Chemistry Coursework
Rates of Reaction Investigation
This investigation is based upon the theories of rates of reactions.
The RATE OF REACTION is HOW FAST the reaction is. Reactions work at both slow and fast rates and the one I will be testing is an example of a fast reaction.
2HCL + Mg MgCl 2 + H2
In my experiment I intend to investigate the effect of both concentration and temperature on the rate of reaction.
From the results acquired I intend to come up with a practical value for the activation energy ( EA ) and deduce a possible order of reaction with respect to [HCL].
Knowing that generally a 10K rise will cause the rate to double I'm going to try and get practical evidence of this.
As we know, an increase in both temperature and concentration ( there are other affecting elements which could be investigated) will increase the rate of reaction by a given amount.
The COLLISION THEORY and the TRANSITION STATE THEORY support these 'beliefs'.
The Collision theory states that a collision must occur between two molecules A and B ( HCL and Mg) for a reaction to take place. This explains why reaction rates increase with increased concentration; if there are more molecules per cubic centimetre collisions will occur more frequently.
As molecules move faster when the temperature increases there will be more collisions per second and the molecules will also hit each other with more energy.
If we know the temperature and therefore the speeds of the reacting molecules and their concentrations it is possible to calculate the exact number of collisions per second.
Rates of Reaction Investigation
This investigation is based upon the theories of rates of reactions.
The RATE OF REACTION is HOW FAST the reaction is. Reactions work at both slow and fast rates and the one I will be testing is an example of a fast reaction.
2HCL + Mg MgCl 2 + H2
In my experiment I intend to investigate the effect of both concentration and temperature on the rate of reaction.
From the results acquired I intend to come up with a practical value for the activation energy ( EA ) and deduce a possible order of reaction with respect to [HCL].
Knowing that generally a 10K rise will cause the rate to double I'm going to try and get practical evidence of this.
As we know, an increase in both temperature and concentration ( there are other affecting elements which could be investigated) will increase the rate of reaction by a given amount.
The COLLISION THEORY and the TRANSITION STATE THEORY support these 'beliefs'.
The Collision theory states that a collision must occur between two molecules A and B ( HCL and Mg) for a reaction to take place. This explains why reaction rates increase with increased concentration; if there are more molecules per cubic centimetre collisions will occur more frequently.
As molecules move faster when the temperature increases there will be more collisions per second and the molecules will also hit each other with more energy.
If we know the temperature and therefore the speeds of the reacting molecules and their concentrations it is possible to calculate the exact number of collisions per second.