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प्रश्न
Which method can be used to find out strength of reductant/oxidant in a solution? Explain with an example.
उत्तर
We can Measure the electrode potential of the given species by connecting the redox couple of the given species with standard hydrogen electrode. If it is positive, the electrode of the given species acts as reductant and if it is negative, it acts as an oxidant. Find the electrode potentials of the other given species in the same way, compare the values and determine their comparative strength as an reductant or oxidant. Example Measurement of standard electrode potential of electrode \[\ce{E^Θ_{Zn^{2+}/Zn}}\] using SHE as a reference electrode.
Types of Redox Reactions
The different types of Redox Reactions are:
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Decomposition Reaction
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Combination Reaction
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Displacement Reaction
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Disproportionation Reactions
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संबंधित प्रश्न
The more positive the value of EΘ, the greater is the tendency of the species to get reduced. Using the standard electrode potential of redox couples given below find out which of the following is the strongest oxidising agent.
EΘ values: \[\ce{Fe^{3+} / Fe^{2+} = + 0.77; I2 (s) / I- = + 0.54}\];
\[\ce{Cu^{2+} / Cu = + 0.34; Ag+ / Ag = + 0.80V}\]
Using the standard electrode potential, find out the pair between which redox reaction is not feasible.
EΘ values: \[\ce{Fe^{3+} / Fe^{2+} = + 0.77; I2/I- = + 0.54}\];
\[\ce{Cu^{2+} / Cu = + 0.34; Ag+ / Ag = + 0.80 V}\]
Thiosulphate reacts differently with iodine and bromine in the reactions given below:
\[\ce{2S2O^{2-}3 + I2 -> S4O^{2-}6 + 2I-}\]
\[\ce{S2O^{2-}3 + 2Br2 + 5H2O -> 2SO^{2-}4 + 2Br- + 10H+}\]
Which of the following statements justifies the above dual behaviour of thiosulphate?
Identify the correct statement (s) in relation to the following reaction:
\[\ce{Zn + 2HCl -> ZnCl2 + H2}\]
(i) Zinc is acting as an oxidant.
(ii) Chlorine is acting as a reductant.
(iii) Hydrogen ion is acting as an oxidant.
(iv) Zinc is acting as a reductant.
Which of the following electrodes will act as anodes, when connected to Standard Hydrogen Electrode?
(i) \[\ce{Al/Al^{3+}; E^Θ = –1.66}\]
(ii) \[\ce{Fe/Fe^{2+}; E^Θ = – 0.44}\]
(iii) \[\ce{Cu/Cu2+ ; E^Θ = + 0.34}\]
(iv) \[\ce{F2 (g)/2F– (aq); E^Θ = + 2.87}\]
On the basis of standard electrode potential values, suggest which of the following reactions would take place? (Consult the book for EΘ value).
\[\ce{Cu + Zn^{2+} -> Cu^{2+} + Zn}\]
On the basis of standard electrode potential values, suggest which of the following reactions would take place? (Consult the book for EΘ value).
\[\ce{Mg + Fe^{2+} -> Mg^{2+} + Fe}\]
On the basis of standard electrode potential values, suggest which of the following reactions would take place? (Consult the book for EΘ value).
\[\ce{Br2 + 2Cl- -> Cl2 + 2Br-}\]
On the basis of standard electrode potential values, suggest which of the following reactions would take place? (Consult the book for EΘ value).
\[\ce{Fe + Cd^{2+} -> Cd + Fe^{2+}}\]
Strongest reducing agent is ______.
