Hydrogen and oxygen gases are produced in the lab through chemical reactions, then combined and ignited to propel a small rocket across the room. The demonstration highlights multiple types of chemical reactions: double replacement, decomposition, combustion, and synthesis.

1. Generate hydrogen gas by reacting zinc with hydrochloric acid.
2. Generate oxygen gas by decomposing hydrogen peroxide with a catalyst such as manganese dioxide or yeast.
3. Collect the gases in small containers or balloons.
4. Mix hydrogen and oxygen in the correct proportions to form a combustible fuel mixture.
5. Ignite the mixture with a flame or spark to launch a small container (such as a teat pipette bulb) forward.
6. Observe the loud “pop” or explosive sound and the motion of the mini rocket.

Making Hydrogen Fueled Mini-Rockets - Beals Science:

📄 Micro Rocket Lab - Flinn Scientific: https://www.flinnsci.com/api/library/Download/73ea6e2a619444b5b3b6eabee20a81e0?srsltid=AfmBOoqZ9uQdqUN-JeLc0yv5UTwPhRRE9e4O4456xuUTtWjvaMjwZeCk

📄 Mini Rockets - U.S. Department of Energy: https://www1.eere.energy.gov/education/pdfs/solar_minirockets.pdf

• Change the ratio of hydrogen to oxygen to see which mixture produces the most powerful launch.
• Try different catalysts for the hydrogen peroxide decomposition (manganese dioxide, potassium iodide, yeast).
• Add fins or a cone to the mini rocket for stability.
• Use electrolysis to produce the hydrogen and oxygen.

• Safety goggles, gloves, and lab apron required.
• Perform only under teacher supervision.
• Keep ignition sources away from gas generators until ready.
• Do not scale up the experiment — only small amounts of gas should be used.
• Ensure the rocket is not aimed at people or breakable objects.

• Which types of chemical reactions are demonstrated in this experiment? (Double replacement, decomposition, combustion, synthesis)
• What is the balanced chemical equation for hydrogen combustion? (2H2 + O2 → 2H2O)
• Why is the correct ratio of hydrogen to oxygen important for the rocket’s power? (Only the stoichiometric ratio ensures all reactants are used, producing the most energy.)
• Why doesn’t the mixture react immediately when the gases are combined? (It requires activation energy from a flame or spark.)
• How is this demonstration similar to real rocket propulsion? (Both rely on rapid combustion of fuel with an oxidizer to release energy and create thrust.)