CBSE Class 12 Electrochemistry Multiple Choice Questions with Answers. MCQ Questions Class 12 Electrochemistry with Answers Is Prepared Based on Latest Exam Pattern. Students can solve NCERT Class 12 Electrochemistry MCQs with Answers to know their preparation level.
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MCQ Questions Class 12 Electrochemistry with Answers - Set - 5
Question 1:
On the basis of the following E° values, the strongest oxidizing agent is
[Fe(CN)6]4– → [Fe(CN)6]3– + e– ; E° = –0.35 V
Fe2+ → Fe3+ + e– ; E° = –0.77 V
(a) Fe3+
(b) [Fe(CN)6]3–
(c) [Fe(CN)6]4–
(d) Fe2+
Correct Answer – (A)
Question 2 :
A solution contains Fe2+, Fe3+ and I– ions. This solution was treated with iodine at 35°C. E° for Fe3+/Fe2+ is + 0.77 V and E° for I2/2I– = 0.536 V. The favourable redox reaction is
(a) I2 will be reduced to I–
(b) there will be no redox reaction
(c) I– will be oxidised to I2
(d) Fe2+ will be oxidised to Fe3+
Correct Answer – (C)
Question 3 :
Standard electrode potentials of three metals X, Y and Z are –1.2 V, + 0.5 V and – 3.0 V respectively.
The reducing power of these metals will be
(a) Y > Z > X
(b) Y > X > Z
(c) Z > X > Y
(d) X > Y > Z
Correct Answer – (C)
Question 4 :
A button cell used in watches function as following :
Zn(s) + Ag2O(s) + H2O(l) ⇌ 2Ag(s) + Zn2+(aq) + 2OH–(aq)
If half cell potentials are
Zn2+(aq) + 2e– → Zn(s); E° = – 0.76 V
Ag2O(s) + H2O(l) + 2e– → 2Ag(s) + 2OH–(aq); E° = 0.34 V
The cell potential will be
(a) 0.84 V
(b) 1.34 V
(c) 1.10 V
(d) 0.42 V
Correct Answer – (C)
Question 5 :
How much time is required to deposit 1 × 10-3 cm thick layer of silver (density of 1.05 g cm-3) on a surface of area 100 cm² by passing a current of 5 A through AgNO3 solution?
(a) 125 s
(b) 115 s
(c) 18.7 s
(d) 27.25 s
Correct Answer – (C)
MCQ Questions Class 12 Electrochemistry with Answers
Question 6:
Consider the following relations for emf of an electrochemical cell
(i) EMF of cell = (Oxidation potential of anode) –(Reduction potential of cathode)
(ii) EMF of cell = (Oxidation potential of anode) + (Reduction potential of cathode)
(iii) EMF of cell = (Reductional potential of anode)+ (Reduction potential of cathode)
(iv) EMF of cell = (Oxidation potential of anode) – (Oxidation potential of cathode)
Which of the above relations are correct?
(a) (iii) and (i)
(b) (i) and (ii)
(c) (iii) and (iv)
(d) (ii) and (iv)
Correct Answer – (D)
Question 7:
Standard electrode potential for Sn4+/Sn2+ couple is +0.15 V and that for the Cr3+/Cr couple is –0.74 V. These two couples in their standard state are connected to make a cell. The cell potential will be
(a) + 1.19 V
(b) + 0.89 V
(c) + 0.18 V
(d) + 1.83 V
Correct Answer – (B)
Question 8:
Standard reduction potentials of the half reactions are given below :
F2(g) + 2e– → 2F–(aq) ; E° = + 2.85 V
Cl2(g) + 2e– → 2Cl–(aq) ; E° = + 1.36 V
Br2(l) + 2e– → 2Br–(aq) ; E° = + 1.06 V
I2(s) + 2e– → 2I–(aq) ; E° = + 0.53 V
The strongest oxidising and reducing agents respectively are
(a) F2 and I–
(b) Br2 and Cl–
(c) Cl2 and Br–
(d) Cl2 and I2
Correct Answer – (A)
Question 9:
The standard electrode potential (E°) values of Al3+/Al, Ag+/Ag, K+/K and Cr3+/Cr are –1.66 V, 0.80 V, –2.93 V and –0.74 V, respectively. The correct decreasing order of reducing power of the metal is
(a) Ag > Cr > Al > K
(b) K > Al > Cr > Ag
(c) K > Al > Ag > Cr
(d) Al > K > Ag > Cr
Correct Answer – (B)
Question 10:
A current of 1.40 ampere is passed through 500 mL of 0.180 M solution of zinc sulphate for 200 seconds. What will be the molarity of Zn2+ions after deposition of zinc?
(a) 0.154 M
(b) 0.177 M
(c) 2 M
(d) 0.180 M
Correct Answer – (B)
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