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Electrochemistry NEET Previous Year Questions

1. 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                    (NEET 2019)

(a) Ag > Cr > Al > K             (b) K > Al > Cr > Ag

(c) K > Al > Ag > Cr             (d) Al > K > Ag > Cr

2.

(NEET 2013)

(a) 0.84 V                                  (b) 1.34 V

(c) 1.10 V                                  (d) 0.42 V

03.

      (Mains 2012)

(a) F2 and I                    (b) Br2 and Cl

(c) Cl2 and Br                 (d) Cl2 and I2

4. 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     (2011)

(a) Y > Z > X

(b) Y > X > Z

(c) Z > X > Y

 (d) X > Y > Z

5. Standard electrode potential for Sn4+/Sn2+couple is +0.15 V and that for the Cr3+ /Couple is –0.74 V. These two couples in their standard state are connected to make a cell. The cell potential will be                                          (2011)

(a) + 1.19 V            (b) + 0.89 V

(c) + 0.18 V            (d) + 1.83 V

6. 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.  (2011)

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+.

7. Consider the following relations for emf of an electrochemical cell            (2011)

(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)

8. 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+

10. Fe2+/Fe = – 0.441 V and E°Fe3+/Fe2+ = 0.771 V, the standard EMF of the reaction Fe + 2Fe3+ → 3Fe2+ will be                                           

(a) 0.111 V                       (b) 0.330 V

(c) 1.653 V                        (d) 1.212 V

17. For a cell involving one electron, E°cell = 0.59 V at 298 K, the equilibrium constant for the cell reaction is                                  (NEET 2019)

(a) 1.0 × 1030                             (b) 1.0 × 102

(c) 1.0 × 105                              (d) 1.0 × 1010