Standard reduction potentials of the half-reactions are given below:
The strongest oxidizing and reducing agents, respectively, are:
1. and
2. and
3. and
4. and
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The strongest oxidising agent among the following is :
1.
2.
3.
4.
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The standard electrode potential (E°) values of Al3+/ Al, Ag+ / Ag, K+ / K, and Cr3+ / Cr are –1.66 V, 0.80 V, –2.93 V, & –0.79 V respectively. The correct decreasing order of the reducing power of the metal is:
1. | Ag > Cr > Al > K | 2. | K > Al > Cr > Ag |
3. | K > Al > Ag > Cr | 4. | Al > K > Ag > Cr |
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(a) | \(E_{k^+/K}^o = - 2.93\ V\); \(E_{Ag^+/Ag}^o = 0.80\ V\) |
(b) | \(E_{Hg^{2+}/Hg}^o = 0.79\ V\); \(E_{Mg^{2+}/Mg}^o = - 2.37\ V\) |
(c) | \(E_{Cr^{3+}/Cr}^o = -0.74\ V\) |
Based on standard electrode potentials given above, the correct arrangement for increasing order of reducing power of
elements is:
1. | \(\mathrm{Ag}<\mathrm{Hg}<\mathrm{Cr}<\mathrm{Mg}<\mathrm{K} \) |
2. | \(\mathrm{Ag}>\mathrm{Cr}>\mathrm{Mg}>\mathrm{Hg}>\mathrm{K}\) |
3. | \(\mathrm{K}>\mathrm{Mg}<\mathrm{Cr}<\mathrm{Hg}>\mathrm{Ag} \) |
4. | \(\mathrm{K}<\mathrm{Mg}<\mathrm{Cr}<\mathrm{Hg}<\mathrm{Ag}\) |
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The correct statement about electrolysis of an aqueous solution of with Pt electrode is-
1. | Cu2+ ion reduced at the cathode; Cl- ion oxidized at the anode |
2. | Cu2+ ion reduced at the anode; Cl- ion oxidized at the cathode |
3. | Cu2+ ion reduced at the cathode; H2O ion oxidized at the anode |
4. | H2O ion reduced at the cathode; Cl- ion oxidized at the anode |
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The correct statement about the electrolysis of an aqueous solution of with Pt electrode is:
1. | Pt(s) gets oxidized at cathode whereas Ag + ( aq ) gets reduced at anode |
2. | Ag+ (aq) gets reduced at cathode and is oxidized at anode |
3. | Ag+ (aq) gets reduced at cathode whereas water is oxidized at anode |
4. | Ag (s) gets oxidized at cathode whereas H2O is oxidised at anode |
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