Which of the following is $NOT$ a redox reaction?
- A$CH_3CHO + 2Cu(OH)_2 \longrightarrow CH_3COOH + Cu_2O + 2H_2O$
- B$SnCl_4 + FeCl_2 \longrightarrow FeCl_3 + SnCl_2$
- C$H_2SO_4 + Ca(OH)_2 \longrightarrow CaSO_4 + 2H_2O$
- D$C_2H_5OH + [O] \longrightarrow CH_3CHO + H_2O$
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Consider the reactions:
$2S_2O_3^{2-}(aq) + I_2(s) \to S_4O_6^{2-}(aq) + 2I^-(aq)$
$S_2O_3^{2-}(aq) + 2Br_2(l) + 5H_2O(l) \to 2SO_4^{2-}(aq) + 4Br^-(aq) + 10H^+(aq)$
Why does the same reductant,thiosulphate,react differently with iodine and bromine?
$2S_2O_3^{2-}(aq) + I_2(s) \to S_4O_6^{2-}(aq) + 2I^-(aq)$
$S_2O_3^{2-}(aq) + 2Br_2(l) + 5H_2O(l) \to 2SO_4^{2-}(aq) + 4Br^-(aq) + 10H^+(aq)$
Why does the same reductant,thiosulphate,react differently with iodine and bromine?
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View SolutionIn acidic medium,one mole each of $MnO_4^-$ and $Cr_2O_7^{2-}$ is reduced by $x$ and $y$ moles of ferrous ions $(Fe^{2+})$ respectively. The sum of $x$ and $y$ is:
$KI$ is oxidised into $I_2$ by using the reagent
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View Solution$A$ solution of $KMnO_{4}$ on reduction yields either a colourless solution,a brown precipitate,or a green solution depending on the $pH$ of the solution. What different stages of the reduction do these represent and how are they carried out?
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View SolutionHot concentrated sulphuric acid is a moderately strong oxidizing agent. Which of the following reactions does not show oxidizing behaviour?
MediumNEET 2016
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