(iv) Both assertion and reason are false.
Cu2+ + 2e-→ Cu(S) E° = 0.34V
Zn2+ + 2e-→ Zn(S) E° = -0.76V
Cu2+ + Zn(S) → Cu(S) + Zn2+ ; E° = 0.34V – (-0.76V) = + 1.1V
Copper (Cu2+) sulphate can’t be stored in zinc vessel as Zinc is more reactive than Copper. Clearly, one can say that Zinc is a stronger reducing agent than Copper. Thus, Zinc donate electrons to Cu2+ and the above radox reaction occurs.
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