Investigating the effect of varying concentration on the reaction between magnesium ribbon and hydrochloric acid
It is to tell how the reaction between magnesium and hydrochloric acid
will be effected if we change the concentration of hydrochloric acid.
In the experiment the magnesium reacts with the hydrochloric acid to
create magnesium chloride and hydrogen. The balanced formula for this
Mg(s) + 2HCL(aq) MgCl2(aq) + H2(g)
Magnesium + hydrochloric acid Magnesium Chloride + Hydrogen
Magnesium will react with hydrochloric acid, because it is higher in
the reactivity series than hydrogen. The magnesium displaces the
hydrogen in the acid, so it forms magnesium chloride and hydrogen gas.
Hydrochloric acid particles
There are many variables that I can change, which are the temperature
and concentration of the hydrochloric acid, and the mass and the
surface area of the magnesium strip. This is all true because they all
link to the collision theory of particles colliding with enough energy
to make a reaction. It is based on the idea that for a chemical
reaction to take place, the reacting particles have to hit each other
hard enough to break or form new bonds. This is called a successful
collision. When particles get stimulated or increased in number, the
reaction will increase in rate because faster collisions will take
place making more successful collisions.
This diagram shows five solutions hydrochloric acid and magnesium
ribbon that are reacting. The arrows represent a simplified way to
show how many successful collisions occur each second; therefore the
more arrows there are, the faster the rate of reaction. They show how
different factors can affect the rate of reaction against these two
reactants (magnesium and hydrochloric acid). The original diagram shows
how the solution will be with 1M hydrochloric acid and 5cm of magnesium
strip. This is to compare with the other diagrams to see what the change
is and if the reaction rate has decreased or increased.
The first one is to see what will happen if I change the temperature
of the solution. As the temperature increases the speed and the power
at which the acid particles hit each other increases, making the
number of successful collisions with the magnesium strip increase.
The second one is to show how increasing the mass of the magnesium
strip can increase the rate of reaction slightly because of the
increased surface area but it is only slightly increased on the sides
and so this is proportional to the rate of reaction of the original
diagram. It is only slower than the original reaction because there is
more of it to react with and produces more of the products.
Figure 3 shows the concentration of the hydrochloric acid increased so
there are more particles to have more successful collisions. This is a
faster reaction then the original reaction.
The final reaction has the same amount of particles of acid and the
magnesium, but the...