The change in the cell voltage when the ion concentrations in the anode half-cell are increased by a factor of 10 is decreased by 0.030 V.
The electrochemical cell has both species the Fe²⁺ and Ag⁺ at 1 M concentration . the cell potential is given the standardbred cell potential E°.
at anode if the concentration increased by 10 then:
ΔE = -(R T / nF ) ln Q
now the reactions are :
at anode : Fe ---> Fe²⁺ + 2e
at cathode : 2 ( Ag⁺ + e ---> Ag)
overall : Fe + 2Ag⁺ ----> Fe²⁺ + 2Ag
Q = [Fe²⁺ ] / [Ag⁺]²
now, n = 2 , the change in cell potential is given as:
ΔE = ( -RT / nF ) ln [Fe²⁺ ] / [Ag⁺]²
[Fe²⁺ ] = 10 M
ΔE = -(8.314 × 298 ) / 2 × 96485 ln [10] / [1]
ΔE = - 0.030 V
Thus, the cell potential at anode half cell will decreased by 0.030 V.
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