A) i) Write the anode, cathode and total battery reactions, balance the reaction and calculate the standard battery potential (E°) at 25°C. ii) Calculate the cell potential at the given concentrations using the Nernst equation. iii) Find the ΔG°298 and equilibrium constant values of the reaction
A) i) Write the anode, cathode and total battery reactions, balance the reaction and calculate the standard battery potential (E°) at 25°C. ii) Calculate the cell potential at the given concentrations using the Nernst equation. iii) Find the ΔG°298 and equilibrium constant values of the reaction
Principles of Modern Chemistry
8th Edition
ISBN:9781305079113
Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Chapter17: Electrochemistry
Section: Chapter Questions
Problem 59P
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A) i) Write the anode, cathode and total battery reactions, balance the reaction and calculate the standard battery potential (E°) at 25°C.
ii) Calculate the cell potential at the given concentrations using the Nernst equation.
iii) Find the ΔG°298 and equilibrium constant values of the reaction. Interpret whether the reaction is spontaneous (E°Mg2+/Mg = -2.363 V, E°Ag+/Ag = 0.80 V).
Mg(s) | Mg2+(0.001M) || Ag^+(0.01 M) | Ag(s)
B) If the water is electrolyzed by passing a current of 0.5 amperes for 2 hours, how much is left from the cell?
electron passes and how many cm3 of H2 is produced at 273 K?
(MH = 1 g/mol, MO = 16 g/mol, F = 96500 C)
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