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Chemistry
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11 Dec 2019

At standard conditions, the electrochemical cell below has Eocellcello = 1.24 V. What is the standard Gibbs free energy for this electrochemical cell at 298K?

Fe (s) | Fe2+ (aq) || Ag+ (aq) | Ag (s)

A.


120 kJ

B.

-239 kJ

C.

-120 kJ

D.

239 kJ

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Trinidad Tremblay
Trinidad TremblayLv2
13 Dec 2019

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Related questions


Calculate the standard change in Gibbs free energy, ?G°rxn, for the following reaction at 25.0 °C. Standard Gibbs free energy of formation values can be found here.

For the following electrochemical cell: Cu(s)/Cu2+(aq, 0.0155 M)//Ag+(aq, 2.50 M)/Ag(s)

write the net cell equation. Phases are optional. Do not include the concentrations. Calculate the following values at 25.0 degrees C using standard potentials as needed: Eknot cell (V), Delta Gknot reaction (kJ/mol), E cell (V), Delta G reaction (kJ/mol).

Ok so this is a question on my sapling homework and I entered:

Cu + 2Ag+ -> Cu2+ +2Ag (correct)

Eknot cell = Eknot red + Eknot ox: (0.80) + (-0.34) = 0.46 V (correct)

*Delta Gknot rxn = nFEknotcell: -2(96,485)(0.46) = -88766.2 J = -8877 kJ/mol (incorrect)

Delta G rxn = Delta Gknot rxn + RTln(Q): -88.77 + (8.3145 x 10-3)(298)[ln(0.155/(2.50)2)] = -103.69 kJ/mol (correct)

*E cell = (-Delta G rxn)/(nF): (-103.690)/[(2)(96485)] = 0.54 V or 0.5 V (incorrect)

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