Physical chemistryLesson 2 of 2 in the course Electrochemistry

Primary and Rechargeable Batteries and Hydrogen Fuel Cells

5 flashcards · 5 quiz questions · 5 match pairs · 5 fill-in sentences · English

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Summary

Batteries are galvanic cells designed to provide electrical power for particular uses. This lesson introduces primary batteries, which are generally intended for single use, and compares two familiar examples: zinc-carbon dry cells and alkaline cells.

A battery is a galvanic cell, or a group of cells, constructed to suit a particular application. In a galvanic cell, a spontaneous redox reaction transfers electrons through an external circuit, producing electrical current. The anode is where oxidation occurs, while reduction occurs at the cathode.

All flashcards

Anode and cathode in a galvanic cell
Oxidation occurs at the anode; reduction occurs at the cathode.
Cells connected in series
A battery arrangement in which the individual cell voltages add together.
Nickel-cadmium (NiCd) battery
A rechargeable battery with a cadmium anode, nickel-containing cathode, and potassium hydroxide electrolyte.
Lithium-ion battery during charging
An external power source drives reactions that reverse the cell's discharge reactions.
Fuel cell
A galvanic cell that generates electricity from continuously supplied fuel and oxidant.

Quiz questions

  1. What makes a secondary cell rechargeable?Answer: An external power source can reverse its discharge reaction.
  2. How does a typical 12 V automobile lead-acid battery obtain its voltage?Answer: Six cells of about 2 V are connected in series.
  3. Why do NiCd batteries require careful handling and disposal?Answer: They contain toxic cadmium, a heavy metal.
  4. What allows a fuel cell to keep generating electricity?Answer: Fuel and oxidant are supplied continuously, while products are removed.
  5. How do typical hydrogen fuel-cell efficiencies compare with internal-combustion-engine efficiencies for the same redox reaction?Answer: Fuel cells are about 50%–75% efficient; engines are about 20%–25% efficient.

Based on Chemistry 2e by Paul Flowers, Klaus Theopold, Richard Langley, William R. Robinson, PhD (OpenStax), licensed CC BY 4.0. Adapted into a summary, flashcards and quizzes.

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