CHMA11H3 Lecture Notes - Lecture 30: Gibbs Free Energy, Membrane Potential, Redox
CHMA11H3 Lecture Notes - Lecture 29: Standard Electrode Potential, Standard Hydrogen Electrode, Electrochemical Cell
CHMA11H3 Lecture Notes - Lecture 30: Gibbs Free Energy, Membrane Potential, Redox
CHMA11H3 Lecture Notes - Lecture 31: Standard Hydrogen Electrode, Ph Meter, Intensive And Extensive Properties
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In thermodynamics, we determine the spontaneity of a reaction by the sign of ÎG. In electrochemistry, spontaneity is determined by the sign of Eâcell. The values of ÎG and Eâcell are related by the following formula: ÎGâ=ânFEâcell where n is the number of moles of electrons transferred and F=96,500J/Vâ mol eâ is the Faraday constant.
Part A The standard reduction potentials of lithium metal and chlorine gas are as follows: Reaction, Reduction potential (V) Li+(aq)+eââLi(s) â3.04
Cl2(g)+2eââ2Clâ(aq) +1.36
In a galvanic cell, the two half-reactions combine to 2Li(s)+Cl2(g)â2Li+(aq)+2Clâ(aq) Calculate the cell potential of this reaction under standard reaction conditions. Express your answer with the appropriate units.
Part B: Calculate the free energy ÎGâ of the reaction. Express your answer with the appropriate units.
Part C:
What can be said about the spontaneity of this reaction?
The reaction is:
a. spontaneous as written. | |
b. spontaneous in the reverse direction. | |
c. at equilibrium. | |
d. nonspontaneous in either direction. |