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Electrochemistry · Question 54

AIPMT 2008MCQEasy📈 Topic in 25% papers+4−1
1

Kohlrausch's law states that at

  1. Infinite dilution, each ion makes definite contribution to conductance of an electrolyte whatever be the nature of the other ion of the electrolyte
  2. Infinite dilution, each ion makes definite contribution to equivalent conductance of an electrolyte, whatever be the nature of the other ion of the electrolyte
  3. Finite dilution, each ion makes definite contribution to equivalent conductance of an electrolyte, whatever be the nature of the other ion of the electrolyte
  4. Infinite dilution, each ion makes definite contribution to equivalent conductance of an electrolyte depending on the nature of the other ion of the electrolyte.

Answer

(1) Infinite dilution, each ion makes definite contribution to conductance of an electrolyte whatever be the nature of the other ion of the electrolyte

Solution

As per NCERT, Kohlrausch's law of independent migration of ions states that the limiting molar conductivity of an electrolyte can be represented as the sum of the individual contributions of the anion and the cation of the electrolyte.

m = + + + - -

The law holds only at infinite dilution, where the ions are far apart and move independently; each ion then makes a definite contribution to the conductance of the electrolyte, whatever the other ion with it is.

At infinite dilution, each ion makes a definite contribution to the conductance of an electrolyte, whatever be the nature of the other ion of the electrolyte.

Answer: (1)

AIPMT 2008

Keep practising — Electrochemistry

2

Standard free energies of formation (in kJ/mol) at 298 K are -237.2, -394.4 and -8.2 for H2O(l), CO2(g) and pentane (g) respectively. The value of E cell for the pentane-oxygen fuel cell is

  1. 1.0968 V
  2. 0.0968 V
  3. 1.968 V
  4. 2.0968 V
AIPMT 2008
3

The equilibrium constant of the reaction: Cu(s) + 2Ag+(aq) Cu2+(aq) + 2Ag(s); E = 0.46 V at 298 K is

  1. 2.0 1010
  2. 4.0 1010
  3. 4.0 1015
  4. 2.4 1010
AIPMT 2007
4

The efficiency of a fuel cell is given by

  1. G/ S
  2. G/ H
  3. S/ G
  4. H/ G
AIPMT 2007
5

A hypothetical electrochemical cell is shown below. A | A+(xM) || B+(yM) | B The emf measured is + 0.20 V. The cell reaction is

  1. A + B+ A+ + B
  2. A+ + B A + B+
  3. A+ + e- A; B+ + e- B
  4. the cell reaction cannot be predicted.
AIPMT 2006
6

E Fe2+/Fe = -0.441 V and E Fe3+/Fe2+ = 0.771 V, the standard EMF of the reaction Fe + 2Fe3+ 3Fe2+ will be

  1. 0.111 V
  2. 0.330 V
  3. 1.653 V
  4. 1.212 V
AIPMT 2006
7

4.5 g of aluminium (at. mass 27 amu) is deposited at cathode from Al3+ solution by a certain quantity of electric charge. The volume of hydrogen produced at STP from H+ ions in solution by the same quantity of electric charge will be

  1. 44.8 L
  2. 22.4 L
  3. 11.2 L
  4. 5.6 L
AIPMT 2005
8

The standard e.m.f. of a galvanic cell involving cell reaction with n = 2 is found to be 0.295 V at 25 C. The equilibrium constant of the reaction would be

  1. 2.0 1011
  2. 4.0 1012
  3. 1.0 102
  4. 1.0 1010
AIPMT 2004
9

The e.m.f. of a Daniell cell at 298 K is E1. [figure] When the concentration of ZnSO4 is 1.0 M and that of CuSO4 is 0.01 M, the e.m.f. changed to E2. What is the relationship between E1 and E2?

  1. E1 > E2
  2. E1 < E2
  3. E1 = E2
  4. E2 = 0 E1
AIPMT 2003
10

On the basis of the information available from the reaction, 4/3 Al + O2 2/3 Al2O3, G = -827 kJ mol-1 of O2, the minimum e.m.f. required to carry out an electrolysis of Al2O3 is ( F = 96500 C mol-1)

  1. 2.14 V
  2. 4.28 V
  3. 6.42 V
  4. 8.56 V
AIPMT 2003
11

In electrolysis of NaCl when Pt electrode is taken then H2 is liberated at cathode while with Hg cathode it forms sodium amalgam because

  1. Hg is more inert than Pt
  2. more voltage is required to reduce H+ at Hg than at Pt
  3. Na is dissolved in Hg while it does not dissolve in Pt
  4. concentration of H+ ions is larger when Pt electrode is taken
AIPMT 2002

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