Consider a galvanic cell composed of a Cu/Cu2+ (1 M) half-cell and a Zn/Zn2+ (1

Question

Consider a galvanic cell composed of a Cu/Cu2+ (1 M) half-cell and a Zn/Zn2+ (1 M) half cell.

A. Which electrode has a stronger pull on electrons?

B. Write the Cathode reaction.

C. Write the Anode reaction.

D. Do the electrons flow from the cathode to the anode or from the anode to cathode?

E. Use the standard potentials to confirm that cell voltage is 1.10V.

Explanation / Answer

standard reduction potenital values are : Cu2+ + 2e- ----> Cu ....Eo = 0.34 V Zn2+ + 2e- -----> Zn ...Eo = -0.76 V as standard reduction potential of Cu2+/Cu is more than Zn2+/Zn so reduction will occur at Cu2+/Cu electrode and oxidation will occur at Zn2+/Zn electrode. A.as reduction is occuring at Cu2+/Cu electrode so it has stronger pull of electrons as in reduction electrons are consumed .. Cu2+ + 2e- ---> Cu this reaction takes place B.reduction takes place at cathode and oxidation takes place at anode cathode : Cu2+ + 2e- ----> Cu C.anode : Zn ----> Zn2+ + 2e- D.as anode is giving electrons so electrons are going from anode to cathode E.Ecell = Eocathode - Eoanode = 0.34 - -0.76 =0.34 + 0.76 = 1.1 V

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