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113. A friend wants you to invest in a new battery she has designed that produces 24 V in a single voltaic cell. Why should you be wary of investing in such a battery?

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Related questions

In some applications nickelā€“cadmium batteries have been replaced by nickelā€“zinc batteries. The overall cell reaction for this relatively new battery is

H2O (l) + 2 NiO(OH) (s) + Zn(s) ā†’2 Ni(OH)2(s) + Zn(OH)2(s)

a)What is the cathode half-reaction? (b) What is the anode half-reaction? (c) A single nickelā€“cadmium cell has a voltage of 1.30 V. Based on the difference in the standard reduction potentials of Cd2+ and Zn2+, what voltage would you estimate a nickelā€“zinc battery will produce? (d) Would you expect the specific energy density of a nickelā€“zinc battery to be higher or lower than that of a nickelā€“cadmium battery?

Heart pacemakers are often powered by lithiumā€“silver chromate ā€œbuttonā€ batteries.

The overall cell reaction is

2 Li(s) + Ag2CrO4(s)ā†’ 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? (b) Choose the two half-reactions from Appendix E 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? (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 Ā°C. How does this compare to the emf you calculated in part (b)?

One Class Solution:-a) Li(s) is oxidized at the anode.

Ag2CrO4(s)+ 2e-ā†’ 2Ag(s) + CrO42-(aq), E= 0.446V

Li(s) ā†’ Li+(aq)+e- E=ā€“3.05V

2 Li(s) + Ag2CrO4(s)ā†’ Li2CrO4(s) + 2Ag(s)

b) E0=0.446V-(-3.05V) =3.496=3.50V

c) The emf of the battery, 3.5 V, is exactly the standard cell potential calculated in part (b).

d) For this battery at ambient conditions, E0= E0, so logQ=O. This makes sense because all reactants and products in the battery are solids and thus present in their standard states. Assuming that E0 is relatively constant with temperature, the value of the second termin the Nernst equation is= 0 at 37Ā°C, and E=3.5V.

How do you do the math for this? I know cost of Zinc is $5.30/100 g, Silver is $0.56/g, and Lead is $2.45/100g..

The construction of a cell with maximum voltage

Use metal strips and solutions of your choice to determine which combination will give the largest potential. Several different metals and metal salt solutions will be available. In general, the solid metal should be the same metal as that in the salt solution it is in contact with. Utilize a table of standard reduction potentials to help decide which cells to construct. Keep in mind that you can connect more than one cell together. You can also vary the concentration of the metal salt solutions. A minimum of 3 different batteries should be made and tested. Your grade will not be based solely on the number of batteries you make, but also on the strategy used for choosing battery designs and the thoroughness of your investigation. In addition to finding the highest voltage you can achieve, determine which battery gives you the best ratio of volts to cost (V/$).

Battery 1.) HALF CELL ONE: 1.0 Mg2+ (aq) and 1.0 Mg (s) HALF CELL TWO: 1.0 M Zn2+ (aq) and Zn (s) observed potential = + 1.12 V

Battery 2.) HALF CELL ONE: 1.0 Mg2+ (aq) and 1.0 Mg (s) HALF CELL TWO: 1.0 M Ag+ (aq) and Ag (s) observed potential = + 2.39 V

Battery 3.) HALF CELL ONE: 1.0 Mg2+ (aq) and 1.0 Mg (s) HALF CELL TWO: 1.0 M Pb2+ (aq) and Pb (s) observed potential = + 1.42 V

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