An Investigation into the reaction between magnesium and hydrochloric acid

*Scissors (to Cut The Mg)                                                                                           *H2 Cl3
*Tube With Polostyrene Exterior

 Variables

I have chosen to repeat the experiment 3 times because it therefore allows me to calculate an average rate of reaction. This will ensure that there are no abnormal results and it will increase accuracy. I have decided to start readings at 2cm and increase by 1cm each time until 7cm is reached, since it will allow me to see the increase in rate of reaction and 6 results should be enough to identify any trends.


Rates of Reaction

Increasing the temperature increases the speed of the particles. The faster the particles move, the greater the number of collisions, and therefore the rate of the reaction increases. An amount of Mg that can make the temp rise by 10C almost doubles the rate of most reactions and cause further increases.
Chemical reactions take place by chance. Particles need to collide with enough velocity so that they react. As the temperature is increasing the particles move faster since they have more energy. This means that they are colliding more often and more of the collisions have enough velocity to cause a reaction. Since there are more collisions the chemical reaction takes place faster.


Analysing Evidence



As the Length increases so does the Temp Increase by reaction. Increasing the temperature by Reaction increases the speed of the particles. The faster the particles move, the greater the number of collisions, and therefore the temp Increase by reaction increases.
Chemical reactions take place by chance. Particles need to collide with enough velocity so that they react. As the temperature is increased the particles move faster since they have more energy. This means that they are colliding more often and more of the collisions have enough velocity to cause a reaction. Since there are more collisions the chemical reaction takes place faster.
In my design I predicted that as the temperature increased the rate of reaction would increase. I predicted that for every 1cm increase in Length the rate of Temp Increase by reaction. I was correct that as the Length increases so does the rate of temp Increase.



Evaluating Evidence

I believe that the experiment was successful but some of the results were unexpected.  
I believe that the experiment was designed well but there were a few problems. Although the initial Temp Increase (which is what I am concerned with in this investigation) seemed to fit a trend, the Temp Increase curves of some Point on the graph Don't Fit. This could have been because some of the magnesium had corroded forming a magnesium oxide layer which would have affected the Reaction.
To improve the experiment I would find a way to Absolutly purify the mg so that the magnesium could be dropped into the acid as pure as it can get.
Additional work, which could be carried out, is to repeat the experiment using, a wider range of Length. The investigation could also be extended to investigate other factors affecting the Temp Increase such as catalysts, concentration of the acid or particle size of the magnesium.