(i) (a) Study the diagram given below that represents Cu-Ag electrochemical cell and answer the questions that follow.





(1) Write the cell reaction for the above cell.
(2) Calculate the standard emf of the cell.
(3) Ifthe concentration of [Cu²⁺] is 0.1 M and E_cell is 0.422 V, at 25°C, calculate the concentration of [Ag⁺].
(4) Calculate ▵G for the cell.

(b) Calculate ^^°_m, for BaCl₂ and Al₂(SO₄)₃ from the following data.



OR

(ii) (a) A 0.05 M NH₄OH solution offers the resistance of 30.8 ohms to a conductivity cell at 298K. If the cell constant is 0.343 cm^-1 and molar conductance of NH₄OH at infinite dilution is 471.4 S cm²mol^-1, calculate the following:

(1) Specific conductance
(2) Molar conductance
(3) Degree of dissociation

(b) Inthe diagram of the electrolytic cell given below, A, B and C are connected in series having electrolytes of ZnSO₄, AgNO₃ and CuSO₄respectively. A steady current of 1.5 A was passed until 1.45 g of Ag was deposited at the cathode of cell B.



(Atomic mass of Ag = 108, Cu = 63.5, Zn = 65.3)

Answer the following questions.

(1) How long did the current flow?
(2) What weight of Cu and Zn was deposited at cathode?

Solution

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