(a)
Interpretation:
Equations for the cell reactions that occur in the voltaic cells (1) and (2) should be written.
Concept introduction:
In amalgam electrode, metal-amalgam is in contact with a solution containing its own ions. The activities of highly reactive metals like first row elements are difficult to measure in aqueous solutions. So their activity is reduced by diluting with mercury.
(b)
Interpretation:
The value of ΔrG for the cell reactions written in part (a) should be determined.
Concept introduction:
From the electrode potential of the cell, the value of ΔrG can be calculated as follows:
Here, z is number of electrons transferred in a reaction, F is Faraday’s constant and
(c)
Interpretation:
The overall equation obtained by combining the equation of part (a) should be written. And ΔrG0 for the overall reaction should be established.
Concept introduction:
For a combination of reaction.
Where, n is the number of species and
(d)
Interpretation:
The value of E0celland E0Na+/Nafor the overall reaction should be determined.
Concept introduction:
From the electrode potential of the cell, the value of ΔrG can be calculated as follows:
Here, z is number of electrons transferred in a reaction, F is Faraday’s constant and
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General Chemistry: Principles and Modern Applications (11th Edition)
- An aqueous solution of an unknown salt of vanadium is electrolyzed by a current of 2.50 amps for 1.90 hours. The electroplating is carried out with an efficiency of 95.0%, resulting in a deposit of 2.850 g of vanadium. a How many faradays are required to deposit the vanadium? b What is the charge on the vanadium ions (based on your calculations)?arrow_forwardA galvanic cell is based on the following half-reactions: In this cell, the copper compartment contains a copper electrode and [Cu2+] = 1.00 M, and the vanadium compartment contains a vanadium electrode and V2+ at an unknown concentration. The compartment containing the vanadium (1.00 L of solution) was titrated with 0.0800 M H2EDTA2, resulting in the reaction H2EDTA2(aq)+V2+(aq)VEDTA2(aq)+2H+(aq)K=? The potential of the cell was monitored to determine the stoichiometric point for the process, which occurred at a volume of 500.0 mL H2EDTA2 solution added. At the stoichiometric point, was observed to be 1 .98 V. The solution was buffered at a pH of 10.00. a. Calculate before the titration was carried out. b. Calculate the value of the equilibrium constant, K, for the titration reaction. c. Calculate at the halfway point in the titration.arrow_forwardAn aqueous solution of an unknown salt of gold is electrolyzed by a current of 2.75 amps for 3.39 hours. The electroplating is carried out with an efficiency of 93.0%, resulting in a deposit of 21.221 g of gold. a How many faradays are required to deposit the gold? b What is the charge on the gold ions (based on your calculations)?arrow_forward
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