At the turn of the 20th century, electric automobiles were more popular than gasoline-fueled cars. Thomas Edison, the prolific American inventor, was interested in electric automobiles and developed an iron-nickel (Fe-Ni) battery to power them. He claimed that, due to their higher energy density, his batteries were superior to the lead-acid batteries then being used in automobiles. Today, the Edison battery is available in various voltages up to 48 V. It is used in London subway locomotives, in New York City subway cars, for standalone locations that are off the electric power grid, and for backup emergency power. The battery has a NiO(OH) cathode, an iron anode, and uses a mixture of KOH and LiOH as the electrolyte. The half-reactions are:
Cathode: ???(??)(?) → ??(??)2(?)
Anode: ??(?) → ??(??)2(?)
The E_cell^o is 1.37 V at 25 °C, which drops to 1.2 V when operating.
(a)Assign an oxidation number to nickel in the reactant and product of the cathode reaction
(b)Identify what is oxidized and what is reduced
(c)Write a balanced chemical equation for the overall cell reaction
(d)Calculate the cell voltage at 25 °C when the hydroxide ion concentration is 3.5 M
Upvote if you find the answer is helpful. Thank you and have a great day. Stay safe
At the turn of the 20th century, electric automobiles were more popular than gasoline-fueled cars. Thomas...
Edison also developed a nickel-zinc battery for use in electric automobiles. The battery is now used in some cellphones and digital cameras. This battery operates in much the same way as the iron-nickel battery; both use NiO(OH) as the cathode. The E_cell^o for the nickel-zinc cell is 1.65 V at 25 °C. (a)Calculate the ∆G° (kJ/mol) for each of the battery reactions. (b)Which battery—the iron-nickel or nickel-zinc—has the more product-favored reaction at standard conditions? Explain your answer. (c)Does the nickel-zinc...