Suppose the galvanic cell sketched below is powered by the following reaction: 3

Question

Suppose the galvanic cell sketched below is powered by the following reaction: 3Zn(s) + 3Fe(NO_3)_3(aq) 3Zn(NO_3)_2(aq) + 2Fe(s) 3Zn(s) + 2Fe(NO_3)_3(aq) rightarrow 3Zn(NO_3)_2(aq) + 2Fe(s) Write a balanced equation for the half-reaction that happens at the cathode of this cell. Write a balanced equation for the half-reaction that happens at the anode of this cell. Of what substance is E_1 made? Of what substance is E_2 made? What are the chemical species in solution S_1? What are the chemical species in solution S_2?

Explanation / Answer

The reaction that is occurring is

3Zn + 2Fe(NO3)3 -----> 3Zn(NO3)2 + 2Fe

From the reaction Zn is oxidised to Zn+2 and Fe+2 is reduced to Fe

1) The anode is zinc as it is oxidised

2) the cathode is Fe as it si reduced

3) the oxidation half reaction at anode is 3Zn ---------> 3Zn+2 +6e-or

3Zn -------> 3Zn(NO3)2 +6e-

4) reduction half reaction at cathode is

2Fe+2 +6e- --------> 2Fe or

2Fe(NO3)3 +6e- ----------> 2Fe

5) E1 is Zn

6) E2 is Fe

7) S1 is Zn(NO3)2

8) S2 is Fe(NO3)3

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