(a)
Interpretation:
The given lithium-iodide cell reaction the oxidation half-reaction and reduction half-reaction have to be explained.
Concept introduction:
A galvanic cell is an
Oxidation half-reaction: The oxidation half-reaction is the part of a redox reaction that shows only for the oxidized species with the transferred electrons and its oxidation state increases with the loss of electrons.
Reduction half-reaction: The reduction half-reaction is also the part of a redox reaction (the counter part of oxidation half-reaction) that shows only for the reduced species with the transferred electrons and its oxidation state decreases with the gain of electrons.
(a)
Explanation of Solution
Oxidation half-reaction:
The lithium
This reaction is oxidation half reaction, because the reactant lithium metal
Reduction half-reaction:
This reaction is a reduction half reaction, because the two electrons are on the reactants side
(b)
Interpretation:
The lithium iodide overall cell reaction has to be written.
Concept introduction:
Overall reaction: It is combining of two molecules in together.
Example: Hydrogen and oxygen to form water, the cell provides a drinking water supply for the astronauts as well as the electricity for the lights, computer, etc., on the board.
Oxidation: If electrons are moved from a species during a
Reduction: If electrons are gained to a species during a chemical reaction. The species which gets electrons are said to be reduced.
(b)
Explanation of Solution
The galvanic cell produces energy through the transfer of electrons from one substance to another. In order to represent the electron transfer process, the overall chemical reaction can be divided into two parts as two half reaction.
One of the half reaction, named as oxidation reaction in which chemical species loses electrons.
Consider the given reaction:
Above reaction is a oxidation half reaction, the lithium
Further the iodine undergoes for reduction half reaction, the two electrons are on the reactants side
Further combine the two half-reaction to obtain the overall balanced equation becomes a lithium iodide
(c)
Interpretation:
The following cell reaction that occurs at the anode and at the cathode has to be identified.
Concept introduction:
A redox reaction is a chemical reaction where both oxidation and reduction occur simultaneously. In a redox reaction, one of the reactants is oxidized, while the other reactant is reduced at the same time. It can be represented as two half-reactions with the number of transferred electrons. They are as follows:
- • Oxidation half-reaction.
- • Reduction half-reaction.
Oxidation half-reaction: The oxidation half-reaction is the part of a redox reaction that shows only for the oxidized species with the transferred electrons and its oxidation state increases with the loss of electrons.
Reduction half-reaction: The reduction half-reaction is also the part of a redox reaction (the counter part of oxidation half-reaction) that shows only for the reduced species with the transferred electrons and its oxidation state decreases with the gain of electrons.
(c)
Explanation of Solution
Oxidation half-reaction:
The lithium
This reaction is oxidation half reaction, because the reactant lithium metal
Reduction half-reaction:
This reaction is a reduction half reaction, because the two electrons are on the reactants side
Want to see more full solutions like this?
Chapter 7 Solutions
Chemistry In Context
- A factory wants to produce 1.00 103 kg barium from the electrolysis of molten barium chloride. What current must be applied for 4.00 h to accomplish this?arrow_forwardA silver oxidezinc cell maintains a fairly constant voltage during discharge (1.60 V). The button form of this cell is used in watches, hearing aids, and other electronic devices. The half-reactions are Zn(s)+2OH(aq)Zn(OH)2(s)+2eAg2O(s)+H2O(l)+2e2Ag(s)+2OH(aq) Identify the anode and the cathode reactions. What is the overall reaction in the voltaic cell?arrow_forwardA voltaic cell can be built using the reaction between Al metal and O2 from the air. If the Al anode of this cell consists of 84 g of aluminum, how many hours can the cell produce 1.0 A of electricity, assuming an unlimited supply of O2?arrow_forward
- Consider a galvanic cell based on the following half-reactions: a. What is the expected cell potential with all components in their standard states? b. What is the oxidizing agent in the overall cell reaction? c. What substances make up the anode compartment? d. In the standard cell, in which direction do the electrons flow? e. How many electrons are transferred per unit of cell reaction? f. If this cell is set up at 25C with [Fe2+] = 2.00 104 M and [La3+] = 3.00 103 M, what is the expected cell potential?arrow_forwardFor the cell: Cr|Cr3+Co2+|Co E° is 0.46 V. The same cell was prepared in the laboratory at standard conditions. The voltage obtained was 0.40 V. A possible explanation for the difference is (a) the surface area of the chromium electrode was smaller than the cobalt electrode. (b) the mass of the chromium electrode was larger than the mass of the cobalt electrode. (c) the concentration of Cr(NO3)2 solution used was less than 1.0 M. (d) the concentration of Cr(NO3)2 solution used was less than 1.0 M. (e) the volume of Cr(NO3)2 solution used was larger than the volume of Cr(NO3)2 solution used.arrow_forward
- Living By Chemistry: First Edition TextbookChemistryISBN:9781559539418Author:Angelica StacyPublisher:MAC HIGHERIntroductory Chemistry: A FoundationChemistryISBN:9781337399425Author:Steven S. Zumdahl, Donald J. DeCostePublisher:Cengage LearningChemistry: An Atoms First ApproachChemistryISBN:9781305079243Author:Steven S. Zumdahl, Susan A. ZumdahlPublisher:Cengage Learning
- ChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage LearningChemistry: Matter and ChangeChemistryISBN:9780078746376Author:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl WistromPublisher:Glencoe/McGraw-Hill School Pub Co