CHAPTER
02
Exercise 1: NCERT Based Topic-wise MCQs
2.0 INTRDUCTION
1. Batteries and fuel cells convert NCERT/ Page-65 / N-32
(a) chemical energy into electrical energy.
(b) electrical energy into chemical energy.
(c) chemical energy into potential energy.
(d) electrical energy into potential energy.
2.1 ELECTROCHEMICAL CELLS
2. Which device converts chemical energy of a spontaneous redox reaction into electrical energy?
(a) Galvanic cell NCERT/ Page-66 / N-33
(b) Electrolytic cell
(c) Daniell cell
(d) Both (a) and (c)
3. Zn(s) ∣ Zn2+ (aq) ∥ Cu2+ (aq) ∣ Cu(s) is The cell is called
(anode) (cathode)
(a) Weston cell
(b) Daniell cell
(c) Calomel cell
(d) Faraday cell
4. In the electrolytic cell, flow of electrons is from NCERT/ Page-66 / N-32
(a) cathode to anode in solution
(b) cathode to anode through external supply
(c) cathode to anode through internal supply
(d) anode to cathode through internal supply
2.2 GALVANIC CELLS
5. Which of the following statements about galvanic cell is incorrect NCERT/ Page-66 / N-33
(a) anode is positive
(b) oxidation occurs at the electrode with lower reduction potential
(c) cathode is positive
(d) reduction occurs at cathode
,6. In which of the following conditions salt bridge is not required in a galvanic cell?NCERT/ Page-67 / N-33
(a) When galvanic cell is used in geyser.
(b) When distance between oxidation half cell and reduction half cell is negligible.
(c) Electrolytic solutions used in both the half cells are of same concentration.
(d) When both the electrodes are dipped in the same electrolytic solution.
7. The tendency of an electrode to lose electrons is known as NCERT/ Page-67 / N-34
(a) electrode potential
(b) reduction potential
(c) oxidation potential
(d) e.m.f.
8. The chemical reaction,
2AgCl(s) + H2 (g) ⟶ 2HCl(aq) + 2Ag(s)
taking place in a galvanic cell is represented by the notation
(a) Pt(s) ∣ H2 (g), 1 bar |1MKCl(aq)|AgCl (s) ∣ Ag (s)
(b) Pt(s) ∣ H2 (g), 1 bar |1MHCl(aq)|1MAg + (aq) ∣ Ag (s)
(c) Pt(s) ∣ H2 (g), 1 bar |1MHCl(aq)|AgCl (s) ∣ Ag (s)
(d) Pt(s) ∣ H2 (g), 1 bar ∣ 1MHCl (aq) ∣ Ag (s) ∣ AgCl (s)
9. For cell representation: NCERT Page-68 / N-33
Cu(s)|Cu2+ (aq)||Ag + (aq)|Ag(s)
Which of the following is correct?
(i) Cu is reducing agent.
(ii) Overall cell reaction is Cu(s) + 2Ag + (aq) ⟶ Cu2+ (aq) + 2Ag(s)
(iii) Cu is cathode
(iv) Ag is anode
(a) (ii), (iii) and (iv)
(b) (ii), (iii) and (iv)
(c) (iii) and (iv)
(d) (i) and (ii)
10. The reference electrode is made by using
(a) ZnCl2
(b) CuSO4
(c) HgCl2
(d) Hg 2 Cl2
11. Standard electrode potential for Sn4+ /Sn2+ couple is +0.15V and that for the Cr 3+ /Cr couple is −0.74V.
These two couples in their standard state are connected to make a cell.
The cell potential will be NCERT/ Page-68 / N-34
(a) +1.19V
(b) +0.89V
(c) +0.18V
(d) +1.83V
12. From the given option identify the electrode in which metal in contact with own ion in solution
(a) Colomel electrode
(b) Pt/Fe2+ , Fe+3
(c) Ag in AgNO3
(d) Gas electrode
,13. Which of the following statements regarding given cell representation is/are correct?
Cd(s)|Cd2+ (aq)||Ag + (aq)|Ag(s)
(i) In the given cell, Cd electrode act as an anode whereas Ag electrode acts as a cathode.
(ii) In the given cell, Cd electrode acts as a cathode whereas Ag electrode acts as a anode.
(iii) 𝐸cell = 𝐸Ag+/Ag − 𝐸Cd2+ /Cd
(a) (i) and (ii)
(b) Only (ii)
(c) Only(i)
(d) (i) and (iii)
14. If salt bridge is removed from two half-cells the voltage
(a) drops to zero
(b) does not change
(c) increases gradually
(d) increases rapidly
2.3 NERNST EQUATION
∘ RT [Mg2+ ]
15. For the given Nernst equation Ecell = Ecell − 2F ln [Ag+]2 NCERT/ Page-70 / N-38
Which of the following representation is correct?
