In the electrochemical cell:
$$\mathrm{Z n \left|\right. Z n S O_{4} \left(\right. 0 . 01 M \left.\right) \left|\right. \left|\right. C u S O_{4} \left(\right. 1 . 0 M \left.\right) \left|\right. C u},$$
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. $$\mathrm{E_{1} < E_{2}}$$

2. $$\mathrm{E_{1} > E_{2}}$$

3. $$\mathrm{E_{2} = 0 \neq E_{1}}$$

4. $$\mathrm{E_{1} = E_{2}}$$

Subtopic:  Electrode & Electrode Potential | Nernst Equation |
69%
From NCERT
NEET - 2017
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Two half cell reactions are given below:
\begin{aligned} &\mathrm{{Co}^{3+}+e^{-} \rightarrow {Co}^{2+}, {E}_{{Co}^{2+} / {Co}^{3+}}^{\circ}=-1.81 {~V}} \\ &2 \mathrm{{Al}^{3+}+6 e^{-} \rightarrow 2 {Al}({s}), {E}_{{Al} / {Al}^{3+}}^{\circ}=+1.66 {~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 |
66%
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%
From NCERT
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Consider the following cell reaction

2Fe(s) + ${\mathrm{O}}_{2}$(g) + 4${\mathrm{H}}^{+}$(aq) $\to$ 2${\mathrm{Fe}}^{2+}$(aq) + 2${\mathrm{H}}_{2}\mathrm{O}$(l)

E° = 1.67 V, At [${\mathrm{Fe}}^{2+}$] = 10${}^{-3}$ M, ${\mathrm{P}}_{{\mathrm{O}}_{2}}$ = 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 |
56%
From NCERT
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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 |
81%
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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Consider the following  reaction:

$\frac{4}{3}\mathrm{Al}+{\mathrm{O}}_{2}\to \frac{2}{3}{\mathrm{Al}}_{2}{\mathrm{O}}_{3},$ $∆\mathrm{G}=-827$ $\mathrm{KJ}$ ${\mathrm{mol}}^{-1}$

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 |
66%
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 3 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%
From NCERT
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