Problem: Sketch a voltaic cell for each redox reaction. Label the anode and cathode and indicate the half-reaction that occurs at each electrode and the species present in each solution. Also indicate the direction of electron flow.c. 2 NO3– (aq) + 8 H+(aq) + 3 Cu(s) → 2 NO(g) + 4 H 2O (/) + 3 Cu2+(aq) 

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We’re being asked to sketch a voltaic cell for the following reaction:

2 NO3–(aq) + 8 H+(aq) + 3 Cu(s)  2 NO(g) + 4 H2O(l) + 3 Cu2+(aq)


Recall that a voltaic or galvanic cell is an electrochemical cell that is spontaneous and produces electricity


From the reaction, we can see that the oxidation state of Cu went from 0 (Cu) to +2 (Cu2+) which means it was oxidized or lost electrons


The anode (–) half-reaction is:

Cu(s)  Cu2+(aq) + 2 e

0 = +2 + x

x = –2 = 2 e to the product side


The other half-reaction is then reduced or gained electrons


The cathode (+) half-reaction is:

2 NO3–(aq) + 8 H+(aq) + 6 e  2 NO(g) + 4 H2O(l)

2(–1) + 8(+1) + x = 0

x = –6 = 6 e to the reactant side


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Problem Details

Sketch a voltaic cell for each redox reaction. Label the anode and cathode and indicate the half-reaction that occurs at each electrode and the species present in each solution. Also indicate the direction of electron flow.
c. 2 NO3 (aq) + 8 H+(aq) + 3 Cu(s) → 2 NO(g) + 4 H 2O (/) + 3 Cu2+(aq)

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Our data indicates that this problem or a close variation was asked in Chemistry: A Molecular Approach - Tro 3rd Edition. You can also practice Chemistry: A Molecular Approach - Tro 3rd Edition practice problems.