A lithium ion battery, such as found in a cell phone, operates at a high cell po

Question

A lithium ion battery, such as found in a cell phone, operates at a high cell potential based on the following half-cell reactions: CoO_2 + Li^+ + e^- doubleheaded arrow LiCoO_2 E degree approximatelyequalto 1 V Li^+ + C_6 (polymer graphite) + e^- doubleheaded arrow LiC_6 (polymer/graphite) E degree approximatelyequalto 3 V Compare to: O_2(g) + 4H^+ + 4e^- doubleheaded arrow 2H_2O E degree = 1.23 V 2H^+ + 2e^- doubleheaded arrow H_2(g) E degree = 0.00 V Li^+ + e^- doubleheaded arrow Li E degree approximatelyequalto -3 V What is the overall cell reaction for the lithium ion battery shown? What is the overall standard cell potential of the reaction you wrote in (a)? what is the n (number of electrons) for the overall cell reaction you wrote in (a)? Which elements of which compounds are being oxidized and which are being reduced in the overall cell reaction you wrote in (a)? Determine the oxidation states of all the species in the reaction. Can the reaction that you wrote in (a) be carried out in water (aqueous solution)? Why or why not?

Explanation / Answer

For the given data

a) Overall cell reaction for lithium ion battery

CoO2 + LiC6 --> LiCoO2 + C6

b) Overall standard potential = 1 - (-3) = 4 V

c) number of electrons = 1

d) Co of CoO2 is getting reduced. C6 of LiC6 is getting oxidized

oxidation state

Co in CoO2 = +4

O in CoO2 = -2

Li in LiC6 = +1

C6 in LiC6 = -1

Co in LiCoO2 = +3

O in LiCoO2 = -2

Li in LiCoO2 = +1

C6 in C6 = 0

e) the reaction may not be carried out in water as the potential value falls below the working range

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