Lesson Plan

• Describe the overall chemical reaction of a hydrogen‑oxygen fuel cell.
• Explain the function of each cell component (anode, cathode, electrolyte, external circuit).
• Illustrate the flow of electrons and protons that generates electrical energy.
• Compare the environmental advantages of hydrogen‑oxygen fuel cells with conventional combustion.
• Predict that water is the only chemical product of the reaction.

• Projector and screen
• PowerPoint/Google Slides with fuel‑cell diagram
• Printed handout of cell components and half‑reactions
• Simple fuel‑cell model or demonstration kit (if available)
• Worksheet for guided practice
• Whiteboard and markers

Begin with a quick video clip of a hydrogen‑oxygen fuel cell powering a small device to spark curiosity. Ask students what they already know about electrochemical cells and how they differ from batteries. Explain that by the end of the lesson they will be able to state the overall reaction and identify why water is the only by‑product.

1. Do‑Now (5'): Students write, in one sentence, what they think a fuel cell does.
2. Mini‑lecture with slides (10'): Present the overall reaction and each component’s role.
3. Guided analysis (10'): Examine the table of components/functions; students label a blank diagram.
4. Half‑reaction walk‑through (8'): Show oxidation and reduction equations; students match them to anode/cathode.
5. Demonstration or video (7'): Observe electron flow and proton migration; discuss energy conversion.
6. Group activity (10'): Complete worksheet comparing fuel‑cell advantages to combustion.
7. Check for understanding (5'): Quick quiz (exit ticket) – write the net reaction and the sole product.

Recap the key points: the net reaction, component functions, and why water is the only by‑product. Collect exit tickets to gauge mastery and assign a short homework task to research one real‑world application of hydrogen‑oxygen fuel cells.