During an experiment, one student heated a crucible containing 1gKCLO3. A neighb

Question

During an experiment, one student heated a crucible containing 1gKCLO3. A neighboring student heated a crucible containing a mixture of 1g of KCLO3 and 00.2g MnO2. A glowing splint at the mouth of the crucible was used to signal the appearance of oxygen. Oxygen gas causes the flowing splint to burst into flame. Which student's glowing splint will burst into flame first? Why? c.) Which crucible will produce oxygen gas at a lower temperature, the one with or without the MnO_2? Explain. d.) Explain how and why a catalyst affects the activation energy of a reaction.

Explanation / Answer

b) Neighboring student's glowing splint burst into flame first, because catalyst MnO2 enhances the rate of reaction. In both case same reactions take place. Catalyst makes reaction go faster forward ------------> that means it makes producing O2 faster

2 KClO3 2 K Cl + 3 O2

MnO2 is a catalyst; since it is not consumed it is not listed as a reactant.

c)

The crucible with MnO2 produces oxygen at lower temperature, because catalyst MnO2 reduced the activation energy.

d) A catalyst provides an alternative pathway for a reaction Usually, this will be more complicated than the original, uncatalyzed reaction. Reaction KCLO3 is heated proceeds in a single step without the catalyst, but takes many steps when catalyzed. However, the activation energy is lowered because each of the steps has a lower-energy transition state than the original reaction.

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