Given that, Ni2+/Ni=0.25V,Cu2+/Cu=0.34V Ag+/Ag=0.80V and Zn2+/Zn=−0.76V Which of the following reactions under standard condition will not take place in the specified direction?
A
Ni2+(aq.)+Cu(s)→Ni(s)+Cu2+(aq.)
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B
Cu(s)+2Ag+(aq.)→Cu2+(aq.)+2Ag(s)
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C
Cu(s)+2H+(aq.)→Cu2+(aq.)+H2(g)
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D
Zn(s)+2H+(aq.)→Zn2+(aq.)+3H2(g)
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Solution
The correct options are ANi2+(aq.)+Cu(s)→Ni(s)+Cu2+(aq.) DCu(s)+2H+(aq.)→Cu2+(aq.)+H2(g)
→ Reduction potential of Ni2+ is less than Cu(s). Hence, reduction of Ni2+ will not take place and it will not form Ni(s) in given reaction. So, reaction A not possible.
→ Copper is not reactive enough to displace hydrogen ions from solution. Hence, reaction C is not possible in specified direction.