Cell Potential and Free Energy of a Lithium-Chlorine Cell In thermodynamics, we

Question

Cell Potential and Free Energy of a Lithium-Chlorine Cell In thermodynamics, we determine the spontaneity of a reaction by the sign of Delta G In electrochemistry, spontaneity is determined by the sign of Edegreecell. The values of Delta G and Edegreecell are related by the following formula: where n is the number of moles of electrons and T = 96,500J/V midddot mol e is the Faraday constant. The standard reduction potentials of lithium metal and chlorine gas are as follows: In a galvanic cell, the two half-reactions combine to Calculate the cell potential of this reaction under standard reaction conditions. Express your answer with the appropriate units. Calculate the free energy Delta G degree of the reaction. Express your answer with the appropriate units.

Explanation / Answer

(A) 2 Li(s) + Cl2(g) => 2 LiCl(aq)

Eo = Eo(Cl2/Cl-) - Eo(Li+/Li)

= 1.36 - (-3.04)

= 4.40 V

(B) Moles of electrons transferred n = 2

Delta Go = -nFEo

= - 2 x 96500 x 4.40

= -849200 J/mol = -849.2 kJ/mol (approximately -849 kJ/mol)

(C) Since Eo is positive and Delta Go is negative

=> the reaction is spontaneous as written

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