Question

Manganese dioxide acts as a catalyst in the decomposition of H2O2 into water and oxygen gas. Which statement best describes this function?

a. The potential energy of the bonds in manganese dioxide is less than the potential energy of the bonds in water and oxygen gas, so the activation energy is lower in the presence of manganese dioxide.

b. Manganese dioxide adds heat to the system so that the molecules of H2O2 collide with more force and are more likely to result in broken atomic bonds.

c. Manganese dioxide lowers the potential energy of the bonds in H2O2 so that less activation energy is required for H2O2 to decompose.

d. The activation energy required for manganese dioxide to form intermediate molecules with H2O2 is less than the activation energy required for H2O2 to decompose on its own.

Answer 1

The function of manganese dioxide as a catalyst in the decomposition of H2O2 is to lower the potential energy of the bonds in H2O2, requiring less activation energy for decomposition.

Step-by-step explanation:

The statement that best describes the function of manganese dioxide as a catalyst in the decomposition of H2O2 is:

Manganese dioxide lowers the potential energy of the bonds in H2O2 so that less activation energy is required for H2O2 to decompose.

As a catalyst, manganese dioxide provides an alternate reaction pathway with a lower activation energy barrier. This allows the decomposition reaction of hydrogen peroxide to occur at a faster rate than it would without the catalyst. Manganese dioxide is not consumed in the reaction and can be used repeatedly.