Investigating the Effect of Concentration of Dilute Hydrochloric Acid with Magnesium Metal
Aim:
To investigate the effect of concentration of dilute hydrochloric acid
when it reacts with magnesium metal.
Scientific Knowledge:
Concentrated acid contains many acid particles. In order for a
reaction to take place acid particles must collide with magnesium
atoms breaking the chemical bonds, there must also be enough energy
within the reaction for them to collide; otherwise they would simply
bounce off each other. A reaction that does have enough energy to
create a reaction is referred to as an effective collision. Within a
reaction containing a high concentration of acid, a collision between
acid particles and magnesium atoms is very likely. The more collisions
made, the quicker the reaction will take place. Therefore using dilute
acid, as there are not as many particles, collisions between the acid
particles and magnesium atoms are less likely causing the reaction to
take more time. Some reactions, such as iron and oxygen, have such a
slow reaction rate, that it can take up to a day to react.
Magnesium + sulphuric acid ==> magnesium sulphate + hydrogen
Mg(s) + H2SO4 (aq) ==> MgSO4 (aq) + H2 (aq)
Magnesium will react with hydrochloric acid because it is higher in
the reactivity series than hydrogen. When the two chemicals react a
displacement reaction will take place and the magnesium will displace
the hydrogen in the hydrochloric acid forming magnesium chloride and
hydrogen gas.
Prediction:
I predict that as the temperature increases due to the reaction, the
reaction will increase further, because at a higher temperature
molecules move around faster as they have more energy, therefore
increasing the likelihood of a collision. I also predict that the
higher the concentration of acid, the quicker the magnesium will react
and dissolve, as in more concentrated acid there are more particles,
also increasing likelihood of a collision.
Apparatus:
* Test Tube Rack
* Strips of Magnesium Ribbon
* Bottle of Sulphuric Acid
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 mass of Mg + the mass of O2=mass of MgxOx. Knowing the mass of
The Effect of Temperature of Hydrochloric Acid on the Rate of Reaction Between Hydrochloric Acid and Magnesium
The aim is to find out if changing the concentration of the hydrochloric acid solution has an effect on the time taken for the reaction. The reaction that will take place is: Hydrochloric acid + Calcium Carbonate + Calcium Chloride + Water + Carbon dioxide 2HCl (aq) + CaCo3 (s) CaCL2 (aq) + H2O + CO2 (g). Collision theory - Collisions between reactant particles are needed. for the reaction to take place in order to form a product.
The Effect of Concentration of Hydrochloric Acid on the Rate of Reaction with Magnesium Aim: To investigate the effect of concentration of hydrochloric acid on the rate of reaction with magnesium Prediction: As the concentration of the hydrochloric acid increases, so will the rate of reaction Hypothesis: In a reaction, particles of two different reactants react together to form a product. The reaction only takes place on account of two things, if the particles collide, and if the collision has enough 'activation energy'. The two reactant particles, in this case magnesium particles and hydrochloric acid particles, must collide with each other on the correct 'collision course'. If this does not occur then no chemical reaction will take place. The reaction must also have enough energy, this can be affected by temperature, the more heat the particles have the faster they move and so the more energy therefore more chance of successful collisions.
The first step that we took to accomplish our goal was to put on our safety goggles and choose a lab station to work at. We received one 400ml beaker, one polyethylene pipet, two test tubes with hole rubber stoppers, two small pieces of magnesium (Mg), one thermometer and a vial of hydrochloric acid (HCl). We took the 400ml beaker and filled it about 2/3 full of water (H20) that was 18 OC. Then we measured our pieces of Mg at 1.5 cm and determined that their mass was 1.36*10-2 g. We filled the pipet 2/3 full of HCl and poured it into one of the test tubes. Then, we covered the HCl with just enough H2O so that no H2O would be displaced when the stopper was inserted. After inserting the stopper, we placed the Mg strip into the hole, inverted the test tube and placed it in the 400ml beaker. HCl is heavier than H2O, so it floated from the tube, into the bottom of the beaker, reacting with the Mg along the way to produce hydrogen gas (H2). We then measured the volume of the H2, cleaned up our equipment and performed the experiment a second time.
Investigation of How Temperature Affects the Rate of Reaction of Sodium Thiosulphate and Hydrochloric Acid
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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.
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