Q1. Define molar conductivity. What is its unit?
Q2. What happens to the cell potential when the concentration of electrolytes in a galvanic cell increases?
Q3. State Kohlrausch’s Law. Write any one application of the law.
Q4. Write the Nernst equation for the following cell:
Zn(s) | Zn²⁺(1M) || Cu²⁺(1M) | Cu(s)
Q5. Differentiate between a galvanic cell and an electrolytic cell (any three points).
Q6. Calculate the standard cell potential of the cell:
Fe(s) | Fe²⁺(1M) || Ag⁺(1M) | Ag(s)
Given:
E°(Ag⁺/Ag) = +0.80 V, E°(Fe²⁺/Fe) = –0.44 V
Q7. Why does the conductivity of a solution decrease with dilution while molar conductivity increases?
Q8.
(a) Derive the relation between Gibbs free energy and EMF of a cell.
(b) Explain the electrolysis of molten NaCl with suitable electrode reactions.
(c) Name the type of cell which is generally used in hearing aids. Mention the electrode reactions for the cell.
Q9.
(a) Define the term fuel cell.
(b) Explain the working of a hydrogen-oxygen fuel cell with a labelled diagram.
(c) Write its two advantages over conventional cells.
Q10.
(a) How is the cell potential affected by temperature and concentration according to the Nernst equation?
(b) The resistance of a conductivity cell containing 0.001 M KCl solution is 1500 ohm. If the cell constant is 1.09 cm⁻¹, calculate its conductivity and molar conductivity.
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