Electrochemistry

The cell, Zn | Zn2+ (1M) || Cu2+ (1M) | Cu(\(E_{cell}^o\) = 1.10V) was allowed to be completely discharged at 298 K. The relative concentration of Zn2+ to Cu2+ $$\left[ {{{\left[ {Z{n^{2 + }}} \right]} \over {\left[ {C{u^{2 + }}} \right]}}...

The equivalent conductances of two strong electrolytes at infinite dilution in H2O (where ions move
freely through a solution) at 25oC are given below:
\(\wedge _{C{H_3}COONa}^o\) = 91.0 S cm2/equiv
\(\wedge _{HCl}^o\) = 426.2 S cm2/equi...

Given the data at 25oC,
Ag + I- \(\to\) AgI + e- , Eo = 0.152 V
Ag \(\to\) Ag+ + e-, Eo = -0.800 V
What is the value of log Ksp for AgI? (2.303 RT/F = 0.059 V)

Resistance of a conductivity cell filled with a solution of an electrolyte of concentration 0.1 M is 100\(\Omega\).
The conductivity of this solution is 1.29 S m–1. Resistance of the same cell when filled with 0.2 M of
the same solution is...

The molar conductivities \(\wedge _{NaOAc}^o\) and \(\wedge _{HCl}^o\) and at infinite dilution in water at 25oC are 91.0 and 426.2 Scm2/mol respectively. To calculate \(\wedge _{HOAc}^o\) , the additional value required is

For a spontaneous reaction the ∆G , equilibrium constant (K) and \(E_{cell}^o\) will be respectively

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Aluminium oxide may be electrolysed at 1000oC to furnish aluminium metal (Atomic
mass = 27 amu; 1 Faraday = 96,500 Coulombs). The cathode reaction is Al3+ + 3e- \(\to\) Alo To prepare 5.12 kg of aluminium metal by this method would require

The highest electrical conductivity of the following aqueous solutions is of :

In a cell that utilises the reaction Zn(s) + 2H+
(aq) \(\to\) Zn2+(aq) + H2(g) addition of H2SO4 to cathode compartment, will

The limiting molar conductivities Λ° for NaCl, KBr and KCl are 126, 152 and 150 S cm2 mol-1 respectively. The Λ° for NaBr is

Consider the following Eo values
\(E_{F{e^{3 + }}/F{e^{2 + }}}^o\) = 0.77 V;
\(E_{S{n^{2 + }}/S{n}}^o\) = -0.14 V
Under standard conditions the potential for the reaction
Sn(s) + 2Fe3+(aq) \(\to\) 2Fe2+(aq) + Sn2+(aq) is :

In a hydrogen – oxygen fuel cell, combustion of hydrogen occurs to :

The standard e.m.f of a cell, involving one electron change is found to be 0.591 V at 25oC.
The equilibrium constant of the reaction is (F = 96,500 C mol-1: R = 8.314 JK-1 mol-1)

The \(E_{{M^{3 + }}/{M^{2 + }}}^o\) values for Cr, Mn, Fe and Co are – 0.41, +1.57, + 0.77 and +1.97 V
respectively. For which one of these metals the change in oxidation state form +2 to +3 is
easiest?

Standard reduction electrode potentials of three metals A,B&C are respectively +0.5 V, -3.0 V & -1.2 V. The
reducing, powers of these metals are

When during electrolysis of a solution of AgNO3, 9650 coulombs of charge pass through the electroplating
bath, the mass of silver deposited on the cathode will be :

For the redox reaction Zn(s) + Cu2+(0.1 M) \(\to\) Zn2+(1M) + Cu(s) taking place in a cell, \(E_{cell}^o\) is 1.10 volt. Ecell for the cell will be (\(2.303{{RT} \over F}\) = 0.0591)

For a cell reaction involving a two-electron change, the standard e.m.f. of the cell is found to be 0.295 V at 25oC. The equilibrium constant of the reaction at 25oC will be

Several blocks of magnesium are fixed to the bottom of a ship to :

For the following cell with hydrogen electrodes at two different pressure p1 and p2. What will be the emf for the given cell :
$$\eqalign{
& Pt({H_2})|{H^ + }(aq)|Pt({H_2}) \cr
& \,\,\,\,\,{p_1}\,\,\,\,\,\,\,\,\,\,\,\,\,\,1M\,\,\,\,\,...

EMF of a cell in terms of reduction potential of its left and right electrodes is :

For a cell given below

$$ \begin{aligned} \mathrm{Ag}^{+}+\mathrm{e}^{-} & \longrightarrow \mathrm{Ag}; E^{\circ}=x \\\\ \mathrm{Cu}^{2+}+2 e^{-} & \longrightarrow \mathrm{Cu}{;} E^{\circ}=y \end{aligned} $$
$$
E^{\circ} \text { cell is }
...

Which of the following reaction is possible at anode?

When the sample of copper with zinc impurity is to be purified by electrolysis, the appropriate
electrodes are :

Conductivity (Seimen’s S) is directly proportional to area of the vessel and the concentration
of the solution in it and is inversely proportional to the length of the vessel then, then constant of proportionality is expressed in :