191. A current of 1.50 amp passed through an electrolytic cell containing AgNO₃ solution with inert electrodes. The weight of Ag deposited was 1.50 g. How long did the current flow?

192. Write the reactions taking place at the anode and cathode in the above cell.
When AgNO₃ is electrolysis in aqueous solution?

193. Give reactions taking place at the two electrodes if these are made up of Ag.

194. The following chemical reaction is occuring in an electro-chemical cell
Mg(s) + 2Ag⁺(0.001 M) → Mg²⁺(0.10 M) + Ag(s)
The E° electrode values are
Mg²/Mg = – 2.36 V
Ag⁺/Ag = 0.81
V For the cell calculate/write:
(a) (i) E° value for the electrode 2Ag⁺/2Ag
(ii) Standard cell potential E°_Cell
(b) Cell potential (E)_cell
(c) (i) Symbolic representation of the above cell
     (ii) Will the above cell reaction be spontaneous?

195. Calculate the equilibrium constant for the reaction:
Cd²⁺(aq) + Zn(s) → Zn²⁺(aq) + Cd(s)
if E°_Cd²⁺/Cd = – 0.403 V.
E°_zn²⁺/zn = – 0.763 V

196. When a current of 0.75 A is passed through a CuSO₄ solution for 25 min, .36 g of copper is deposited at the cathode. Calculate the atomic mass of copper.

197. Tarnished silver contains Ag₂S. Can this tarnish removed by placing silver in an aluminium pan containing an inert electrolytic solution such as NaCl. The standard electrode potential for half reaction.

198. Calculate the standard free energy change for the following reaction at 25°C.
Au(s) + Ca²⁺(aq.1M) → Au³⁺(aq. 1M) + Ca(s)
E°_Au²⁺/Au = – 0.403 V.
E°_Au²⁺/Cu = – 0.763 V.
Predict whether the reaction will be spontaneous or not at 25°C. Which of the above two half cells will act as an oxidizing agent and which one will be a reducing agent?

199. The conductivity of 0.001 M acetic acid is 4 x 10^–5 s/cm. Calculate the dissociation constant of acetic acid, if λ°_m for acetic acid is 390.5 s cm² mol. 

200. A solution of sodium in liquid ammonia at -33°C conducts electricity. On cooling, the conductivity of this solution is_________.