Electro Chemistry Model Question Paper

12th Standard EM

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Chemistry

Time : 02:00:00 Hrs
Total Marks : 50
    7 x 1 = 7
  1. The number of electrons that have a total charge of 9650 coulombs is

    (a)

    6.22 ×1023

    (b)

    6.022 ×1024

    (c)

    6.022 ×1022

    (d)

    6.022 ×10−34

  2. The molar conductivity of a 0.5 mol dm-3 solution of AgNO3 with electrolytic conductivity of 5.76 ×10−3 S cm−1at 298 K is

    (a)

    2.88 S cm2mol-1

    (b)

    11.52 S cm2mol-1

    (c)

    0.086 S cm2mol-1

    (d)

    28.8 S cm2 mol -1

  3. During electrolysis of molten sodium chloride, the time required to produce 0.1mol of chlorine gas using a current of 3A is

    (a)

    55 minutes

    (b)

    107.2 minutes

    (c)

    220 minutes

    (d)

    330 minutes

  4. Which of the following electrolytic solution has the least specific conductance

    (a)

    2N

    (b)

    0.002N

    (c)

    0.02N

    (d)

    0.2N

  5. Zinc can be coated on iron to produce galvanized iron but the reverse is not possible. It is because

    (a)

    Zinc is lighter than iron

    (b)

    Zinc has lower melting point than iron

    (c)

    Zinc has lower negative electrode potential than iron

    (d)

    Zinc has higher negative electrode potential than iron

  6. A conductivity cell has been calibrated with a 0.01M, 1:1 electrolytic solution (specific conductance ( k =1.25x10-3cm-1) in the cell and the measured resistance was 800 Ω at 25oC. The cell constant is,

    (a)

    10−1 cm−1

    (b)

    101 cm−1

    (c)

    1 c m−1

    (d)

    5.7x10-12

  7. Conductivity of a saturated solution of a sparingly soluble salt AB (1:1 electrolyte) at 298K is 1.85 ×10−5 S m−1. Solubility product of the salt AB at 298K (Aom)AB = 14 ×10−3Sm2 mol−1.

    (a)

    5.7 x10 -12

    (b)

    1.32×10−12

    (c)

    7.5 ×10−12

    (d)

    1.74 x10 -12

  8. 7 x 2 = 14
  9. Define anode and cathode

  10. Describe the electrolysis of molten NaCl using inert electrodes

  11. State Faraday’s Laws of electrolysis

  12. Why is anode in galvanic cell considered to be negative and cathode positive electrode?

  13. Which of 0.1M HCl and 0.1 M KCl do you expect to have greater and why?

  14. A conductivity cell has two platinum electrodes separated by a distance 1.5 cm and the
    cross sectional area of each electrode is 4.5 sq cm. Using this cell, the resistance of 0.5 N electrolytic solution was measured as 15 Ω . Find the specific conductance of the solution.

  15. The resistance of a conductivity cell is measured as 190 Ω using 0.1M KCl solution (specific conductance of 0.1M KCl is 1.3 Sm-1) . When the same cell is filled with 0.003M sodium chloride solution, the measured resistance is 6.3KΩ. Both these measurements are made at a particular temperature. Calculate the specific and molar conductance of NaCl solution. Given that

  16. 3 x 3 = 9
  17. Why is AC current used instead of DC in measuring the electrolytic conductance?

  18. A current of 1.608A is passed through 250 mL of 0.5M solution of copper sulphate for 50 minutes. Calculate the strength of Cu2+ after electrolysis assuming volume to be constant and the current efficiency is 100%.

  19. Two metals M1 and M2 have reduction potential values of -xV and +yV respectively. Which will liberate H2 and H2SO4.

  20. 4 x 5 = 20
  21.  Calculate the standard emf of the cell: Cd|Cd2+||Cu2+|Cu and determine the cell reaction.
    The standard reduction potentials of Cu2+|Cu and Cd2+|Cd  are 0.34V and -0.40 volts
    respectively. Predict the feasibility of the cell reaction.

  22. 0.1M copper sulphate solution in which copper electrode is dipped at 250C . Calculate the electrode potential of copper. [Given: E0Cu2+|Cu=0.34].

  23. Derive an expression for Nernst equation

  24. Explain the function of H2 - O2 fuel cell.

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