Turning Chemistry Into Electricity

Part of Fuel Cells · Section 1 of 13

IntroductionUnit: Energy ChangesGCSE
Every time you drop a zinc rod and a copper rod into lemon juice, you have built a battery. The lemon's acid acts as the electrolyte, and electrons flow through a wire from the more reactive zinc to the less reactive copper — creating a measurable voltage. Scale this up, swap the metals, and you have the chemistry behind every battery you've ever owned. Replace the metals with hydrogen and oxygen, and you have the fuel cell technology being fitted to buses and trains right now.

This introduction covers Turning Chemistry Into Electricity within Fuel Cells for GCSE Chemistry. Revise Fuel Cells in Energy Changes for GCSE Chemistry with 5 exam-style questions and 6 flashcards. This topic appears regularly enough that it should still be part of a steady revision cycle. It is section 1 of 13 in this topic. Use this introduction to connect the idea to the wider topic before moving on to questions and flashcards.

Practice questions for Fuel Cells

A simple electrochemical cell is made by placing two different metal electrodes into an electrolyte. Which statement correctly describes what affects the voltage produced?

  • A. The larger the size of the electrodes, the greater the voltage
  • B. The greater the difference in reactivity between the two metals, the greater the voltage
  • C. Two identical metal electrodes always produce a small voltage
  • D. Using a more concentrated electrolyte always increases the voltage
1 markfoundation

Compare a non-rechargeable alkaline battery with a rechargeable lithium-ion battery. Give one advantage and one disadvantage of the rechargeable battery.

3 marksstandard

Quick recall flashcards

What is a fuel cell?
An electrochemical cell that generates electricity continuously from an external fuel supply (hydrogen) and an oxidant (oxygen). Unlike a battery, it does not run down — it operates as long as fuel is supplied. Only product: water.
Write the overall equation for the hydrogen–oxygen fuel cell.
2H₂ + O₂ → 2H₂O Only product: water. No carbon dioxide or air pollutants produced at point of use.

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Inside a Hydrogen Fuel Cell

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