A voltaic cell is constructed from a silver wire in a 1.0M aqueous solution AgNO

Question

A voltaic cell is constructed from a silver wire in a 1.0M aqueous solution AgNO3 and a zinc electrode in a 1.0M aqueous solution of Zn(NO3)2. Consider the following standard reduction potentials.

Zn^2+(aq) + 2e^-   ------> Zn (s)           E standard red = -0.762 V

Ag^+ (aq) + e^-     -------> Ag(s)            E standard red = 0.799 V

a. Write the shorthand cell notation for the reaction that takes place.

b. What is the overall cell potential?

c. Which metal strip is the anode?

d. What is the number of moles of electrons transferred?

Explanation / Answer

a)

oxidation // reduction

Zn(s)/(Zn+2(aq), 1M) // (Ag+(aq), 1 M)/Ag(s)

b)

E°cell = Ered - Eox = 0.799 - -0.762 = 1.561 V

c)

anode --> oxidation takes places --> Zn

d)

number of moles being transferred is the minimum multiply = 1*2 = 2 electrons!

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