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Main_ISM_ch11

# Main_ISM_ch11 - Chapter 11 Electrochemical Cells Batteries...

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11-1 Chapter 11: Electrochemical Cells, Batteries, and Fuel Cells Problem numbers in italics indicate that the solution is included in the Student’s Solutions Manual . Questions on Concepts Q11.1) What is the difference in the chemical potential and the electrochemical potential for an ion and for a neutral species in solution? Under what conditions is the electrochemical potential equal to the chemical potential for an ion? . z μ μ φ = + % For a neutral species, the chemical potential and electrochemical potential have the same value. They differ by z φ for an ion. The electrochemical potential is equal to the chemical potential for an ion if φ = 0. Q11.2) Show that if ( ) H , 0 for all , f G aq T + Δ = o the potential of the standard hydrogen electrode is zero. ( ) 2 2 / 1 2 and H , 0 H H H f H H H G aq F F μ μ μ φ μ + + + + + = = − = Δ = o o o o o o Q11.3) To determine standard cell potentials, measurements are carried out in very dilute solutions rather than at unit activity. Why is this the case? In order to determine the standard potential, the mean ionic activity must be known. It can be calculated in dilute solutions using the Debye-Huckel limiting law, but there is no reliable way to calculate the activity coefficient near unit activity. Q11.4) Explain why it is possible that the magnitude of the maximum work available from a battery can be greater than the magnitude of the reaction enthalpy of the overall cell reaction. 1 if 0 electrical T S w G H H S H Δ = −Δ = −Δ > −Δ Δ < Δ Q11.5) The temperature dependence of the potential of a cell is vanishingly small. What does this tell you about the thermodynamics of the cell reaction? Because , 0 R R R P P G E S nF S T T ∂Δ Δ = − = Δ o o o o

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