Answered: Heart pacemakers are often powered by…

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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3. Heart pacemakers are often powered by lithium–silver chromate “button” batteries. The overall cell reaction is: 2 Li(s) + Ag2CrO4(s) → Li2CrO4(s) + 2Ag(s)

a) Lithium metal is the reactant at one of the electrodes of the battery. Is it the anode or the cathode? Explain.

b) Choose the two half-reactions that most closely approximate the reactions that occur in the battery. What standard emf would be generated by a voltaic cell based on these half-reactions? Refer your answer on the electrode reduction potential table.

c) The battery generates an emf of +3.5 V. How close is this value to the one calculated in part (b)?

d) Calculate the emf that would be generated at body temperature, 37°C. How does this compare to the emf you calculated in part (b)?

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Quiz 5: Batteries and Corrosion
1. In the following:
a) What happens to the emf of a battery as it is used? Why does this
happen?
b) The AA-size and D-size alkaline batteries are both 1.5-V batteries that
are based on the same electrode reactions. What is the major difference
between the two batteries? What performance feature is most affected
by this difference?
2. During a period of discharge of a lead-acid battery, 402 g of Pb from the
anode is converted into PbSO4(s).
a) What mass of PbO2(s) is reduced at the cathode during this same
period?
b) How many coulombs of electrical charge are transferred from Pb to
PbO2?
3. Heart pacemakers are often powered by lithium-silver chromate
"button" batteries. The overall cell reaction is: 2 Li(s) + AgCrO4(s) →
LizCrO4(s) + 2Ag(s)
a) Lithium metal is the reactant at one of the electrodes of the battery. Is
it the anode or the cathode? Explain.
b) Choose the two half-reactions that most closely approximate the
reactions that occur in the battery. What standard emf would be
generated by a voltaic cell based on these half-reactions? Refer your
answer on the electrode reduction potential table.
c) The battery generates an emf of +3.5 V. How close is this value to the
one calculated in part (b)?
d) Calculate the emf that would be generated at body temperature, 37°C.
How does this compare to the emf you calculated in part (b)?
4. The hydrogen-oxygen fuel cell has a standard emf of 1.23 V. What
advantages and disadvantages there to using this device as a source of
power compared to a 1.55-V alkaline battery?
5. In the following:
a) What is the difference between a battery and a fuel cell?
b) Can the "fuel" of a fuel cell be a solid? Explain.
6. In the following:
a) Write the anode and cathode reactions that cause the corrosion of iron
metal to aqueous iron(II).
b) Write the balanced half-reactions involved in the air oxidation of
Fe2*(ag) to Fe2O3 -3H2O.
7. In the following:
a) Magnesium metal is used as a sacrificial anode to protect underground
pipes from corrosion. Why is the magnesium referred to as a "sacrificial
anode"?
b) What meta
the underground pipes
be mac
rom in ord
for
magnesium to be successful as a sacrificial anode?
8. A plumber's handbook states that you should not connect a brass pipe
directly to a galvanized steel pipe because electro- chemical reactions
between the two metals will cause corrosion. The handbook recommends
you use instead an insulating fitting to connect them. Brass is a mixture of
copper and zinc. What spontaneous redox reaction(s) might cause the
corrosion? Justify your answer with standard emf calculations.

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