An aqueous solution of copper sulphate, CuSO₄ was electrolysed between platinum electrodes using a current of  0.1287 ampere for 50 minutes. (Atomic mass of Cu=63.5 g mol^-1].
(a) Write the cathodic reaction.
(b) Calculate:
(i) Electric charge passed during electrolysis.
(ii) Mass of copper deposited at the cathode
[Given : 1F = 96,500 C mol^-1]

For the cell
\(Zn(s)\left| { Zn }^{ 2+ }(2M) \right| \left| { Cu }^{ 2+ }(0.5M) \right| Cu(s)\)
(a) Write equation for each half-reaction.
(b) Calculate the cell potential at 25 ^oC.
[Given: \({ E }_{ { Zn }^{ 2+ }/Zn }^{ o }=-0.76V;{ E }_{ { Cu }^{ 2+ }/Cu }^{ o }=+0.34V\)]

The E^o values at 298 K corresponding to the following two reduction electrode processes are:
(i) Cu⁺/Cu = +0.52 V
(ii) Cu²⁺/Cu⁺ = +0.16 V
Formulate the galvanic cell for their combination. What will be the cell potential? Calculate the \({ \triangle }_{ r }{ G }^{ o }\) for the cell reaction.(1F = 96500 C mol^-1).

Calculate the standard cell potentials of galvanic cell in which the following reactions take place:
(i) \(2Cr(s)+{ 3Cd }^{ 2+ }(aq)\rightarrow { 2Cr }^{ 3+ }(aq)+3Cd(s)\)
(ii) \({ Fe }^{ 2+ }(aq)+{ Ag }^{ + }(aq)\rightarrow { Fe }^{ 3+ }(aq)+Ag(s)\)
Calculate the \({ \triangle }_{ r }{ G }^{ o }\) and equilibrium constant for the reactions.

A solution of CuSO₄ is electrolysed for 10 minutes with a current of 1-5 amperes. What is the mass of copper deposited at the cathode? (Molar mass of Cu = 63.5 g mol^-1)

Two electrolytic cells containing silver nitrate solution and copper sulphate solution are connected in series. A steady current of 2-5 ampere was passed through them till 1.078 g of Ag were deposited. How long did the current flow? What weight of copper will be depopsited?(at mass of Ag = 107.8, Cu = 63.5)

Which of the following has larger molar conductance:
a. 0.08 M soln. having conductivity equal to 2 × 10^-2 ohm^-1cm^-1
b. 0.10 M soln. having resistivity equal to 5.8 ohm cm

Electrolysis of the solution of MnSO4 in aq sulphuric acid is a method for the preparation of MnO₂ as per the chemical reaction
Mn²⁺ + 2H₂O → MnO₂ + 2H⁺ + H₂
Passing a current of 27 A for 24 Hrs gives 1 kg of MnO₂. What is the current efficiency ? What are the reactions occurring at anode and cathode?

Calculate the emf of the following cell at 25° C:
\(Fe|{ Fe }^{ 2+ }(0.01M)\parallel { H }^{ + }\left( 0.01M \right) { H }_{ 2 }(g)(1bar)|Pt(s)\)
\({ E }^{ ° }\left( { Fe }^{ 2+ }|Fe \right) =-0.44V{ E }^{ ° }\left( { H }^{ + }|{ H }_{ 2 } \right) =0.00V\)

A 100W and 110 V incandescent lamp is connected in series with an electrolytic cell containing CdSO₄  solution. What mass of cadmium will be deposited at the cathode after 4 hrs of electricity?