Calculate the quantity of electricity (i.e. charge) delivered by a Daniel cell initially containing 1L each of 1 M Cu2+ion and 1M Zn2+,which is operated until its potential drops to 1V.
(Given : \(E_{Zn2+/Zn}^0 = -0.76V; E_{Cu2+/Cu}^0 = +0.34V\))
(1) 0.029 x 105C
(2) 2.239 x 105C
(3) 1.92 x 105C
(4) 3.123 x 105C

Subtopic:  Nernst Equation |
 57%
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Some half cell reaction & their standard potential are given which combination would result in a cell with the largest potential.

(i) A+e-  A-        E° =  0.24

(ii) B- + e-  B-2           E° = 1.25

(iii) C- + 2e-  C-3           E -=  1.25

(iv) D + 2e-  D-2            E° = 0.06

(v) E + 4e-E-4           E° = 0.38

(A) i and ii                                                   

(B) ii and iii

(C) iv and v                                                 

(D) ii and v

 

 

Subtopic:  Electrode & Electrode Potential |
 68%
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A hydrogen electrode is immersed in a solution with pH = 0 (HCl). By how much will the potential (reduction) change if an equivalent amount of NaOH is added to the solution. (Take pH2 = 1 atm) T = 298 K.

(1) increase by 0.41 V                             

(2) increase by 59 mV

(3) decrease by 0.41 V                            

(4) decrease by 59 mV

Subtopic:  Electrode & Electrode Potential |
 51%
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The solubility product of silver iodide is 8.3 × 10-17and the standard potential (reduction) of Ag,Ag+ electrode is + 0.800 volts at  25°C.The standard potential of Ag, AgI/I- electrode (reduction) from these data is-

(1) – 0.30 V                            

(2) + 0.15 V

(3) + 0.10 V                            

(4) – 0.15 V

Subtopic:  Relation between Emf, G, Kc & pH |
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How much time is required for the complete decomposition of 2 moles of water using a current of 2 ampere-

1. 26.805 h                                   

2. 53.61 h

3. 107.22 h                                   

4. None of these

Subtopic:  Faraday’s Law of Electrolysis |
 60%
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The standard redox potentials Eof the following systems are-
 

System Eo(Volts)
\(MnO_{4}^{-}+8 H^{+}+5 e \rightarrow M n^{2+}+4 H_{2}O\) 1.51
Sn4+ +   2e-   →   S n2+ 0.15
Cr2O72- + 14H+ +  6e- →  2Cr3+ +  7H2O 1.33
C e4+  +  e- →   Ce3+   1.61

The oxidizing power of the various species decreases in the order-

1. Ce4+>Cr2O72-> Sn4+ > MnO4-

2. Ce4+>MnO4- >Cr2O72-> Sn4+

3. Cr2O72->Sn4+>Ce4++ MnO4-

4. MnO4->Ce4+ > Sn4+>Cr2O72-

Subtopic:  Electrode & Electrode Potential |
 85%
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Calculate the maximum work that can be obtained from the Daniell cell given below -

Zn(s) | Zn2+ (aq) || Cu2+ (aq) | Cu(s).

Given that EZn2+/Zn°=-0.76 V and ECu2+/Cu°=+0.34 V

(1) – 212300 J                                        

(2) – 202100 J

(3) – 513100 J                                        

(4) – 232120 J

 

Subtopic:  Relation between Emf, G, Kc & pH |
 81%
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The metal that cannot be produced on reduction of its oxide by aluminium is :

(1) K                                                        

(2) Mn

(3) Cr                                                      

(4) Fe

Subtopic:  Electrode & Electrode Potential |
 77%
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We have taken a saturated solution of AgBr, Ksp of AgBr is 12 × 10-14.   If 10-7 mole of AgNO3  is added to 1 litre of this solution then the conductivity of this solution in terms of  10-10   Sm-1 units will be:

[λ°Ag+=6×10-3Sm2mol-1 ;
λ°Br-=8×10-3Sm2mol-1,
λ°NO3-=7×10-3Sm2mol-1]

1. 39 
2. 55
3. 15 
4. 41

Subtopic:  Electrode & Electrode Potential |
 65%
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Calculate the e.m.f. for the following cell reaction:
\(F e^{2+}+Z n → Z n^{2+}+F e\)
The standard potentials \(E^{\circ} \text {,for the half reactions are as}\)

\(Z n →Z n^{2+}+2 e ; E^{\circ}=+0.76 \mathrm{~V}\)
\(F e → F e^{2+}+2 e ; E^{\circ}=+0.41 \mathrm{~V}\)

1. – 0.35 V                                            

2. + 0.35 V

3. + 1.17 V                                           

4. – 1.17 V

Subtopic:  Electrode & Electrode Potential |
 65%
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