The standard reduction potentials of Cu2+(aq) | Cu(s) and Ag+(aq) | Ag(s) are .3

Question

The standard reduction potentials of Cu2+(aq) | Cu(s) and Ag+(aq) | Ag(s) are .34 and .8 volts, respectively.
Determine the value of the actual cell potential, Ecell, (in volts) for the following cell at 25C.
Cu(s) | Cu2+(.250 M) || Ag+(.001 M) | Ag(s)
A) .30 V * B) .14 V C) .62 V D) .78 V E) .39 V The standard reduction potentials of Cu2+(aq) | Cu(s) and Ag+(aq) | Ag(s) are .34 and .8 volts, respectively.
Determine the value of the actual cell potential, Ecell, (in volts) for the following cell at 25C.
Cu(s) | Cu2+(.250 M) || Ag+(.001 M) | Ag(s)
A) .30 V * B) .14 V C) .62 V D) .78 V E) .39 V The standard reduction potentials of Cu2+(aq) | Cu(s) and Ag+(aq) | Ag(s) are .34 and .8 volts, respectively.
Determine the value of the actual cell potential, Ecell, (in volts) for the following cell at 25C.
Cu(s) | Cu2+(.250 M) || Ag+(.001 M) | Ag(s)
A) .30 V * B) .14 V C) .62 V D) .78 V E) .39 V

Explanation / Answer

Answer : option A) 0.30 V

anode reaction: oxidation takes place

Cu(s) -------------------------> Cu+2 (aq) + 2e-   ,   E0Cu+2/Cu = 0.34 V

cathode reaction : reduction takes palce

2Ag+(aq) + 2e- -----------------------------> 2Ag(s) , E0Ag+/Ag = 0.8 V

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net reaction: Cu(s) + 2Ag+(aq) -------------------------> Cu+2 (aq) + 2Ag(s)

E0cell= E0cathode- E0anode

E0cell= E0Ag+/Ag - E0Cu+2/Cu

          = 0.8 - (0.34)

          = 0.46 V

nernest equation

Ecell = E0cell -2.303RT/nF* log [Cu+2]/[Ag+]^2

Here R= universal gas constant 8.314 J/K mol

T = absolute temperature =25(0C)= 298k

F= faraday = 96500 Coloumb/mol

n = no of moles of electrons are transfered =2

2.303RT/F= 0.0591

Ecell = E0cell -(0.0591/n)* log [Cu+2]/[Ag+]^2

Ecell = 0.46 - (0.059 x1/2) *log {(0.250)/(0.001)^2}

Ecell   = 0.3 V

cell potential =Ecell   = 0.3 V

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