EASY
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How many kJ of energy is evolved, when a current of 2.00 A passes for 200 s under the potential of 230 V?

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Important Questions on Electrochemistry

EASY
The standard free energy change (in J) for the reaction 3Fe2+aq+2Crs2Cr3+aq+3Fes given EFe2+/Fe0=-0.44 V and ECr3+/Cr0=-0.74 V is (F = 96500 C)
EASY
The equilibrium constant of a 2 electron redox reaction at 298 K is 3.8×10-3. The cell potential Eoin V and the free energy change ΔGo in kJ mol- for this equilibrium respectively, are
EASY
The standard electrode potential of Zn2+/Zn is-0.76 V and that of Cu2+/Cu is 0.34 V. The emf V and the free energy change, in kJ mol-1, respectively, for a Daniel cell will be
EASY
The standard emf of a galvanic cell involving 2 moles of electrons in its redox reaction is 0.59 V. The equilibrium constant for the redox reaction of the cell is:
HARD

The standard electrode potential Eo and its temperature coefficient dEdT for a cell are 2V and -5×10-4 V K-1 at 300 K, respectively. The reaction is Zn s+Cu2+ aqZn2+ aq+Cu s. The standard reaction enthalpy ΔrH- at 300K in mol-1 is 

[Use R=8 J K-1 mol-1 and F=96,500 Cmol-1]

MEDIUM
For a cell involving one electron Ecell=0.59 V at 298 K, the equilibrium constant for the cell reaction is:
Given that 2.303 RTF=0.059 V at T=298 K 
EASY
What is the standard reduction potential Eo for Fe3+Fe?

Given that:

Fe2++2e-Fe;EFe2+/Feo=-0.47V

Fe3++e-Fe2+;EFe3+/Fe2+o=+0.77V
MEDIUM

The emf of the following cell is 1.229 V at 298 K.

Pt,H21atmH+1MO21atm,Pt 

H2+12O2H2O

The standard free energy change for the cell reaction is________ F=9.649×104 C mol-1

MEDIUM
If the standard electrode potential for a cell is 2 V at 300 K, the equilibrium constant K for the reaction.

Zns+Cu2+aqZn2+aq+Cus 

at 300 K is approximately:

R=8 JK-1mol-1, F=96000 C mol-1
EASY
If the Ecello for a given reaction has a negative value, which of the following gives the correct relationship for the values of Go and Keq?
MEDIUM
Given EMn+7|Mn+2=1.5 V and EMn+4|Mn+2=1.2 V, then EMn+7/Mn+4 is
HARD

Calculate G° for the reaction Zn s + Cu2+ aq Zn2+ aq + Cu s

Given:

E° for Zn2+/Zn = -0.76VE° for Cu2+/Cu = +0.34VR = 8.314 JK-1 mol-1F = 96500 C mol-1

MEDIUM
For a reaction, A+B2+B+A2+, at 250C E0=0.2955V. The value of Keq is
MEDIUM

For the cell reaction

2Fe3+aq+2I-aq2Fe2+aq+I2aq

Ecell0=0.24V at 298 K. The standard Gibbs energy ΔrGo of the cell reaction is:

[Given that Faraday constant F=96500 Cmol-1 ]

MEDIUM

The standard e.m.f. of the cell, CdsCdCl2aq0.1M|AgCls|Ags in which the cell reaction is Cds+2AgCls2Ags+Cd2+aq+2Cl-aq is 0.6915 V at 0°C and 0.6753 V at 25°C. The enthalpy change of the reaction at 25°C is

MEDIUM
The standard free energy change for the cell reaction
Zn(s)+Cu(aq)2+Zn(aq)2++Cu(s) is EZn2+/Zn°=-0.76V,ECu2+/Cu°=+0.34V,1 F=96500Cmol-1
EASY
Given the standard potentials EoCu2+Cu and EoCu+Cu as 0.340V and 0.522V respectively, the value of EoCu2+Cu+ is
MEDIUM
The emf of a particular voltaic cell with the cell reaction, Hg22++H22Hg+2H+, is 0.65 V. What is the maximum electrical work of this cell when 0.5 g of H2 is consumed?
HARD
The cell in which the following reaction occurs: 
2Fe3+aq+2I-aq2Fe2+aq+I2(s) has Ecell0=0.236 V at 298 K. Calculate the standard Gibbs energy and the equilibrium constant of the cell reaction.