CHEM 1412 Project
Group 4
Hydrogen peroxide is an oxidizer commonly used a disinfectant, antiseptic, oxidizer, and in
rocketry as a propellant. It is highly reactive, flammable and corrosive which means that it
should be harmful to any living (especially human) tissue. It might be a surprise then that the
human body actually produces hydrogen peroxide which however decomposes to water and
oxygen gas, and the activation energy for this process is 42 kJ/mol.
1. If the temperature required for this process is 1600°C, what observations would you
make considering the fact that the reaction occurs in biological processes?
2. The hydrogen peroxide formed in biological processes is harmful to tissue, but the
enzyme catalase catalyzes the decomposition hydrogen peroxide by lowering the
activation energy. Assuming the frequency factor is the same for both processes and
independent of temperature; calculate activation energy required for the uncatalyzed
decomposition to proceed at the same rate as the enzyme-catalyzed decomposition at
98.6°F (normal human body temperature).
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Answer Key
1. 1600°C; not reasonable for biological systems
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