객관식
Why does increasing the surface area cause a reaction to proceed more quickly?
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15. Chemical Kinetics
Factors Influencing Rates
객관식
Which of the following would most effectively increase the rate of decomposition of hydrogen peroxide (H2O2)?
A
Diluting the hydrogen peroxide solution with water
B
Adding manganese dioxide (MnO2) as a catalyst
C
Removing light from the reaction environment
D
Lowering the temperature of the reaction mixture
검증된 단계별 안내1
Understand that the rate of decomposition of hydrogen peroxide (H\_2O\_2) can be influenced by factors such as concentration, temperature, presence of catalysts, and environmental conditions like light exposure.
Recall that catalysts increase the rate of a chemical reaction by providing an alternative reaction pathway with a lower activation energy, without being consumed in the process.
Analyze each option: Diluting the solution decreases concentration, which generally slows down the reaction rate according to the rate law; removing light may reduce photochemical effects but is not the primary factor here; lowering temperature decreases kinetic energy, thus slowing the reaction.
Recognize that adding manganese dioxide (MnO\_2) acts as a catalyst for the decomposition of hydrogen peroxide, significantly increasing the reaction rate by lowering the activation energy.
Conclude that among the given options, adding MnO\_2 as a catalyst most effectively increases the rate of hydrogen peroxide decomposition.
