Using the data given below find out the strongest oxidizing agent.

ECr2O72-/Cr3+=1.33V  ;  ECl2/Cl-=1.36VEMn04-/Mn2+=1.51V    ;  ECr3+/Cr=-0.74V

1.  Cl-

2.  Mn2+

3.  MnO4-

4.  Cr3+

Subtopic:  Electrochemical Series |
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ECr2O72-/Cr3+=1.33V  ;  ECl2/Cl-=1.36VEMn04-/Mn2+=1.51V    ;  ECr3+/Cr=-0.74V

Using the data given above find out in which option the order of reducing power is correct.

1.  Cr3+ < Cl- < Mn2+ < Cr

2.  Mn2+ < Cl- < Cr3+ < Cr

3.  Cr3+ < Cl- < Cr2O72- < MnO4-

4.  Mn2+ < Cr3+ < Cl- < Cr

 

Subtopic:  Electrochemical Series |
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ECr2O72-/Cr3+=1.33V  ;  ECl2/Cl-=1.36VEMn04-/Mn2+=1.51V    ;  ECr3+/Cr=-0.74V

Use the data given above to find out the most stable ion in its reduced form.

1.  Cl- 

2.  Cr3+ 

3.  Cr

4.  Mn2+ 

Subtopic:  Electrochemical Series |
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From the data given below, the most stable oxidized species is : 
\(\begin{aligned} &E_{{\mathrm{Cr}_2 \mathrm{O}_7^2}/ \mathrm{Cr}^{3+}}^{o} =1.33 \mathrm{~V} ; E_{\mathrm{Cl}_2 / \mathrm{Cl}^{-}}^{o}=1.36 \mathrm{~V} \\ &E_{\mathrm{MnO_{4}}^{-} / \mathrm{Mn}^{2+}}^{o}=1.51 \mathrm{~V} ; E_{\mathrm{Cr}^{3+} / \mathrm{Cr}}^{o}=-0.74 \mathrm{~V} \end{aligned}\)

1. Cr3+ 

2. MnO4-

3. Cr2O72-

4. Mn2+ 

Subtopic:  Electrochemical Series |
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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

Subtopic:  Faraday’s Law of Electrolysis |
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The cell constant of a conductivity cell-

1. Changes with the change of electrolyte.

2. Changes with the change of concentration of electrolyte.

3. Changes with the temperature of the electrolyte.

4. Remains constant for a cell.

Subtopic:  Conductance & Conductivity |
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The correct statement about charging of the lead storage battery is -

1. PbSO4 anode is reduced to Pb

2. PbSO4 cathode is reduced to Pb

3. PbSO4 cathode is oxidised to Pb

4. PbSO4 anode is oxidised to PbO2

Subtopic:  Batteries & Salt Bridge |
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\(\Lambda _{m(NH_{4}OH)}^{o}\) is equal to -

1. \(\Lambda _{m(NH_{4}OH)}^{o} \ + \ \Lambda _{m(NH_{4}Cl)}^{o} \ - \ \Lambda _{m(HCl)}^{o}\)
2. \(\Lambda _{m(NH_{4}Cl)}^{o} \ + \ \Lambda _{m(NaOH)}^{o} \ - \ \Lambda _{m(NaCl)}^{o}\)
3. \(\Lambda _{m(NH_{4}Cl)}^{o} \ + \ \Lambda _{m(NaCl)}^{o} \ - \ \Lambda _{m(NaOH)}^{o}\)
4. \(\ \Lambda _{m(NaOH)}^{o} \ + \ \Lambda _{m(NaCl)}^{o}\ - \ \Lambda _{m(NH_{4}Cl)}^{o}\)

Subtopic:   Kohlrausch Law & Cell Constant |
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In the electrolysis of concentrated aqueous sodium chloride solution, the half cell reaction that will occur at the anode is : 

1. Na+(aq) + e- ⟶ Na(s) ; \(E_{cell}^{o} \ = \ -2.71 \ V\)

2. 2H2O(l) ⟶ O2(g) + 4H+(aq) + 4e; \(E_{cell}^{o}\) = 1.23 V

3. H+(aq) + e-\(\frac{1}{2}\)H2(g) ; \(E_{cell}^{o}\) = 0.00 V

4. Cl-(aq) ⟶ \(\frac{1}{2}\)Cl2(g) + e- ; \(E_{cell}^{o}\) 1.36 V

Subtopic:  Electrolytic & Electrochemical Cell |
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The positive value of the standard electrode potential of Cu2+ / Cu indicates that-

a.  This redox couple is a stronger reducing agent than the H+ /H2 couple

b.  This redox couple is a stronger oxidising agent than H+ /H2

c.  Cu can displace H2 from acid.

d.  Cu cannot displace H2 from acid.


1. (a, b)
2. (b, c)
3. (c, d)
4. (b, d)

Subtopic:  Electrochemical Series | Electrolytic & Electrochemical Cell |
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