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Gibbs Energy Of Cell

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Gibbs Energy of Cell

What is Cell potential? 

It is a measure of the flowing source behind an electrochemical reaction, expressed in volts. The potential of an electrochemical cell gauges how far an oxidation-reduction reaction is from equilibrium.

Changes in reaction conditions can tremendously affect the course of a redox reaction. For instance, under standard conditions, the reaction of Co(s) with Ni2+(aq) to frame Ni(s) and Co2+(aq) occurs spontaneously, however on the off chance that we decrease the concentration of Ni2+ by 100, so that [Ni2+] is 0.01 M, at that point the reverse reaction occurs spontaneously instead. The relationship among voltage and concentration is one of the factors that must be understood to anticipate whether a reaction will be spontaneous.

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For the reduction of silver ions with copper metal, the standard cell potential was found to be +0.46V at 25 ^ (@)C the value of the standard Gibb's energy , DeltaG^(@) will be

The standard Gibbs energy for the given cell reaction is KJmol^(-1) at 298 K is : Zn(s)+CU^(2+) (aq) rightarrow Zn^(2+) (aq) + Cu(s) E^(@)= 2V at 298 K (Friday's constant , F = 96000 C mol^-1 )

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(a) The cell in which the following reactions occurs: 2Fe^(3+)(aq)=2I^(-)(aq)to2Fe^(2+)(aq)+I_(2)(s) has E_(cell)^(@)=0.236V at 298 K. Calculate the standard Gibbs energy of the cell reaction. (Given: 1F=96,500" C "mol^(-1) ) (b) How many electrons flow through a metallic wire if a current of 0.5 A is passed for 2 hours? (Given: 1F=96,500" C "mol^(-1) )