Catalyst affect on hydrogen peroxide

Essay by maddy99High School, 10th grade November 2014

download word file, 12 pages 0.0


The aim of the experiment conducted is to observe the effects of the amount of catalyst put in hydrogen peroxide [and detergent].

*Amounts of catalyst [Manganese Dioxide MNO2]: 0.1g, 0.2g, 0.3g, 0.4g, & 0.5g


There are there a lot of chemical reactions out there, some work slow, some work fast, and some might or might not take hours to react, and this is where the catalyst come to the rescue. In many chemical reactions, a catalyst is needed to make the reaction happen faster, to do so, it is needed to increase the number of successful collisions. A way of doing so is to provide an alternative way for the reaction to happen which has a lower activation energy. In this case, it is Manganese Dioxide added to Hydrogen Peroxide, and it is an exothermic and an immediate reaction. When Manganese Dioxide was added to Hydrogen Peroxide, it bubbled, it created water and oxygen gas, meaning this is a decomposition reaction, so its equation would be

MnO 2 (s)

2H2O2(aq) ------------> 2H2O(l)+O2(g)

The topic of the catalyst is chosen because with just knowing the existence of the catalyst, it gets interesting to the mind.

With this, the experiment is all about the catalyst. According to 'One Green Generation', the chemical has a job of being a stain remover. Hydrogen peroxide is an oxygen bleach. Oxidizers destroy odors, it destroys both disperse and organic dyes, plus acid and synthetic dyes as well. This is of course a good thing because people would not want coffee smells, or sweet smells, or stinky odors like vomit filling the house' air, or let alone sticking onto their furniture. In other cases such as when the stain has 'settled' on its place, or it has become chemically bonded to the material, and cannot...