The time required to liberate one gram equivalent of an element by passing one ampere current through its solution is

Which has the highest oxidizing power ?

For the reduction of silver ions with copper metal, the standard cell potential was found to be + 0.46 V at 25°C. The value of standard Gibbs energy, \({ \Delta G }^{ ° }\) will be (F = 96500 C mol^-1)

Using the data given below find out the strongest reducing agent.
\({ E }_{ { Cr }_{ 2 }{ O }_{ 7 }^{ 2- }/{ Cr }^{ 3+ } }^{ \circleddash }=1.33V\ ,\ { E }_{ { Cl }_{ 2 }/{ Cl }^{ - } }^{ \circleddash }=1.36V\)
\({ E }_{ { MnO }_{ 4 }^{ - }/{ Mn }^{ 2+ } }^{ \circleddash }=1.51V\ ,\ { E }_{ { Cr }^{ 3+ }/{ Cr } }^{ \circleddash }=-0.74V\)

One faraday of electricity is passed thorugh molten Al₂ O₃ , aqueous solution of CuSO₄ and molten NaCl taken in three different electrolytic cells connected in series. The mole ratio of Al, Cu and Na deposited at the respective cathode is

Ezpress the relation among cell constant, resistance of the solution in the cell and conductivity of the solution. How is molar conductivity of solution related to its conductivity.

The molar conductivity of 1.5 M solution of an electrolyte is found to be 138.9 S cm² mol^-1 . Calculete the conductivity of this solution.

Fluorine has a low electron gain enthalpy compared to chlorine, yet it is a more powerful oxidant. Explain why?

When a certain electrolytic cell was filled with 0.1 M KCl, it has resistance of 85 ohms at 25 ^oC. When the same cell was filled with an aqueous solution of 0.052 M unknown electrolyte, the resistance was 96 ohms. Calculate the molar conductance of the electrolyte at this concentration. [Specific conductance of 0.1 M KCl = \(1.29\times { 10 }^{ -2 }{ ohm }^{ -1 }{ cm }^{ -1 }\)]

(i) Arrange the following metals in the order in which they displace each other from the solution of their salts.
Al, Cu, Fe, Mg and Zn.
(ii) Given the standard electrode potentials;
K⁺/K = -2.93V,Ag⁺/Ag = 0.80V, Hg²⁺/Hg = +0.79V.
Mg²⁺/Mg = -2.37V, Cr³⁺/Cr = -0.74V.
Arrange these metals in their increasing order of reducing power.

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.

Three electrolytic cells A, B, C containing solutions of ZnSO₄, AgNO_3, and CuSO₄, respectively are connected in series. A steady current of 1.5 amperes was passed through them until 1.45 g of silver deposited at the cathode of cell B. How long did the current flow? What mass of copper and zinc were deposited?

Using the standard electrode potentials, predict if the reaction between the following is feasible:
(i) Fe³⁺(aq) and I^-(aq)
(ii) Ag⁺(aq) and Cu(s)
(iii) Fe³⁺(aq) and Br^-(aq) 
(iv) Ag(s) and Fe³⁺(aq)
(v) Br₂(aq) and Fe²⁺(aq)

The standard electrode potentials of different electrodes are given as
E⁰ Co³⁺ /Co 2+ = 1.81 V, E⁰ Al 3+ /Al = -1.66 V, E⁰ Fe ²⁺ /Fe = -0.44 V, E⁰ _Br2/Br- = 1.01 V
a. Identify all the possible combination for construction of a feasible electrochemical cell?
b. Write their electrochemical cell representation.
c. Calculate the emf in each case.

EMF of Daniell cell was found using different concentrations of Zn²⁺ ion and Cu² ion. A graph was then plotted between E_cell and \(\log { \frac { \left[ { Zn }^{ 2+ } \right] }{ \left[ { Cu }^{ 2+ } \right] } } \) . The plot was found to be linear with intercept on E_cell axis equal to 1.10 V. Calculate E_cell for Zn | Zn²⁺ (0.1 M) || Cu²⁺ (0.01 M) | Cu.