Investigating how changing the concentration of hydrochloric acid
affects the rate of its reaction with magnesium metal.
Introduction:
During a chemical reaction, old bonds are broken and new bonds formed
thus creating a new substance. In order for bonds to be broken there must
be a supply of energy, however, when bonds are formed energy is
released. This means that bond breaking is an endothermic reaction and
bond forming an exothermic reaction. This bond breaking and forming
can be done faster or slower depending on the rate of the reaction.
The rate of a reaction is dependent upon the number of collisions the
molecules have in any set time. This is the theory I shall be testing in this
experiment. To test this I must take into consideration the factors which
affect the rate of reaction. The main ones are: Concentration of the
reactants, for instance if I had a lower amount of hydrochloric acid the
reaction would be slower because concentration affects rate; the
temperature at which the reaction takes place, for example most reactions
happen quicker at higher temperatures but if I was experimenting with an
enzyme the reaction would work best at a certain temperature like 37?c for
body enzymes; surface area of the magnesium, i.e. whether I will keep it in
one large piece or cut it into evenly sized smaller pieces so I may cover a
larger surface area and have more collisions thus increasing the reaction
rate.
The equation for this reaction is:
Mg(s) + 2Hcl(aq) =Mgcl2(aq) +H2(g)
Prediction:
I think that if I change the concentration of the acid by lowering it the rate
of the reaction will be similarly lowered or decreased. I think this because,
if the hydrochloric acid has a lower concentration it will have less
collisions with the magnesium metal, causing less bonds to break and
slowing the reaction rate.
Theory:
Reactions only happen if the particles collide with enough energy. At a
higher temperatures there will be more particles colliding with enough
energy to make the reaction possible. This 'initial energy' is known as
activation energy and is needed to break initial bonds.
The rate of a reaction can be explained by the collision theory. The
collision theory states that the rate of any reaction is dependent upon how
hard or often the reactants collide with each other. This rate can be
measured in three main ways: Precipitation, Change in mass -usually when
a gas is given off, and the volume of gas given off- using a gas cylinder.
The main ways of increasing the rate of reactions can be explained in
terms of increasing the number of collisions between the particles.
For example:
affects the rate of its reaction with magnesium metal.
Introduction:
During a chemical reaction, old bonds are broken and new bonds formed
thus creating a new substance. In order for bonds to be broken there must
be a supply of energy, however, when bonds are formed energy is
released. This means that bond breaking is an endothermic reaction and
bond forming an exothermic reaction. This bond breaking and forming
can be done faster or slower depending on the rate of the reaction.
The rate of a reaction is dependent upon the number of collisions the
molecules have in any set time. This is the theory I shall be testing in this
experiment. To test this I must take into consideration the factors which
affect the rate of reaction. The main ones are: Concentration of the
reactants, for instance if I had a lower amount of hydrochloric acid the
reaction would be slower because concentration affects rate; the
temperature at which the reaction takes place, for example most reactions
happen quicker at higher temperatures but if I was experimenting with an
enzyme the reaction would work best at a certain temperature like 37?c for
body enzymes; surface area of the magnesium, i.e. whether I will keep it in
one large piece or cut it into evenly sized smaller pieces so I may cover a
larger surface area and have more collisions thus increasing the reaction
rate.
The equation for this reaction is:
Mg(s) + 2Hcl(aq) =Mgcl2(aq) +H2(g)
Prediction:
I think that if I change the concentration of the acid by lowering it the rate
of the reaction will be similarly lowered or decreased. I think this because,
if the hydrochloric acid has a lower concentration it will have less
collisions with the magnesium metal, causing less bonds to break and
slowing the reaction rate.
Theory:
Reactions only happen if the particles collide with enough energy. At a
higher temperatures there will be more particles colliding with enough
energy to make the reaction possible. This 'initial energy' is known as
activation energy and is needed to break initial bonds.
The rate of a reaction can be explained by the collision theory. The
collision theory states that the rate of any reaction is dependent upon how
hard or often the reactants collide with each other. This rate can be
measured in three main ways: Precipitation, Change in mass -usually when
a gas is given off, and the volume of gas given off- using a gas cylinder.
The main ways of increasing the rate of reactions can be explained in
terms of increasing the number of collisions between the particles.
For example:
