Question

draw the result for the n Ernest eqn. .......




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help your fr jimmy

Answer 1

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The Nernst equation is derived from the standard changes in the Gibbs free energy associated with an electrochemical transformation. For any electrochemical reduction reaction of the form

Ox + z e− → Red

standard thermodynamics says that the actual free energy change ΔG is related to the free energy change under standard state ΔGo by the relationship

{\displaystyle \Delta G=\Delta G^{\ominus }+RT\ln Q,}

where Q is the reaction quotient. The electrochemical potential E associated with the electrochemical reaction is defined as the decrease in Gibbs free energy per coulomb of charge transferred, which leads to the relationship

{\displaystyle \Delta G=-zFE.}

The constant F (the Faraday constant) is a unit conversion factor F = NAq, where NA is Avogadro's number and q is the fundamental electron charge. This immediately leads to the Nernst equation.

The Nernst equation for an electrochemical half-cell is

{\displaystyle E_{\text{red}}=E_{\text{red}}^{\ominus }-{\frac {RT}{zF}}\ln Q=E_{\text{red}}^{\ominus }-{\frac {RT}{zF}}\ln {\frac {a_{\text{Red}}}{a_{\text{Ox}}}}.}

For a complete electrochemical reaction (full cell), the equation can also be written as

{\displaystyle E_{\text{cell}}=E_{\text{cell}}^{\ominus }-{\frac {RT}{zF}}\ln Q_{r},}    (total cell potential)

where

Ered is the half-cell reduction potential at the temperature of interest,Eo

red is the standard half-cell reduction potential,Ecell is the cell potential (electromotive force) at the temperature of interest,Eo

cell is the standard cell potential,R is the universal gas constant: R = 8.314472(15) J K−1 mol−1,T is the temperature in kelvins,