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Chemsitry Coursework

Chemistry Coursework
An investigation: Reacting magnesium with hydrochloric acid
Introduction
Experiment equation =
Magnesium + Hydrochloric acid Magnesium Chloride + Hydrogen
Mg + 2HCl MgCl2 + H2
The aim of the experiment is to investigate how the concentration of hydrochloric acid affects the rate of reaction with magnesium, i.e. how quickly/how much hydrogen is produced.
The factors that may affect the rate of reaction are as follows:
• Temperature of the Hydrochloric Acid
• Catalyst

The effect of temperature
is taking place, the particles move more quickly. This has two effects:
1) More collisions take place
lead to a reaction, because the activation energy is higher so the reactions will be more successful.
The effect of concentration
The concentration of a solution is how strong the solution is. In this leads to a greater frequency of collisions so the rate of the increases.
The Effect of surface area
increases the number of collisions. The energy of the particles remains the same.

Catalyst
To increase the rate of a reaction you need to increase the number of successful an alternative which has a lower activation energy. On a graph it would look like this

Chosen Factor- I have chosen to use concentration as my variable.

Prediction
I in the same volume. With a more concentrated acid, the number of acid particles is of colliding successfully.

Key-
Magnesium particles-
Hydrochloric acid particles-
The higher the, which means there will be more successful collisions per second, so the rate of reaction in the reactivity series than hydrogen. When the two chemicals react a displacement reaction will take place and the magnesium will displace the hydrogen in the hydrochloric acid forming magnesium chloride.
Ways that I could record my experiment
(1) I could use a gas syringe to collect the gas that will be the product of my experiment. Increasing the concentration of acid molecules increases the...