Investigating How Concentration of Acid Affects the Reaction Between Calcium Carbonate and Hydrochloric Acid Essay Example
Investigating How Concentration of Acid Affects the Reaction Between Calcium Carbonate and Hydrochloric Acid
Introduction
============
According to the collision theory temperature, concentration, surface
area and catalysts all affect rates of reaction as shown in the
diagrams below. Increasing any of these should increase the number of
collisions and so increase the reaction rate up to an optimum point.
Increasing the temperature causes the particles to collide with more
energy and more frequently, thereby increasing the reaction rate.
Surface area is like concentration in that the greater numbers of
particles present means that a useful collision is more likely
(collision theory). Catalysts provide a surface area for reactions to
take place on and so also increase the chances of a reaction.
I will be investigating concentration and how it affects the rate of
reaction in the reaction between calcium carbonate and hydrochloric
acid. Concentration will be my variable (different mole) and the only
thing to be changed each time. Temperature can change easily and is
difficult to keep constant and surface area is very difficult to
measure and almost impossible with chips of marble. No catalysts were
available for use so I could not investigate this leaving me with my
choice of concentration as the variable in the reaction below:
CaCO + 2HCL à CaCL + H O + CO
Calcium Carbonate + Hydrochloric acid à Calcium Chloride + Water +
Carbon Dioxide
Temperature Surface Area
Concentration Catalyst
Prediction
==========
If a solution (HCL) is made more concentrated it means that there are
more particles of reactant colliding between the water molecules,
which makes collisions between the reactants (HCL and Calcium
carbonate) more likely and so increasing the rate of reaction. From
this theory I predict that the higher the concentration, the quicker
the rate of reaction will be, shown by the
Introduction
============
According to the collision theory temperature, concentration, surface
area and catalysts all affect rates of reaction as shown in the
diagrams below. Increasing any of these should increase the number of
collisions and so increase the reaction rate up to an optimum point.
Increasing the temperature causes the particles to collide with more
energy and more frequently, thereby increasing the reaction rate.
Surface area is like concentration in that the greater numbers of
particles present means that a useful collision is more likely
(collision theory). Catalysts provide a surface area for reactions to
take place on and so also increase the chances of a reaction.
I will be investigating concentration and how it affects the rate of
reaction in the reaction between calcium carbonate and hydrochloric
acid. Concentration will be my variable (different mole) and the only
thing to be changed each time. Temperature can change easily and is
difficult to keep constant and surface area is very difficult to
measure and almost impossible with chips of marble. No catalysts were
available for use so I could not investigate this leaving me with my
choice of concentration as the variable in the reaction below:
CaCO + 2HCL à CaCL + H O + CO
Calcium Carbonate + Hydrochloric acid à Calcium Chloride + Water +
Carbon Dioxide
Temperature Surface Area
Concentration Catalyst
Prediction
==========
If a solution (HCL) is made more concentrated it means that there are
more particles of reactant colliding between the water molecules,
which makes collisions between the reactants (HCL and Calcium
carbonate) more likely and so increasing the rate of reaction. From
this theory I predict that the higher the concentration, the quicker
the rate of reaction will be, shown by the