How Does Calcium Carbonate And Hydrochloric Acid Affect The Rate Of Reaction
An investigation in to the rate of reaction
Plan:
I am going to investigate the rate of reaction. The reaction I will be using is:
Calcium Carbonate + Hydrochloric acid ---- Calcium Chloride + water + carbon dioxide.
CaCO3 + 2HCl ---- CaCl +H2O + CO2
Measurements and Variables:
The variables I have chosen to change is strength of the hydrochloric acid which will be 1 mole, 0.7 mole, 0.5 mole, 0.3 mole and 0.1 mole some variable I will not be using are temperature, mass, density.
The measurements I will be using are time (s) and volume in (cm3).
Fair Test:
To make sure this a fair test I will get exact amounts of the Hydrochloric acid and Calcium Carbonate. I will also make sure that the Gas syringe is at zero when I start the …show more content…
This is because as I stated in my plan that if there is a more concentrated solution there will be more particles in a certain area (15cm3) so inevitably there will be more collisions which is backed up by the collision theory. The Collision Theory is based on the idea that for a chemical reaction to take place, it is necessary for the reacting particles to collide with each other with enough energy to break or form new bonds between the other particles, which is called a successful collision. If when they collide and they do not have enough energy to break or form new bonds then they will simple bounce of each other, causing an unsuccessful …show more content…
I followed my safety precautions by wearing goggles at all times, washing my hands after the experiment and I was very cautious when handling acid. I got one anomalous result which is pointed out on my graph showing rate of reactions, I think this is due to one of the three tests being to different on my 0.3 mole tests.
I think that the test was fair to a certain extent but their was a few problems such as not being able to put the rubber plug quick enough before the carbon dioxide was released and also that the gas syringe got stuck a couple of times. Additional evidence to support my conclusion could have included more justifiable scientific knowledge that fitted my evidence. To extend my investigation further I could use the other to methods and see if I get a similar result, which will show me if this investigation was a success or not.
If I were to repeat this experiment again I would try and find a more efficient way of mixing the Hydrochloric acid with the calcium carbonate without losing any carbon
Plan:
I am going to investigate the rate of reaction. The reaction I will be using is:
Calcium Carbonate + Hydrochloric acid ---- Calcium Chloride + water + carbon dioxide.
CaCO3 + 2HCl ---- CaCl +H2O + CO2
Measurements and Variables:
The variables I have chosen to change is strength of the hydrochloric acid which will be 1 mole, 0.7 mole, 0.5 mole, 0.3 mole and 0.1 mole some variable I will not be using are temperature, mass, density.
The measurements I will be using are time (s) and volume in (cm3).
Fair Test:
To make sure this a fair test I will get exact amounts of the Hydrochloric acid and Calcium Carbonate. I will also make sure that the Gas syringe is at zero when I start the …show more content…
This is because as I stated in my plan that if there is a more concentrated solution there will be more particles in a certain area (15cm3) so inevitably there will be more collisions which is backed up by the collision theory. The Collision Theory is based on the idea that for a chemical reaction to take place, it is necessary for the reacting particles to collide with each other with enough energy to break or form new bonds between the other particles, which is called a successful collision. If when they collide and they do not have enough energy to break or form new bonds then they will simple bounce of each other, causing an unsuccessful …show more content…
I followed my safety precautions by wearing goggles at all times, washing my hands after the experiment and I was very cautious when handling acid. I got one anomalous result which is pointed out on my graph showing rate of reactions, I think this is due to one of the three tests being to different on my 0.3 mole tests.
I think that the test was fair to a certain extent but their was a few problems such as not being able to put the rubber plug quick enough before the carbon dioxide was released and also that the gas syringe got stuck a couple of times. Additional evidence to support my conclusion could have included more justifiable scientific knowledge that fitted my evidence. To extend my investigation further I could use the other to methods and see if I get a similar result, which will show me if this investigation was a success or not.
If I were to repeat this experiment again I would try and find a more efficient way of mixing the Hydrochloric acid with the calcium carbonate without losing any carbon