Tiêu đề 16.ELECTROCHEMISTRY.pdf ✅

UNIT 02 ELECTROCHEMISTRY 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+ (anode) (aq) ∥ Cu2+(aq) (cathode) ∣ Cu(s) is The cell is called (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) Hg2Cl2 11. Standard electrode potential for Sn4+/Sn2+ couple is +0.15V and that for the Cr3+/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? NCERT/ Page-68 / N-34 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