After balancing the reaction $Cu + HNO_3 \rightarrow Cu(NO_3)_2 + NO_2 + H_2O$ in an acidic medium,the number of nitrogen atoms,the number of water molecules,and the net charge on the product side are respectively:
- A$3, 2, 0$
- B$6, 3, 0$
- C$4, 2, 2$
- D$4, 2, 0$
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Identify the elements undergoing reduction and oxidation respectively in the following redox reaction.
$3 H_3AsO_{3(aq)} + BrO_{3(aq)}^{-} \rightarrow Br_{(aq)}^{-} + 3 H_3AsO_{4(aq)}$
$3 H_3AsO_{3(aq)} + BrO_{3(aq)}^{-} \rightarrow Br_{(aq)}^{-} + 3 H_3AsO_{4(aq)}$
Which of the following reactions is a redox reaction?
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View SolutionIn the reduction of dichromate by $Fe(II)$,the number of electrons involved per chromium atom is:
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View Solution$KMnO_4$ acts as an oxidising agent in acidic medium. The number of moles of $KMnO_4$ that will be needed to react with one mole of sulphide ion $(S^{2-})$ in acidic solution is . . . . . . (in $/5$)?
The product of oxidation of $I^-$ ion by $MnO_4^-$ in alkaline medium is
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