Rate of Chemical Reaction between Magnesium and Hydrochloric Acid
Aim: -
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I plan to investigate the effect of temperature, to see if it
increases or decreases the rate of reaction between magnesium and
hydrochloric acid.
Prediction: -
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I predict that as the temperature of the hydrochloric acid increases,
the quicker the rate of reaction will be. This is due to the molecules
in the hydrochloric acid gaining energy from the heat. Consequently,
the molecules have increased kinetic energy, which will produce more
activation energy. The particles will have more successful collisions
resulting in a faster reaction rate.
No heat Heat present
Lines of reaction
[IMAGE]
Mg turnings
Beaker
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Hcl
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The above diagram show that when there is more heat present there are
more lines of reaction than if there was less heat. This is due to the
number of successful collisions being far greater when the
hydrochloric acid is heated.
I predict also that if I did a graph showing the volume of gas against
time it would look like the following.
[IMAGE]
From the above graph you can see that when the Time Increases the
volume of gas being produced goes up, then it levels off. It levels
off because the volume of hydrogen gas being produced is slowing down
because all the magnesium and hydrochloric acid is being used up.
Fair test
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In order to keep my experiment as fair as possible I will have to make
sure I keep the following factors the same: -
Volume of acid (25cm3)
Mass of Magnesium (0.1g)
I will make sure the gas syringe is connected correctly and securely
to the side arm conical, so no hydrogen gas can escape.
I will start the syringe at 0 for each run.
Also I would make sure to put the bung on quickly, to prevent the
hydrogen gas escaping.
As the temperature increases, the movements of molecules also increase. This is the kinetic theory. When the temperature is increased the particles gain more energy and therefore move around faster. This gives the particles more of a chance with other particles and with more force.
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
You can speed up the reaction by stirring the solution. 8. You can also change the rate of the reaction by adding a catalyst, which is something that speeds up the reaction. In my experiment I will change the temperature of the hydrochloric acid. I will not change anything else; I will keep the amount of calcium carbonate, the form of calcium carbonate, the concentration of hydrochloric acid, the surface area of the calcium carbonate and the amount of hydrochloric acid all the same.
The number and strength of collisions is increased so that the reaction can happen faster than it should. If the particles have more energy then more particles will be able to react to it. Solid reactants like marble chips are affected by surface area. The larger the surface area, the more collisions that will take place.
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
The reason I believe this is that chemical reactions occur when particles of the reacting substances collide. Increasing the number of the particles increases the number of collisions per second and this increases the reaction rate. In the reaction between hydrochloric acid and calcium carbonate you can increase the number of particles in two ways. The first of these is to increase the surface area of the calcium carbonate.
from 10cm to 50cm to make it easier to see the difference in a graph.
There is not really that much I can do to help make this experiment a
To make sure it was a fair test. i had to constantly keep cleaning and
My aim in this piece of work is to see the effect of temperature on the rate of a reaction in a solution of hydrochloric acid containing sodium thiosulphate.
It is also important we keep the colour and size of the cross the same this will help keep the results fair for the experiment. Another thing we must do is to make sure that the beaker is completely clean and free of any water or any other substance before we attempt to start the next experiment.
Effect of Temperature on the Rate of Reaction between Sodium Thiosulphate and Hydrochloric Acid Investigation Chemical reactions are used in our everyday life, they literally keep us alive. They are used in food, respiration and everywhere else in the environment. A chemical reaction mainly occurs when reactants react together to produce a new product. The speed at which this reaction takes place is called the rate of reaction. The product produced has a number of particles in the solution that has formed from the reactants.
3 cm of magnesium ribbon generally has a mass of 0.04 g and yields 40 cm3 of hydrogen when reacted with excess acid. 50 cm3 of 1M hydrochloric in this experiment is in excess.