Advertisements
Advertisements
प्रश्न
Justify that the following reaction is redox reaction; identify the species oxidized/reduced, which acts as an oxidant and which acts as a reductant.
\[\ce{I2_{(aq)} + 2S2O^{2-}_{3(aq)}->S4O^{2-}_{6(aq)} + 2I^-_{ (aq)}}\]
Advertisements
उत्तर
\[\ce{I2_{(aq)} + 2S2O^{2-}_{3(aq)}->S4O^{2-}_{6(aq)} + 2I^-_{ (aq)}}\]
- Write oxidation number of all the atoms of reactants and products.
- Identify the species that undergoes a change in oxidation number.
- The oxidation number of S increases from +2 to +2.5 and that of I decreases from 0 to –1. Because oxidation number of one species increases and that of the other decreases, the reaction is a redox reaction.
- The oxidation number of S increases by loss of electrons and therefore, S is a reducing agent and itself is oxidized. On the other hand, the oxidation number of I decreases by a gain of electrons, and therefore, I is an oxidizing agent and itself is reduced.
Result:
- The given reaction is a redox reaction.
- Oxidant/oxidizing agent (Reduced species): I2
- Reductant/reducing agent (Oxidized species): \[\ce{S2O^2-_3}\]
APPEARS IN
संबंधित प्रश्न
Choose the correct option.
Oxidation number of oxygen in superoxide is
Choose the correct option.
The process \[\ce{SO2->S2Cl2}\] is
In which chemical reaction does carbon exhibit variation of oxidation state from - 4 to + 4? Write a balanced chemical reaction.
In which reaction does nitrogen exhibit variation of oxidation state from –3 to +5?
Calculate the oxidation number of the underlined atom.
K2C2O4
Identify the following pair of species is in its oxidized state?
Cu/Cu2+
Provide the stock notation for the following compound:
HAuCl4
Provide the stock notation for the following compound:
FeO
Assign oxidation number atom in the following species.
H3BO3
Which of the following redox couple is a stronger reducing agent?
Li (E0 = - 3.05 V) and Mg (E0 = - 2.36 V)
Which of the following redox couple is a stronger reducing agent?
Zn (E0 = - 0.76 V) and Fe (E0 = - 0.44 V)
Complete the following table:
Assign oxidation number to the underlined species and write Stock notation of compound
| Compound | Oxidation number | Stock notation |
| AuCl3 | ||
| SnCl2 | ||
| \[\ce{\underline{{V}}_2O^{4-}_{7}}\] | ||
| \[\ce{\underline{{Pt}}Cl^2-_6}\] | ||
| H3AsO3 |
The oxidation number of oxygen in peroxides is ____________.
What is the oxidation number of As in H3AsO3?
In the complex [Co(en)3]Cl3, ____________.
In the following reaction, the oxidation number of Cr changes.
\[\ce{ClO^-_{( aq)} + Cr(OH)^-_{4(aq)} -> CrO^{2-}_{4(aq)} + Cl^-_{( aq)} (basic)}\]
The oxidation number of sulphur in S8 molecule is ______.
In which of the following, oxidation number of oxygen is +2?
All of these are CORRECT for the complex K4[Mn(CN)6], EXCEPT:
Stock notations are used to specify the oxidation numbers of ____________.
The sum of oxidation number of all atoms in \[\ce{SnO^{2-}_3}\] ion is _______.
The oxidation number of Cr in \[\ce{Cr(OH)^-_4}\] ion is ______.
What is the oxidation state of chlorine atom in perchloric acid?
The brown ring complex is formulated as [Fe(H2O)5NO]SO4. The oxidation number of iron is ______.
Which of the following explanation is correct about the given below reaction?
\[\ce{Cr2O^2-_7 + H2O -> 2CrO^2-_4 + 2H+}\]
