Standard reduction potentials of the half-reactions are given below: 

F2(g) + 2e-2F-(aq) ; E° =+2.85 V 

Cl2(g) + 2e-2Cl-(aq) ; E° =+1.36 V 

Br2(g) + 2e-2Br-(aq) ; E° =+1.06 V 

I2(g) + e-2I-(aq) ; E° =+0.53 V 

The strongest oxidizing and reducing agents, respectively, are: 

1. Br2 and Cl-

2. Cl2 and Br-

3. Cl2 and I2

4. F2 and l-

Subtopic:  Emf & Electrode Potential |
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AIPMT - 2012
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 The strongest oxidising agent among the following is :

1. BrO3/Br2+,Eo=+1.50

2. Fe3+/Fe2+,Eo=+0.76

3. MnO4/Mn2+,Eo=+1.52

4. Cr2O72/Cr3+,Eo=+1.33

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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
Subtopic:  Emf & Electrode Potential |
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NEET - 2019
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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 CuCl2 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 AgNO3 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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