Consider the following reduction potentials: Cu^2+ +2e^- rightarrow Cu E degree

Question

Consider the following reduction potentials: Cu^2+ +2e^- rightarrow Cu E degree = +0.335 V Pb^2+ + 2e^- rightarrow Pb E degree =-0.130 V For a galvanic cell employing the Cu, Cu^2+ and Pb, Pb^2+ couples, calculate the amount of work that would accompany the reaction of 1 mol of lead under conditions. -39.6 kJ -44.9 kJ -89.7 kJ No work can be done. The system is at equilibrium. none of these A reaction is spontaneous when Delta G degree is negative and E degree is positive. Delta G degree is negative and E degree is negative. Delta G degree is positive and E degree is negative. Delta G degree is positive and E degree is positive. Delta G degree is negative, Delta H degree is negative, and E degree is negative. A piece of iron half-immersed in a sodium chloride solution will corrode more than a piece of iron half-immersed in pure water, because the sodium ions oxidize the iron atoms. the chloride ions oxidize the iron atoms. the chloride ions form a precipitate with iron. the chloride ions increase the pH of the solution. the sodium ions and chloride ions carry a current through the solution. Given: Cr^3+ (aq) + 3e^- Cr(s); E degree = -0.74 v Fe^2+ (aq) + 2e^- Fe(s); E degree = -0.41 V What is the standard Gibbs free-energy change for the following reaction? 2 Cr(s) + 3 Fe^2+ (aq) rightarrow 3 Fe(s) + 2Cr^3+ (aq) -504 kJ -191 kJ 191 kJ 63.7 kJ 1060 kJ

Explanation / Answer

8.

E°cell =Ered - Eox

E°cell = 0.335 + 0.130 = 0.465 V

then

G = -nF*E°cell

G = -2*96500*0.465

G = -77200 J/mol

G = -77.2 kJ/mol

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