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If an iron rod is dipped in CuSO₄ solution, then:
1. Blue colour of the solution turns red.
2. Brown layer is deposited on iron rod.
3. No change occurs in the colour of the solution.
4. None of the above.

When 0.1 mol MnO₄^2– is oxidized, the quantity of electricity required to completely oxidise MnO₄^2– to MnO₄^– is:

Calculate the emf of the given cell: 
Zn(s) | Zn⁺² (0.1M) || Sn⁺² (0.001M) | Sn(s)
(Given ${\mathrm{E}}_{{\mathrm{Zn}}^{+2}/\mathrm{Zn}}^{\mathrm{o}}=-0.76$ $\mathrm{V},$ ${\mathrm{E}}_{{\mathrm{Sn}}^{2+}/\mathrm{Sn}}^{\mathrm{o}}=-0.14$ $\mathrm{V)}$
1. 0.62 V
2. 0.56 V
3. 1.12 V
4. 0.31 V

The potential of a hydrogen electrode having a pH = 10 is : 
1. 0.59 V
2. –0.59 V
3.  0.0 V
4. –5.9 V

The equilibrium constant of a 2 electron redox reaction at 298 K is 3.8 x ${10}^{-3}$. The cell potential E^o (in V) and the free energy change ∆G^o (in kJ mol^-1 ) for this equilibrium respectively, are -

Aluminium metal can be produced by the electrolysis of molten aluminium oxide at about 1000 °C.
The cathode reaction is: \(Al^{3 +} + 3 e^{-} \rightarrow Al\)
Given that the atomic mass of aluminium is 27 amu and 1 Faraday = 96,500 C, calculate the quantity of electricity (in coulombs) required to produce 5.12 kg of aluminium by this method:
1. \(5 . 49 \times 10^{1 } C\) of electricity
2. \(5 . 49 \times 10^{4 } C\) of electricity
3. \(1 . 83 \times 10^{7 } C\) of electricity
4. \(5 . 49 \times 10^{7 } C\) of electricity

For the cell, Ti/Ti⁺(0.001M)||Cu²⁺(0.1M)|Cu, ${\mathrm{E}}_{\mathrm{cell}}^{\mathrm{o}}$ $$at
25 $°$C is 0.83 V. E_cell can be increased :
1. By increasing [Cu²⁺]
2. By increasing [Ti⁺]
3. By decreasing [Cu²⁺]
4. None of the above.

The electrode potential of Cu electrode dipped in 0.025 M CuSO₄ solution at 298 K is:
(standard reduction potential of Cu = 0.34 V)
1. 0.047 V
2. 0.293 V
3. 0.35 V
4. 0.387 V

\(Cu(s)|Cu^{+2}(10^{-3} \ M) \ || \ Ag^{+}(10^{-5} \ M)|Ag(s)\)
if \(E_{Cu^{+2}/Cu}^{o} \ = \ +0.34 \ V\), and \(E_{Ag^{+}/Ag}^{o} \ = \ +0.80 \ V\)
E_cell will be: 
1. 0.46 V
2. \(0.46-\frac{RT}{2F}ln10^{7}\)
3. \(0.46+\frac{RT}{2F}ln10^{7}\)
4. \(0.46-\frac{RT}{2F}ln10^{2}\)

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

A fuel cell develops an electrical potential from the combustion of butane at 1 bar and 298 K 
C₄H₁₀(g) + 6.5O₂(g) → 4 CO₂(g) + 5H₂O(l); E^o  of a cell is: 
(Given \(\Delta G^{o}\) \(= - 2746  k J / m o l e\) )
1. 4.74 V
2. 0.547 V
3. 4.37 V
4. 1.09 V

A gas X at 1 atm is bubbled through a solution containing a mixture of 1 M Y^- and 1 M Z^- at 25 ^oC . If the reduction potential of Z > Y > X, then:

The number of Faradays required to produce 20.0 g of Ca from molten CaCl₂ is-
1. 2F
2. 1F
3. 4F
4. 3F

The cell that will measure the standard electrode potential of a copper electrode is:

The electrode potential for the 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 E_{Mg²⁺ / Mg} vs log [Mg²⁺] among the following is:

1.		2.
3.		4.

The correct statement among the following options is: 

The difference between the electrode potentials of two electrodes when no current is drawn through the cell is called:
1. Cell potential.
2. Cell emf.
3. Potential difference.
4. Cell voltage.

An electrochemical cell behaves as an electrolytic cell when the externally applied potential (Eext)
becomes greater than the cell potential (Ecell). Which of the following conditions is correct?
1. E_cell = 0
2. E_cell > E_ext
3. E_ext > E_cell
4. E_cell = E_ext

The most stable oxidized species among the following is: 
\(E_{{\mathrm{Cr}_2 \mathrm{O}_7^2}/ \mathrm{Cr}^{3+}}^{o} =1.33 \mathrm{~V} ; E_{\mathrm{Cl}_2 / \mathrm{Cl}^{-}}^{o}=1.36 \mathrm{~V} \)
\( E_{\mathrm{MnO_{4}}^{-} / \mathrm{Mn}^{2+}}^{o}=1.51 \mathrm{~V} ; E_{\mathrm{Cr}^{3+} / \mathrm{Cr}}^{o}=-0.74 \mathrm{~V}\)

The quantity of charge required to obtain one mole of aluminium from Al₂O₃ is :
1.  1 F
2.  6 F
3.  3 F
4.  2 F