(a) Ag + |Ag||Mg 2+ |Mg
(b) Mg 2+ |Mg||Ag|Ag +
(c) Mg|Mg 2+ ||Ag + |Ag
(d) Mg|Mg 2+ ||Ag|Ag +
16. Standard electrode potential of three metals 𝑋, 𝑌 and 𝑍 are −1.2V, +0.5V and −3.0V, respectively. The
reducing power of these metals will be: NCERT/ Page-71 / N-37
(a) 𝑌 > 𝑍 > 𝑋
(b) 𝑋 > 𝑌 > 𝑍
(c) 𝑍 > 𝑋 > 𝑌
(d) 𝑋 > 𝑌 > 𝑍
17. Standard reduction potentials of the half reactions are given below : NCERT/ Page-71 / N-37
F2 (g) + 2e− → 2F − (aq); 𝐸 ∘ = +2.85V
Cl2 (g) + 2e− → 2Cl− (aq); 𝐸 ∘ = +1.36V
Br2 (l) + 2e− → 2Br(aq); 𝐸 ∘ = +1.06V
I2 (s) + 2e− → 2I − (aq); 𝐸 ∘ = +0.53V
The strongest oxidising and reducing agents respectively are
(a) F2 and I−
(b) Br2 and Cl
(c) Cl2 and Br
(d) Cl2 and I2
18. The value of electrode potential (10−4 M)H+ |H2 (1atm)|Pt at 298K would be NCERT/ Page-70 / N-38
(a) −0.236V
(b) +0.404V
(c) +0.236V
(d) −0.476V
, 19. The electrode potential 𝐸(Zn2+ /Zn) of a zinc electrode at 25∘ C with an aqueous solution of 0.1MZnSO4 is
∘ 2.303𝑅𝑇
[𝐸(Zn 2+ /Zn) = −0.76V. Assume = 0.06 at 298K]. NCERT Page-70 / N-38
𝐹
(a) +0.73
(b) -0.79
(c) -0.82
(d) -0.70
20. For a cell reaction involving two electron change, the standard EMF of the cell is 0.295V at 2∘ C. The
equilibrium constant of the reaction at 25∘ C will be: NCERT Page-74 / N-39
−2
(a) 29.5 × 10
(b) 10
(c) 1 × 1010
(d) 2.95 × 10−10
21. Without losing its concentration; ZnCl2 solution cannot be kept in contact with NCERT Page-71 / N-37
(a) Au
(b) Al
(c) Pb
(d) Ag
22. The oxidation potentials of 𝐴 and 𝐵 are +2.37 and +1.66V respectively. In chemical reactions
(a) 𝐴 will be replaced by 𝐵 NCERT/Page-71 / N-37
(b) 𝐴 will replace 𝐵
(c) 𝐴 will not replace 𝐵
(d) 𝐴 and B will not replace each other
23. For a cell, Cu(s) ∣ Cu2+ (0.001M||Ag + (0.01M) ∣ Ag(s) the cell potential is found to be 0.43V at 298K. The
magnitude of standard electrode potential for Cu2+ /Cu is × 10−2 V.
Θ 2.303RT
[⬚ Given : EAg + /Ag = 0.80V and = 0.06V] NCERT/Page-70 / N-38
F
(a) 0.34
(b) 3.4
(c) 9.2
(d) 34.0
24. According to Nernst equation, which is not correct if 𝑄 = 𝐾𝑐 : NCERT (Page-73 / N-38
(a) 𝐸cell = 0
𝑅𝑇 ∘
(b) ln 𝑄 = 𝐸cell
𝑛𝐹
𝑛𝐹𝐸∘cell
(c) 𝐾𝑐 = 𝑒 𝑅𝑇
∘
(d) 𝐸cell = 𝐸cell
25. For the galvanic cell Zn|Zn2+ (0.1M) ∥ Cu2+ (1.0M)|Cu the cell potential increase if: NCERT/Page-72 / N-38
(a) [Zn2+ ] is increased
(b) [Cu2+ ] is increased
(c) [Cu2+ ] is decreased
(d) surface area of anode is increased
26. For the reaction taking place in the cell: NCERT/ Page-74 / N-40
Pt(s) ∣ H2 (g) ∣ H + (aq) || Ag + (aq) ∣ Ag(s)
02
Exercise 1: NCERT Based Topic-wise MCQs
2.0 INTRDUCTION
1. Batteries and fuel cells convert NCERT/ Page-65 / N-32
(a) chemical energy into electrical energy.
