In the electrochemical cell: 
  Zn | ZnSO4 (0.01 M) || CuSO4(1.0 M) | Cu, the emf of this Daniel cell is E1. When the concentration of ZnSO4 is changed to 1.0 M and that of CuSO4 is changed to 0.01 M, the emf changes to E2. From the following, which one is the relationship between E1 and E2
(Given, \(\frac{RT}{F}\) = 0.059)

1. E1<E2

2. E1>E2

3. E2=0E1

4. E1=E2

Subtopic:  Electrode & Electrode Potential | Nernst Equation |
 68%
From NCERT
NEET - 2017
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Two half cell reactions are given below:
\(\begin{aligned} &\mathrm{Co}^{3+}+e^{-} \rightarrow \mathrm{Co}^{2+}, \mathrm{E}_{\mathrm{Co}^{2+} / \mathrm{Co}^{3+}}^{\circ}=-1.81 \mathrm{~V} \\ &2 \mathrm{Al}^{3+}+6 e^{-} \rightarrow 2 \mathrm{Al}(\mathrm{s}), \mathrm{E}_{\mathrm{Al} / \mathrm{Al}^{3+}}^{\circ}=+1.66 \mathrm{~V} \end{aligned} \)
The standard EMF of a cell with feasible redox reaction will be:

1. +7.09 V 2. +0.15 V
3. +3.47 V 4. –3.47 V
Subtopic:  Electrode & Electrode Potential |
 64%
From NCERT
NEET - 2022
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The electrode potential for Mg electrode varies according to the equation

\(E_{Mg^{2+}/Mg}\ = \ E_{Mg^{2+}/Mg}^{o} \ - \ \frac{0.059}{2}log\frac{1}{[Mg^{2+}]}\)

The graph of EMg2+ / Mg vs log [Mg2+] among the following is:

1.    2.  
3.    4.  
Subtopic:  Nernst Equation |
 60%
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Consider the following cell reaction 

2Fe(s) + O2(g) + 4H+(aq)  2Fe2+(aq) + 2H2O(l)

E° = 1.67 V, At [Fe2+] = 10-3 M, PO2 = 0.1 atm and pH = 3, the cell potential at 25 °C is : 

1. 1.27 V

2. 1.77 V

3. 1.87 V

4. 1.57 V

Subtopic:  Nernst Equation |
 57%
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Standard electrode potential for the cell with cell reaction
Zn(s) + Cu2+(aq) → Zn2+(aq) + Cu(s)
is 1.1 V. Calculate the standard Gibbs energy change for the cell reaction.
(Given F = 96487 C mol-1)
1. -200.27 kJ mol-1 2. -212.27 kJ mol-1
3. -212.27 J mol-1 4. -200.27 J mol-1
Subtopic:  Relation between Emf, G, Kc & pH |
 80%
From NCERT
NEET - 2022
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The value of E0 cell for the following reaction is:
\(Cu^{2+}+ Sn^{2+}\to Cu +Sn^{4+ } \)

(Given, equilibrium constant is 106)

1. 0.17 2. 0.01
3. 0.05 4. 1.77
Subtopic:  Electrode & Electrode Potential |
 73%
From NCERT
AIPMT - 1999
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On the basis of the information available from the reaction:

43Al+O223Al2O3, G=-827 KJ mol-1

The minimum e.m.f. required to carry out the electrolysis of Al2O3 is:
(F = 96500 C mol–1)

1. 2.14 V

2. 4.28 V

3. 6.42 V

4. 8.56 V

Subtopic:  Electrode & Electrode Potential |
 65%
From NCERT
AIPMT - 2003
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The potential of hydrogen electrode in contact with a solution with pH =10, is -


1. −0.0591 V
2. −5.91 V
2. 0.0591 V
4. −0.591 V
Subtopic:  Relation between Emf, G, Kc & pH |
 73%
From NCERT
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The most stable oxidized species among the following is: 
\(E_{{\mathrm{Cr}_2 \mathrm{O}_7^2}/ \mathrm{Cr}^{3+}}^{o} =1.33 \mathrm{~V} ; E_{\mathrm{Cl}_2 / \mathrm{Cl}^{-}}^{o}=1.36 \mathrm{~V} \)
\( E_{\mathrm{MnO_{4}}^{-} / \mathrm{Mn}^{2+}}^{o}=1.51 \mathrm{~V} ; E_{\mathrm{Cr}^{3+} / \mathrm{Cr}}^{o}=-0.74 \mathrm{~V}\)

1. Cr3+  2. MnO4-
3. Cr2O72- 4. Mn2+ 
Subtopic:  Electrochemical Series |
 59%
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The standard reduction potential of Zn2+/Zn  and Cu2+/Cu  is -0.76 and +0.34 V respectively. The oxidising agent and reducing agent, respectively, are 
1. Cu & Zn2+ 2. Zn & Cu
3. Cu2+ & Zn2+ 4. Cu2+ & Zn
Subtopic:  Electrochemical Series |
 66%
From NCERT
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