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Lithium-ion battery. (a) Ideal formulas for the electrodes of the Li-ion battery

Quantitative Chemical Analysis | 8th Edition | ISBN: 9781429218153 | Authors: Daniel C. Harris ISBN: 9781429218153 475

Solution for problem 13-11 Chapter 13

Quantitative Chemical Analysis | 8th Edition

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Quantitative Chemical Analysis | 8th Edition | ISBN: 9781429218153 | Authors: Daniel C. Harris

Quantitative Chemical Analysis | 8th Edition

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Problem 13-11

Lithium-ion battery. (a) Ideal formulas for the electrodes of the Li-ion battery described in the chapter opener are C6Li (FM 79.01) and LiCoO2 (FM 97.87). When the battery operates, C6Li is consumed and LiCoO2 is formed. Write a half-reaction for each electrode, assuming that x 1 in the reaction . (In fact, in real cells.) Which is the anode and which is the cathode? (b) Charge capacity of an electrode in a battery is expressed as mAh/g, which is the number of milliamperes delivered by 1 g of material for 1 hour. How many coulombs are in 1 mAh? (c) Show that the theoretical capacity of the battery is 274 mAh/g LiCoO2. (d) A Li-ion battery can deliver 140 mAh/g LiCoO2. What fraction of Li in the formula LiCoO2 is available? (e) Energy stored by a battery per unit mass of an electrode material is expressed as Wh/g. A Li-ion battery delivers 140 mAh/g LiCoO2 at 3.7 V. Express the energy storage as Wh/g LiCoO2. St

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Entropy Changes & Spontaneity methane from gas leak in LA reacts with O2 in atmosphere and combusts to form • water and CO2 —CH4(g) + 2O2(g)—>CO2(g) + 2H2O(l) —3 gas molecules—> 1 gas molecule + 2 liquid molecules results in decrease in entropy • ∆Ssys=∆Hsys/T • ∆Ssurr=∆Hsurr/T • ∆Suniv=∆Ssys + ∆Ssurr = ∆Ssys - (∆Hsys/T) • ex. Calculate ∆Ssys, ∆Ssurr, and ∆Suniv when 1 mole of water in ice at 0˚C melts to 22˚C. ∆H=6.01 kJ —∆Ssys=6010 J/273 K=22.0 J/K —∆Ssurr=-6010 J/295 K=-20.4 J/K —∆Suniv=22.0 J/K - 20.4 J/K=1.6 J/K • if ∆Suniv>0, the reaction is spontaneous —only ∆Suniv can determine spontaneity, not ∆Ssys (determines # microstates) • ∆Srxn=(#moles x ∆S) products - (#moles x ∆S) reactants • Gibbs free energy formula

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Chapter 13, Problem 13-11 is Solved
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Textbook: Quantitative Chemical Analysis
Edition: 8
Author: Daniel C. Harris
ISBN: 9781429218153

Since the solution to 13-11 from 13 chapter was answered, more than 238 students have viewed the full step-by-step answer. The answer to “Lithium-ion battery. (a) Ideal formulas for the electrodes of the Li-ion battery described in the chapter opener are C6Li (FM 79.01) and LiCoO2 (FM 97.87). When the battery operates, C6Li is consumed and LiCoO2 is formed. Write a half-reaction for each electrode, assuming that x 1 in the reaction . (In fact, in real cells.) Which is the anode and which is the cathode? (b) Charge capacity of an electrode in a battery is expressed as mAh/g, which is the number of milliamperes delivered by 1 g of material for 1 hour. How many coulombs are in 1 mAh? (c) Show that the theoretical capacity of the battery is 274 mAh/g LiCoO2. (d) A Li-ion battery can deliver 140 mAh/g LiCoO2. What fraction of Li in the formula LiCoO2 is available? (e) Energy stored by a battery per unit mass of an electrode material is expressed as Wh/g. A Li-ion battery delivers 140 mAh/g LiCoO2 at 3.7 V. Express the energy storage as Wh/g LiCoO2. St” is broken down into a number of easy to follow steps, and 166 words. This full solution covers the following key subjects: . This expansive textbook survival guide covers 55 chapters, and 1224 solutions. This textbook survival guide was created for the textbook: Quantitative Chemical Analysis, edition: 8. The full step-by-step solution to problem: 13-11 from chapter: 13 was answered by , our top Chemistry solution expert on 03/16/18, 04:33PM. Quantitative Chemical Analysis was written by and is associated to the ISBN: 9781429218153.

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Lithium-ion battery. (a) Ideal formulas for the electrodes of the Li-ion battery