Calculate the emf of the following cell at 25°C.
Ag(s)/Ag+ (10^-3)// Cu^2+ (10^-1m)/Cu(s)
Given E°cell =+0.46V,and log 10^n=n.
The answer is 0.314
Need explanation
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Calculate the emf of the following cell at 25°C.
Ag(s)/Ag+ (10^-3)// Cu^2+ (10^-1m)/Cu(s)
Given E°cell =+0.46V,and log 10^n=n.
The answer is 0.314
Need explanation
Best answer brainlist
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Answer:
Explanation:
Here silver (Ag) undergoes oxidation by loss of electrons, thus act as anode. Copper (Cu) undergoes reduction by gain of electrons and thus act as cathode.
Using Nernest equation :
where,
n = number of electrons in oxidation-reduction reaction = 2
= standard electrode potential = 0.46 V
Now put all the given values in the above equation, we get
Therefore, the EMF of the cell at is, 0.61 V
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