Cell Potential and Gibbs Energy of a Lithium Chlorine Cell Part A The standard r

Question

Cell Potential and Gibbs Energy of a Lithium Chlorine Cell Part A The standard reduction potentials of lithium metal and chlorine gas are as follows In thermodynamics, we determine the spontaneity of a reaction by the sign of .G In electrochemistry spontaneity is determined by the sign of Fel The values of ,C and Ecell are related by the following formula Reduction potential Reaction 3.04 Li+ (aq) + e-Li(s) Cl2 (g) + 2e-2C1-(aq) +1.36 where n is the number of moles of electrons and In a galvanic cell, the two half-reactions combine to F = 96 485 J V-1 mol-1 is the Faraday's constant. 2Li (s) + C12 (g)--2LiCl (ag) Calculate the cell potential of this reaction under standard reaction conditions Express your answer with the appropriate units Ecell = 1 Value Units Submit Hints My Answers Give Up Review Part Part B Calculate the standard Gibbs energy change r G° of the reaction Express your answer with the appropriate units 0 Submit Hints My Answers Give Up Review Part

Explanation / Answer

1] Eo = Reduction half reaction + Oxidation half reaction

Eo = 3.04+1.36 = 4.4 V

2] Delta G = -nFEo

n = no of moles of electrons transferred =2 from the given reaction.

so,

Delta G = -2*96485*4.4 = - 849.068KJ

Part C

The reaction spontaneous as written .

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