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Rates of Reaction Between Magnesium and Hydrochloric Acid

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Rates of Reaction Between Magnesium and Hydrochloric Acid


In my experiment I am going to investigate the rates of reaction. A
2cm strip of Magnesium is placed in a beaker full of Hydrochloric acid
I will then time how long it takes for the magnesium to disappear. The
concentration of the acid will be diluted and timed again. After
collecting these results I will figure out the rate of reaction, and
comment on the trends.


[IMAGE]Magnesium + hydrochloric acid magnesium chloride + hydrogen

[IMAGE]Mg + 2HCl MgCl2 + H2



The experiment was set up as shown in the diagram. The experiment will
be using 100cm3 Hydrochloric acid and will be changing the
concentration every time by diluting the acid by substituting 10cm3 of
acid for 10cm3 of water. We will do this process until we get 60cm3 of
acid and 40cm3 of water, this will give me enough results to plot a

To make this a fair test I will measure the Magnesium strip as
accurately as I can. This will make my experiment a fair test also I
will try to keep the beaker at the temperature by leaving at room
temperature. To make sure I have no major injuries in my experiment, I
will insure I wipe up any spills immediately because hydrochloric acid
is a corrosive chemical, which will burn the skin and wear the safety
classes that are provided.


I think that the more concentrated hydrochloric acid will react with
the Magnesium strip in a shorter time.

I think this because in a more concentrated acid there are more
particles to collide with the magnesium therefore making the reaction

In everyday lives we see rates of reaction, one of these rates of
reaction is the plastic bag. The plastic bag has a very slow rate of
reaction. We know this because it does not react with air or water.
Which means it's a nasty piece of litter!

In my prediction I said that the higher concentrated acid would give
the fastest rate of reaction in the shortest time. I know this from a
past experiment. The past experiment included: -

[IMAGE]Sodium thiosulphate + hydrochloric acid Sulphur + Sodium
Chloride + sulphur dioxide +water




Results table

Concentration of acid

Time (s)

Rate (s-1)

















My graph of time against concentration is a straight line. I also have
a graph of the rate against concentration of acid. This graph is a

This shows my results were quite accurate as if they weren't the graph
wouldn't look right (i.e anomalous results stand out on graphs).

My prediction was right from another experiment the results were very
similar. My overall conclusion is that the concentration is
proportional to the time, but the Concentration is inversely
proportional to the Rate.


To improve my experiment, I would make it more accurate. I would do
this by asking for a second opinion on the length of the Magnesium,
and by using a more precise measuring tool. I believe that this would
have made the experiment a lot fairer and accurate. Also, I could
improve it by making sure that the beakers were all dry before I put
the Hydrochloric acid into them. This would have given me a more
specific result.

To extend my work, I could've gone lower in the concentration. I
could've gone to just water to check if there was a trend in the

Having found this out, I would like to do another experiment to see if
the results are similar.

How to Cite this Page

MLA Citation:
"Rates of Reaction Between Magnesium and Hydrochloric Acid." 20 Apr 2014

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