Final answer:
The decomposition reaction of hydrogen peroxide in the presence of a catalyst is 2H₂O₂ (l) → 2H₂O(g) + O₂(g). A catalyst like manganese dioxide increases the reaction rate. The stoichiometric mole ratio helps determine the volume of oxygen produced.
Step-by-step explanation:
The decomposition reaction of hydrogen peroxide (H₂O₂) in the presence of a catalyst can be represented by the following chemical equation:
2H₂O₂ (l) → 2H₂O(g) + O₂(g)
This reaction shows that two moles of liquid hydrogen peroxide decompose to form two moles of water vapor and one mole of oxygen gas. The reaction is often catalyzed by substances such as manganese dioxide (MnO₂) or other catalysts to increase the reaction rate without being consumed in the process. In the context of a controlled thrust system in space vehicles, the rapid decomposition of hydrogen peroxide can generate sufficient quantities of oxygen gas and steam to produce thrust.
The stoichiometric mole ratio is important to calculate the amount of product formed from a given amount of reactant. For every 2 moles of H₂O₂ that decompose, 1 mole of O₂ is produced. Using this ratio alongside the ideal gas law equation, one can calculate the volume of oxygen gas at a given temperature and pressure.