Find Out About Collision Theory and Use It to Explain What Is Happening on Each Graph for Each Graph for Each Different Factor and Why You Observed the Change When a Catalyst Was Added to the Hydrogen Peroxide.

1. The collision theory is explained by reaction rates, the rate of reaction depends on how often and how hard the reacting particles collide with each other, they must collide in order for them to react.

When investigation different concentration the graph is the steepest for 2M concentration, thus illustrating reaction rate is fastest. This is because the solution is more concentrated which means there are more particles of reactants knocking about between the molecules, which makes collision more likely to occur.

When investigating different temperature the graph is steepest at the hottest temperature, and therefore rate of reaction is highest at this point. The reason for this is because when the temperature is increased the particle start moving faster, this will increase the chances of successful collision therefore increasing the rate of reaction. At low temperature the particles don’t move fast enough to collide often therefore showing a slow rate of reaction this can be seen in the graph by a flat slope.

When investigating surface area and rate of reactions, smaller particle have a higher surface area therefore they increase rate of reaction, as particles have more area to work on so there’ll be more useful collisions. Hence the graph is steepest when surface area is highest.

During the experiment when a catalyst was added to the hydrogen peroxide the rate of reaction increased this is because   the catalyst gives   the reacting particles a surface to stick to where they can bump into each other thus increasing the amount of successful collisions.

2. Why is it important to know how to change the rate of a chemical reaction in industry?
This will allow you to increase the rate of reaction, therefore making reactions happens quicker so you save time, energy and money.

3. If you make a reaction faster how might this affect the cost of the process? Will it always be a good idea to make a reaction happen faster?
You can make you product faster...