_{4}\right)_{2} \mathrm{Cr}_{2} \mathrm{O}_{7}}\) and thus it is intramolecular redox.
315457
During the disproportionation of iodine to iodide and iodate ions, the ratio of iodate and iodide ions formed in alkaline medium is
1 \(1: 5\)
2 \(5: 1\)
3 \(3: 1\)
4 \(1: 3\)
Explanation:
\(3 \mathrm{I}_{2}+\underline{6} \mathrm{OH}^{-} \rightarrow \mathrm{IO}_{3}^{-}+5 \mathrm{I}^{-}+3 \mathrm{H}_{2} \mathrm{O}\) So, ratio of iodate to iodide ion is \(1: 5\).
315453
\(\mathrm{\mathrm{H}_{2} \mathrm{O}_{2}+\mathrm{H}_{2} \mathrm{O}_{2} \longrightarrow 2 \mathrm{H}_{2} \mathrm{O}+\mathrm{O}_{2}}\) is an example of disproportionation because
1 O.N. of oxygen only decreases
2 O.N. of oxygen only increases
3 O.N. of oxygen decreases as well as increases
4 O.N. of oxygen neither decreases nor increases
Explanation:
Conceptual Questions
CHXI08:REDOX REACTIONS
315454
In the reaction, \(\mathrm{3 \mathrm{Br}_{2}+6 \mathrm{CO}_{3}^{2-}+3 \mathrm{H}_{2} \mathrm{O} \rightarrow 5 \mathrm{Br}^{-}+\mathrm{BrO}_{3}^{-}+6 \mathrm{HCO}_{3}^{-}}\)
1 Bromine is oxidised and carbonate is reduced
2 Bromine is oxidised as well as reduced
3 Bromine is reduced and water is oxidised
4 \(\mathrm{\mathrm{Br}_{2}}\) is neither oxidised nor reduced
Explanation:
O.N. of \(\mathrm{\mathrm{Br}}\) in \(\mathrm{\mathrm{Br}_{2}=0}\) \(\mathrm{\mathrm{Br}^{-}=-1}\) \(\mathrm{\mathrm{BrO}_{3}^{-}=+5}\) \(\mathrm{\mathrm{Br}}\) is oxidised as well as reduced.
CHXI08:REDOX REACTIONS
315455
Which reaction does not represent auto redox or disproportionation?
In auto redox or disproportionation, same element is oxidized as well as reduced. In (1) \(\mathrm{\mathrm{Cl}_{2}}\); (2), \(\mathrm{\mathrm{H}_{2} \mathrm{O}_{2}}\) and (3), \(\mathrm{\mathrm{Cu}^{+}}\)is oxidized as well as reduced. In (4), \(\mathrm{\mathrm{N}}\) is oxidized and \(\mathrm{\mathrm{Cr}}\) is reduced in one molecule of \(\mathrm{\left(\mathrm{NH}_{4}\right)_{2} \mathrm{Cr}_{2} \mathrm{O}_{7}}\) and thus it is intramolecular redox.
315457
During the disproportionation of iodine to iodide and iodate ions, the ratio of iodate and iodide ions formed in alkaline medium is
1 \(1: 5\)
2 \(5: 1\)
3 \(3: 1\)
4 \(1: 3\)
Explanation:
\(3 \mathrm{I}_{2}+\underline{6} \mathrm{OH}^{-} \rightarrow \mathrm{IO}_{3}^{-}+5 \mathrm{I}^{-}+3 \mathrm{H}_{2} \mathrm{O}\) So, ratio of iodate to iodide ion is \(1: 5\).
315453
\(\mathrm{\mathrm{H}_{2} \mathrm{O}_{2}+\mathrm{H}_{2} \mathrm{O}_{2} \longrightarrow 2 \mathrm{H}_{2} \mathrm{O}+\mathrm{O}_{2}}\) is an example of disproportionation because
1 O.N. of oxygen only decreases
2 O.N. of oxygen only increases
3 O.N. of oxygen decreases as well as increases
4 O.N. of oxygen neither decreases nor increases
Explanation:
Conceptual Questions
CHXI08:REDOX REACTIONS
315454
In the reaction, \(\mathrm{3 \mathrm{Br}_{2}+6 \mathrm{CO}_{3}^{2-}+3 \mathrm{H}_{2} \mathrm{O} \rightarrow 5 \mathrm{Br}^{-}+\mathrm{BrO}_{3}^{-}+6 \mathrm{HCO}_{3}^{-}}\)
1 Bromine is oxidised and carbonate is reduced
2 Bromine is oxidised as well as reduced
3 Bromine is reduced and water is oxidised
4 \(\mathrm{\mathrm{Br}_{2}}\) is neither oxidised nor reduced
Explanation:
O.N. of \(\mathrm{\mathrm{Br}}\) in \(\mathrm{\mathrm{Br}_{2}=0}\) \(\mathrm{\mathrm{Br}^{-}=-1}\) \(\mathrm{\mathrm{BrO}_{3}^{-}=+5}\) \(\mathrm{\mathrm{Br}}\) is oxidised as well as reduced.
CHXI08:REDOX REACTIONS
315455
Which reaction does not represent auto redox or disproportionation?
In auto redox or disproportionation, same element is oxidized as well as reduced. In (1) \(\mathrm{\mathrm{Cl}_{2}}\); (2), \(\mathrm{\mathrm{H}_{2} \mathrm{O}_{2}}\) and (3), \(\mathrm{\mathrm{Cu}^{+}}\)is oxidized as well as reduced. In (4), \(\mathrm{\mathrm{N}}\) is oxidized and \(\mathrm{\mathrm{Cr}}\) is reduced in one molecule of \(\mathrm{\left(\mathrm{NH}_{4}\right)_{2} \mathrm{Cr}_{2} \mathrm{O}_{7}}\) and thus it is intramolecular redox.
315457
During the disproportionation of iodine to iodide and iodate ions, the ratio of iodate and iodide ions formed in alkaline medium is
1 \(1: 5\)
2 \(5: 1\)
3 \(3: 1\)
4 \(1: 3\)
Explanation:
\(3 \mathrm{I}_{2}+\underline{6} \mathrm{OH}^{-} \rightarrow \mathrm{IO}_{3}^{-}+5 \mathrm{I}^{-}+3 \mathrm{H}_{2} \mathrm{O}\) So, ratio of iodate to iodide ion is \(1: 5\).
