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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: \[\ce{Fe^{3+} / Fe^{2+} = + 0.77; I2 (s) / I- = + 0.54}\];
\[\ce{Cu^{2+} / Cu = + 0.34; Ag+ / Ag = + 0.80V}\]
विकल्प
\[\ce{Fe^{3+}}\]
\[\ce{I2(s)}\]
\[\ce{Cu^{2+}}\]
\[\ce{Ag+}\]
उत्तर
\[\ce{Ag+}\]
Explanation:
The strongest oxidising agent means it has greater tendency to oxidise other species and itself gets easily reduced. So higher the EΘ values, stronger is the oxidising agent it is. Thus, \[\ce{Ag+}\] having highest EΘ positive value among the given systems, is the strongest oxidising agent.
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संबंधित प्रश्न
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).
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\[\ce{Mg + Fe^{2+} -> Mg^{2+} + Fe}\]
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).
\[\ce{Fe + Cd^{2+} -> Cd + Fe^{2+}}\]
Which method can be used to find out strength of reductant/oxidant in a solution? Explain with an example.
Strongest reducing agent is ______.
