Problem: 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)

FREE Expert Solution

Part A


If a balanced reaction equation is not given you can determine the anode and cathode by comparing their E° values.

oxidation anode

reduction cathode


Half-reactions:

Cu2+ (aq) + 2 e- → Cu (s)        E° = 0.34 V         oxidation anode

Ag(aq) + e- → Ag (s)             E° = 0.80 V         reduction cathode


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Problem Details

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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