An investigation to find out how the concentration of acid affects the rate of reaction between hydrochloric acid and calcium carbonate
(magnesium ribbon)
Planning
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The aim of my investigation is to find out how changing the concentration of acid affects the rate of the reaction between CaCO3 and HCl. To make my experiments fair tests, I will only change one variable: the concentration of the acid. I will have to keep the volume of the acid, the mass and size of the marble chips and the temperature of the acid the same in all my experiments to insure a fair test, because by changing any of the above I will change the conditions and therefore the results will be inaccurate and the rate of reaction will be affected.
The products of the reaction between the hydrochloric acid and the magnesium ribbon are calcium chloride, water and carbon dioxide.
CaCO3 (s) + 2HCl(aq) CaCl2 (l) + H2O (l) + CO2 (g)
As CO2 is a gas it will escape as the reaction is taking place, therefore there will be a mass loss. Following from that I have decided to monitor this mass loss by weighing my components on a set of scales as the reaction takes place, the conical flask with the reactants will be constantly on the scales and I will be reading the mass of the display every 10 seconds. I will use 5 different concentrations of the acid. The strongest concentration will be 2 molar and the weakest will be 0.4 molar. The different concentrations will be obtained by adding a certain volume of water to the acid to dilute it this will reduce the concentration.
GRAPH
I predict that the higher concentration of the acid will have a much faster rate of reaction than the weaker solution, i.e. the mass loss will be more rapid. This is because a higher concentration of acid will contain more acid molecules per a set volume than low concentration solution. This means that there will be a higher chance of the calcium carbonate molecules colliding with the hydrochloric acid molecule and reacting.
According to the collision theory, reactant particle have to collide in order for the reaction to form a product in this case (calcium chloride, water and carbon dioxide). However not all the collisions are successful and if there is not enough energy the molecules will simply rebound.
We began this investigation by suiting up in lab aprons and goggles, we then gathered our materials, found a lab station and got to work. We decided to start with the magnesium in hydrochloric acid first, we measured out 198.5 L of HCl and put it in the foam-cup calorimeter and took initial temperature reading. We then selected a piece of magnesium ribbon and found its mass: 0.01g. This piece was placed in the calorimeter and the lid was shut immediately to prevent heat from escaping. We “swirled” the liquid mixture in the calorimeter to ensure a reaction, and waited for a temperature change. After a few moments, the final temperature was recorded and DT determined.
The Effect of Temperature of Hydrochloric Acid on the Rate of Reaction Between Hydrochloric Acid and Magnesium
Hydrochloric acid + calcium carbonate arrow calcium chloride + carbon dioxide + water. HCl(aq) + CaCO3(s) arrow CaCl2(aq) + CO2(g) + H2O(l) Things that affect the reaction rate of this experiment are: 1. The temperature of the hydrochloric acid. 2.
Rate of Reaction Between Marble Chips and Hydrochloric Acid. The aim of this experiment is to find out how different variables affect the rate at which the reaction between Marble chips (CaCO ) and Hydrochloric acid (HCl) is used. There are many variables that affect the rate of this reaction such as the following. 1.
the acid was at 14 C the magnesium took 141 seconds to react and 27 C
The Effect of Temperature on the Rate of Reaction Between Hydrochloric Acid and Calcium Carbonate
If there is not enough energy no reaction takes place. In a solution of 0.5M hydrochloric acid, there are less hydrochloric acid particles compared to that of 2M hydrochloric acid, therefore, there are less particles to react with magnesium particles thus meaning less chance of collisions between the two reactants: [IMAGE] Therefore, as the concentration of the hydrochloric acid is increased, the chances of collisions increase thus giving a faster rate of reaction. Apparatus: Beaker Hydrochloric acid Distilled water Measuring cylinder Pipette Test tubes Test tube rack Diagram: [IMAGE] Method: Measure out 10cm3 of hydrochloric acid, as the concentration requires, for each concentration its composition is: Moles Volume HCl Volume Water 2M 10 cm³ 0 cm³ 1.5M 7.5 cm³ 2.5 cm³ 1M 5 cm³ 5 cm³ 0.5M 2.5 cm³ 7.5 cm³ 0M 0 cm³
Experiment is to investigate the rate of reaction between hydrochloric acid and calcium carbonate Hydrochloric acid + Calcium Carbonate Þ Calcium Chloride + Water + Carbon Dioxide 2HCl (aq) CaCo3 (s) CaCl2(s) H2O (aq) CO2 (g) There are a number of variables in this experiment and these are listed below as input variables and outcome variables.
will result in an increase in the speed of the rate of reaction it has
from 10cm to 50cm to make it easier to see the difference in a graph.
* Concentration - I will try my best to use all the acid from the
If they collide with sufficient energy, then they will react. The minimum amount of kinetic energy required for particles at the time of collision is called the activation energy and this theory is known as the?collision theory?. Reactions occur in all circumstances. Chemicals are always combining and breaking up. Reactants and products combine and break apart in all reactions.
Conclusion This experiment was set out to find the effect of different temperatures of hydrochloric acid on the rate of reaction with magnesium. The information recorded was then interpreted and compared to the hypothesis. From this information, a conclusion can be made to show that the rate of reaction relates to temperature in the reaction between hydrochloric acid and magnesium. In conclusion, as proven in this experiment, the higher the temperature of hydrochloric acid, the faster the reaction it has with magnesium.
Investigating How the Concentration of Hydrochloric Acid Affects the Rate of Reaction with Calcium Carbonate
An investigation into how changing one variable influences the rate of reaction between marble chips and dilute Hydrochloric acid