(b) electrical energy into chemical energy.
(c) chemical energy into potential energy.
(d) electrical energy into potential energy.
2.1 ELECTROCHEMICAL CELLS
2. Which device converts chemical energy of a spontaneous redox reaction into electrical energy?
(a) Galvanic cell NCERT/ Page-66 / N-33
(b) Electrolytic cell
(c) Daniell cell
(d) Both (a) and (c)
3. Zn(s) ∣ Zn2+ (aq) ∥ Cu2+ (aq) ∣ Cu(s) is The cell is called
(anode) (cathode)
(a) Weston cell
(b) Daniell cell
(c) Calomel cell
(d) Faraday cell
4. In the electrolytic cell, flow of electrons is from NCERT/ Page-66 / N-32
(a) cathode to anode in solution
(b) cathode to anode through external supply
(c) cathode to anode through internal supply
(d) anode to cathode through internal supply
2.2 GALVANIC CELLS
5. Which of the following statements about galvanic cell is incorrect NCERT/ Page-66 / N-33
(a) anode is positive
(b) oxidation occurs at the electrode with lower reduction potential
(c) cathode is positive
(d) reduction occurs at cathode
,6. In which of the following conditions salt bridge is not required in a galvanic cell?NCERT/ Page-67 / N-33
(a) When galvanic cell is used in geyser.
(b) When distance between oxidation half cell and reduction half cell is negligible.
(c) Electrolytic solutions used in both the half cells are of same concentration.
(d) When both the electrodes are dipped in the same electrolytic solution.
7. The tendency of an electrode to lose electrons is known as NCERT/ Page-67 / N-34
(a) electrode potential
(b) reduction potential
(c) oxidation potential
(d) e.m.f.
8. The chemical reaction,
2AgCl(s) + H2 (g) ⟶ 2HCl(aq) + 2Ag(s)
taking place in a galvanic cell is represented by the notation
(a) Pt(s) ∣ H2 (g), 1 bar |1MKCl(aq)|AgCl (s) ∣ Ag (s)
(b) Pt(s) ∣ H2 (g), 1 bar |1MHCl(aq)|1MAg + (aq) ∣ Ag (s)
(c) Pt(s) ∣ H2 (g), 1 bar |1MHCl(aq)|AgCl (s) ∣ Ag (s)
(d) Pt(s) ∣ H2 (g), 1 bar ∣ 1MHCl (aq) ∣ Ag (s) ∣ AgCl (s)
9. For cell representation: NCERT Page-68 / N-33
Cu(s)|Cu2+ (aq)||Ag + (aq)|Ag(s)
Which of the following is correct?
(i) Cu is reducing agent.
(ii) Overall cell reaction is Cu(s) + 2Ag + (aq) ⟶ Cu2+ (aq) + 2Ag(s)
(iii) Cu is cathode
(iv) Ag is anode
(a) (ii), (iii) and (iv)
(b) (ii), (iii) and (iv)
(c) (iii) and (iv)
(d) (i) and (ii)
10. The reference electrode is made by using
(a) ZnCl2
(b) CuSO4
(c) HgCl2
(d) Hg 2 Cl2
11. Standard electrode potential for Sn4+ /Sn2+ couple is +0.15V and that for the Cr 3+ /Cr couple is −0.74V.
These two couples in their standard state are connected to make a cell.
The cell potential will be NCERT/ Page-68 / N-34
(a) +1.19V
(b) +0.89V
(c) +0.18V
(d) +1.83V
12. From the given option identify the electrode in which metal in contact with own ion in solution
(a) Colomel electrode
(b) Pt/Fe2+ , Fe+3
(c) Ag in AgNO3
(d) Gas electrode
,13. Which of the following statements regarding given cell representation is/are correct?
Cd(s)|Cd2+ (aq)||Ag + (aq)|Ag(s)
(i) In the given cell, Cd electrode act as an anode whereas Ag electrode acts as a cathode.
(ii) In the given cell, Cd electrode acts as a cathode whereas Ag electrode acts as a anode.
(iii) 𝐸cell = 𝐸Ag+/Ag − 𝐸Cd2+ /Cd
(a) (i) and (ii)
(b) Only (ii)
(c) Only(i)
(d) (i) and (iii)
14. If salt bridge is removed from two half-cells the voltage
(a) drops to zero
(b) does not change
(c) increases gradually
(d) increases rapidly
2.3 NERNST EQUATION
∘ RT [Mg2+ ]
15. For the given Nernst equation Ecell = Ecell − 2F ln [Ag+]2 NCERT/ Page-70 / N-38
Which of the following representation is correct?
