Which of the following changes would tend to decrease the measured cell potentia

Question

Which of the following changes would tend to decrease the measured cell potential of a voltaic cell with cell reaction cu (aq) + 2 Ag^+(s) rightarrow Cu^2+(aq) + 2 Ag(s) X. decrease the [Ag^+] in the cathode compartment Y. increase the size the solid copper electrode Z. decrease the [Cu^2+] in the anode compartment A. Y and Z B. Z only C. X and Z D. X only Calculate E_cell at 298 K for the voltaic cell Cr(s)|Cr^2+(aq, 0.015M)||Fe^3+(aq, 0.800M)|Fe(s) For this cell, E degree = 0.87 V at 298 K and the cell reaction is 3 Cr(s) + 2 Fe^3+ (aq) doubleheadarrow 3 Cr^2+(aq) + 2 Fe(s). A. 1.03 V B. 0.97 V C. 0.92 V D. 082 V Given Au^3+ + 3e^- rightarrow Au(s) E degree = 1.40 V Cu^2+ + 2e^- rightarrow Cu(s) E degree = 0.34 V calculate Delta G degree for the reaction 3 Cu(s) + 2 Au^3+(aq) rightarrow 3 Cu^2+(aq) + 2 Au(s). A. -205 kJ B. -614 kJ C. 205 kJ D. -307 kJ

Explanation / Answer

Q36

decrease the E value is given by:

E = E°-0.0592/n * log(Q)

since E° and n are constant, only Q changes

If Q products increase, then the E decreases

therefore, increase of Cu2+

or a decrease in reactants, such as Ag+,

choose X only

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