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Electrochemistry

Short Answer Type

91. What is the effect of an increase in the concentration of zinc ions on the electrode potential of zinc electrode for which E° equals – 0.76 V?

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92. What is a primary cell? Give an example.

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93. Express the relation between conductivity and molar conductivity of a solution.

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Long Answer Type

94. Explain with examples the terms weak and strong electrolytes. How can these be distinguished?

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95.
Predict the products of electrolysis in each of the following:
(i) An aqueous solution of AgNO₃ with silver electrodes.
(ii) An aqueous solution of AgNO₃ with platinum electrodes.
(iii) A dilute solution of H₂SO₄ with platinum electrodes.
(iv) An aqueous solution of CuCl₂ with platinum electrodes.

At cathode: Ag⁺ are preferably discharged as compared to H⁺ as its reduction potential is higher

Ag to the power of plus plus straight e to the power of minus space rightwards arrow space Ag left parenthesis straight s right parenthesis

At anode: Silver electrode (being reactive) dissolves to produce Ag⁺As the electrodes are inert, these do not take part in the reaction. At cathode, Ag⁺ ions are discharged in preference to H⁺ ions and OH^– are discharged in preference to NO₃^– ions at anode
At cathode: Ag+ are preferably discharged as compared to H+ as its

At cathode: Ag+ are preferably discharged as compared to H+ as its

Here, only H⁺ are discharged at cathode as there is no other positive ion. Out of OH^– and SO₄^2– ions, OH^– ions are discharged at anode preferably
At cathode: Ag+ are preferably discharged as compared to H+ as its

The platinum electrodes are inert and do not take part in the reaction. The following reactions occur at platinum (inert) electrodes.
At cathode: Ag+ are preferably discharged as compared to H+ as its

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96.

Depict the galvanic cell in which the reaction
Zn(s) + 2Ag⁺(aq) → Zn²⁺(aq) + 2Ag(s) takes place. Further show:
(i) Which of the electrode is negatively charged?
(ii) The carriers of the current in the cell.
(iii) Individual reaction at each electrode.

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Short Answer Type

97. Following two reactions can occur at cathode in the electrolysis of aqueous sodium chloride:
Na⁺ + e^– → Na(s) 2H₂O(l) + 2r → H₂(g) + 2OH^–(aq)
E°_red = – 0.83 V
Which reaction takes place preferentially and why?

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98. Iron does not rust even if zinc coating is broken in galvanized iron pipe. Explain.

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99. Explain why:
(i) E° for Mn³⁺/ Mn²⁺ couple is more positive than that Fe³⁺/Fe²⁺. (At. No. Mn = 25, Fe = 26).
(ii) Ce³⁺ can be easily oxidised to Ce⁴⁺ (At. No. Ce= 58).

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100. With the halp of ionic equations describe what happen: When
(i) pH of a solution of dichromate ions is raised.
(ii) Potassium manganate is electro-chemically oxidised.

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Previous Year Papers

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Test Yourself

Short Answer Type

Long Answer Type

95. Predict the products of electrolysis in each of the following:(i) An aqueous solution of AgNO3 with silver electrodes.(ii) An aqueous solution of AgNO3 with platinum electrodes.(iii) A dilute solution of H2SO4 with platinum electrodes.(iv) An aqueous solution of CuCl2 with platinum electrodes.

Short Answer Type