(a) Ag + |Ag||Mg 2+ |Mg
(b) Mg 2+ |Mg||Ag|Ag +
(c) Mg|Mg 2+ ||Ag + |Ag
(d) Mg|Mg 2+ ||Ag|Ag +
16. Standard electrode potential of three metals 𝑋, 𝑌 and 𝑍 are −1.2V, +0.5V and −3.0V, respectively. The
reducing power of these metals will be: NCERT/ Page-71 / N-37
(a) 𝑌 > 𝑍 > 𝑋
(b) 𝑋 > 𝑌 > 𝑍
(c) 𝑍 > 𝑋 > 𝑌
(d) 𝑋 > 𝑌 > 𝑍
17. Standard reduction potentials of the half reactions are given below : NCERT/ Page-71 / N-37
F2 (g) + 2e− → 2F − (aq); 𝐸 ∘ = +2.85V
Cl2 (g) + 2e− → 2Cl− (aq); 𝐸 ∘ = +1.36V
Br2 (l) + 2e− → 2Br(aq); 𝐸 ∘ = +1.06V
I2 (s) + 2e− → 2I − (aq); 𝐸 ∘ = +0.53V
The strongest oxidising and reducing agents respectively are
(a) F2 and I−
(b) Br2 and Cl
(c) Cl2 and Br
(d) Cl2 and I2
18. The value of electrode potential (10−4 M)H+ |H2 (1atm)|Pt at 298K would be NCERT/ Page-70 / N-38
(a) −0.236V
(b) +0.404V
(c) +0.236V
(d) −0.476V
, 19. The electrode potential 𝐸(Zn2+ /Zn) of a zinc electrode at 25∘ C with an aqueous solution of 0.1MZnSO4 is
∘ 2.303𝑅𝑇
[𝐸(Zn 2+ /Zn) = −0.76V. Assume = 0.06 at 298K]. NCERT Page-70 / N-38
𝐹
(a) +0.73
(b) -0.79
(c) -0.82
(d) -0.70
20. For a cell reaction involving two electron change, the standard EMF of the cell is 0.295V at 2∘ C. The
equilibrium constant of the reaction at 25∘ C will be: NCERT Page-74 / N-39
−2
(a) 29.5 × 10
(b) 10
(c) 1 × 1010
(d) 2.95 × 10−10
21. Without losing its concentration; ZnCl2 solution cannot be kept in contact with NCERT Page-71 / N-37
(a) Au
(b) Al
(c) Pb
(d) Ag
22. The oxidation potentials of 𝐴 and 𝐵 are +2.37 and +1.66V respectively. In chemical reactions
(a) 𝐴 will be replaced by 𝐵 NCERT/Page-71 / N-37
(b) 𝐴 will replace 𝐵
(c) 𝐴 will not replace 𝐵
(d) 𝐴 and B will not replace each other
23. For a cell, Cu(s) ∣ Cu2+ (0.001M||Ag + (0.01M) ∣ Ag(s) the cell potential is found to be 0.43V at 298K. The
magnitude of standard electrode potential for Cu2+ /Cu is × 10−2 V.
Θ 2.303RT
[⬚ Given : EAg + /Ag = 0.80V and = 0.06V] NCERT/Page-70 / N-38
F
(a) 0.34
(b) 3.4
(c) 9.2
(d) 34.0
24. According to Nernst equation, which is not correct if 𝑄 = 𝐾𝑐 : NCERT (Page-73 / N-38
(a) 𝐸cell = 0
𝑅𝑇 ∘
(b) ln 𝑄 = 𝐸cell
𝑛𝐹
𝑛𝐹𝐸∘cell
(c) 𝐾𝑐 = 𝑒 𝑅𝑇
∘
(d) 𝐸cell = 𝐸cell
25. For the galvanic cell Zn|Zn2+ (0.1M) ∥ Cu2+ (1.0M)|Cu the cell potential increase if: NCERT/Page-72 / N-38
(a) [Zn2+ ] is increased
(b) [Cu2+ ] is increased
(c) [Cu2+ ] is decreased
(d) surface area of anode is increased
26. For the reaction taking place in the cell: NCERT/ Page-74 / N-40
Pt(s) ∣ H2 (g) ∣ H + (aq) || Ag + (aq) ∣ Ag(s)
