Given that ΔG = 83.1 Kj or 83100 J
ΔG = -n*F*E
83100 = -2*96500*E
E = - 0.431 V
If the standard cell potential is positive, then the reaction is spontaneous, while if the standard cell potential is negative, then the reaction is non-spontaneous
Here the value of standard cell potential is -0.431 means the given reaction is non-spontaneous.
Given that AGo = 83.1 Kj or 83100 J AGo = -n*F*EO 83100 = -2*96500*EO Eo=-0.431 V n=Number of electron use: The Nernst equation: Ecell = Ecell(standard) - 0.0591/n * log Q Q= [Product] /[reactants] E = E0 -0.059/n * log ([Cd2+]/[Zn2+]) = -0.431 -0.059/2 * log (1.17/4.80*10^-3) = -0.431 -0.059/2 * log (4.10*10^-3) =-0.431 -0.059/2 *(+2.39) = -0.431 -0.0704 =-0.501 V If the standard cell potential is positive, then the reaction is spontaneous, while if the standard cell potential is negative, then the reaction is non- spontaneous Here the value of standard cell potential is -0.501 vmeans the given reaction is non- spontaneous.
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