For the following reactions: Zn→Zn2++2e−;E=+0.76V Au→Au3++3e−;E=−1.42V If gold foil is placed in a solution containing Zn2+, the reaction potential would be:
−1.34V
−2.18V
−0.66V
+1.34V
+2.18V
A
−2.18V
B
+1.34V
C
−1.34V
D
−0.66V
E
+2.18V
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Solution
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If gold foil is placed in a solution containing Zn2+, Gold will be reduced and Zinc will be oxidised and the following reaction will take place:
3Zn+2Au3+→3Zn2++2Au
The reaction potential for the above reaction is given by :
E=Ecathode−Eanode=−1.42−0.76=−2.18V
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Q1
For the following reactions: Zn→Zn2++2e−;E=+0.76V Au→Au3++3e−;E=−1.42V If gold foil is placed in a solution containing Zn2+, the reaction potential would be:
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Q2
Electrode potentials are: Zn0→Zn2++2e−;E0=+0.76V Au0→Au3++3e−;E0=−1.42V What is the potential of the reaction, if a gold foil is kept in a solution containing zinc ions?
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Q3
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Q4
The standard reduction potentials, E∘, for the half-reactions are as Zn=Zn2++2e, E∘= + 0.76 V and Fe=Fe2++2e, E∘ = + 0.41 V. The e.m.f. for the cell reaction, Fe2++Zn=Zn2++Fe is
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Q5
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