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Worksheet for Class 12 Chemistry Unit 3 Electrochemistry
Class 12 Chemistry students should refer to the following printable worksheet in Pdf for Unit 3 Electrochemistry in Class 12. This test paper with questions and answers for Class 12 will be very useful for exams and help you to score good marks
Class 12 Chemistry Worksheet for Unit 3 Electrochemistry
Important Questions for NCERT Class 12 Chemistry Electrochemistry
Question. Given that the standard reduction potentials for M+/M and N+/N electrodes at 298 K are 0.52 V and 0.25 V respectively. Which of the following is correct in respect of the following electrochemical cell ? M/M+ | | N+/N
(a) The overall cell reaction is a spontaneous reaction.
(b) The standard EMF of the cell is – 0.27 V.
(c) The standard EMF of the cell is 0.77 V.
(d) The standard EMF of the cell is – 0.77 V.
Question. The specific conductance of a 0.1 N KCl solution at 23°C is 0.012 ohm–1 cm–1. The resistance of cell containing the solution at the same temperature was found to be 55 ohm. The cell constant will be
(a) 0.918 cm–1
(b) 0.66 cm–1
(c) 1.142 cm–1
(d) 1.12 cm–1
Question. On heating one end of a piece of a metal, the other end becomes hot because of
(a) energised electrons moving to the other end
(b) minor perturbation in the energy of atoms
(c) resistance of the metal
(d) mobility of atoms in the metal.
Question. On electrolysis of dil. sulphuric acid using platinum (Pt) electrode, the product obtained at anode will be
(a) hydrogen gas
(b) oxygen gas
(c) H2S gas
(d) SO2 gas.
Question. 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
Question. 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
Question. 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
Question. 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
Question. 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
Question. 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+.
Question. 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)
Question. 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+
Please click the link below to download full pdf file for CBSE Class 12 Chemistry Electrochemistry Commercial Cells.
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CBSE Class 12 Chemistry Unit 3 Electrochemistry Worksheet
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Worksheet for Chemistry CBSE Class 12 Unit 3 Electrochemistry
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Unit 3 Electrochemistry worksheet Chemistry CBSE Class 12
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Unit 3 Electrochemistry CBSE Class 12 Chemistry Worksheet
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Worksheet for CBSE Chemistry Class 12 Unit 3 Electrochemistry
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