Hydrogen Peroxide

... a higher concentration although the temperature stays the same there will be a higher chance that because there are more molecules there will be more successful reactions, and so the overall reaction will occur much faster.

From the research I have carried out, I have found information that shows clearly one molecule hitting another and combining to form and end produce. This is shown clearly below. The bottom diagram shows us how one molecule collides with another, then hit the transition state and then at the end forming a different compound. The graph above shows us how the energy increases as the two reactants collide and combine and then slowly loose its energy when it has finally formed the end product. But again all this depends on the two molecules when collided actually reacting, because in some cases this does not happen, also the transition state does not always proceed to the products of the reaction - it can also return back to reactant molecules. So from this we know that the Hydrogen peroxide might not decompose when it hits the enzyme and so not all of the H2O2 might be used and so we are not getting the maximum amount oh H2O2.

These are the results I collected after my experiments:

Concentration Oxygen produced Average Produced Time (min) H2O2 + H2O In ml3 In ml3 10 5.8 5 10 7.2 6.4 5 10 6.4 5 8+2 5 5 8+2 5.2 5.4 5 8+2 6 5 6+4 4 5 6+4 3.5 3.9 5 6+4 4.4 5 4+6 2 5 4+6 1.8 1.7 5 4+6 1.4 5 2+8 1.4 5 2+8 2.2 1.6 5 2+8 1.2 5 From the results I had collected I hav ...