In the electrochemical cell shown above, which of the following half-reactions occurs at the anode?
Cu2++e→Cu−
Zn(s)→Zn2++2e
Zn2++2e→Zn(s)
Cu(s)→Cu2++2e
Cu2++2e→Cu(s)
A
Zn2++2e→Zn(s)
B
Cu2++e→Cu−
C
Zn(s)→Zn2++2e
D
Cu2++2e→Cu(s)
E
Cu(s)→Cu2++2e
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Solution
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At anode, oxidation will take place and Zn(s) will get oxidised to Zn2+ leaving negatively charged electrons, making anode negatively charged, repelling negatively charged NO−3.
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