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 numbers of Cl atoms marked as Cla and Clb in CaOCl2 (bleaching powder) are
\[\begin{array}{cc} \ce{Cl^{{a}}}\phantom{.} \\/\phantom{...} \\ \ce{Ca}\phantom{......} \\ \backslash\phantom{..} \\\phantom{........} \ce{O-Cl^{{b}}}\phantom{.} \end{array}\]
Choose the correct option.
Oxidation number of carbon in H2CO3 is
Choose the correct option.
Which of the following halogens does always show oxidation state -1?
Calculate the oxidation number of the underlined atom.
H2S4O6
Justify that the following reaction is redox reaction; identify the species oxidized/reduced, which acts as an oxidant and which acts as a reductant.
\[\ce{HF_{(aq)} + {OH}^-_{ (aq)}->H2O_{(l)} + {F}^ -_{ (aq)}}\]
Identify the following pair of species is in its oxidized state?
Cl2/Cl−
Justify the following reaction as a redox reaction.
\[\ce{2Na_{(s)} + S_{(s)} -> Na2S_{(s)}}\]
Find out the oxidizing and reducing agents.
Provide the stock notation for the following compound:
Tl2O
Provide the stock notation for the following compound:
FeO
Assign oxidation number atom in the following species.
Na2S2O3
Which of the following redox couple is a stronger oxidizing agent?
\[\ce{MnO^Θ_4}\](E0 = 1.51 V) and \[\ce{Cr2O^{2Θ}_7}\](E0 = 1.33 V)
Which of the following redox couple is a stronger reducing agent?
Zn (E0 = - 0.76 V) and Fe (E0 = - 0.44 V)
The following statements are CORRECT, EXCEPT:
Which of the following is CORRECT?
\[\ce{H3PO4_{(aq)} + 3KOH_{(aq)} -> K3PO4_{(aq)} + 3H2O_{(l)}}\]
Which of the following is NOT an example of redox reaction?
In the complex [Co(en)3]Cl3, ____________.
Oxidation state of nitrogen in nitric oxide is ______.
In which among the following compounds, oxidation number of nitrogen is + 5?
Stock notations are used to specify the oxidation numbers of ____________.
The sum of oxidation states of all atoms in \[\ce{SnO^{2-}_2}\] and CO2 are ____________ respectively.
Which of the following is INCORRECT?
What is the oxidation number of Carbon in K2C2O4?
Carbon is present in highest oxidation number in ______.
The oxidation number of Cr in \[\ce{Cr(OH)^-_4}\] ion is ______.
The oxidation number of phosphorous in Ba(H2PO2)2 is ______.
Which of the following explanation is correct about the given below reaction?
\[\ce{Cr2O^2-_7 + H2O -> 2CrO^2-_4 + 2H+}\]
Among group 16 elements, which one does not show −2 oxidation state?
