Q9 of 26 Page 1

In a galvanic cell, the following cell reaction occurs:

Zn(s) + 2Ag+(aq) → Zn2+(aq) + 2Ag(s), E°cell = +1.56 V


(a) Is the direction of flow of electrons from zinc to silver or silver to zinc?


(b) How will concentration of Zn2+ ions and Ag+ ions be affected when the cell functions?


At cathode, 2Ag+ (aq) + 2e- → 2Ag(s)


At anode, Zn(s) → Zn2+(aq) + 2e-


(a) The electrons move from anode to cathode. Electrons are released at anode which is zinc after oxidation and then are accepted at cathode which is silver for reduction. So, the direction of flow of electrons is from zinc to silver.


(b) As the cell functions, more and more Zn will be converted to Zn2+ at anode through oxidation and more and more Ag+ will be converted to Ag at cathode through reduction. Therefore, the concentration of Zn2+ ions will increase and that of Ag+ ions will decrease.


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