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Investigating chemical reactions lab report
Observing chemical reactions lab
Investigating chemical reactions lab report
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.Experiment for Chemistry Coursework
For this investigation I am looking at how the concentration of acid can change the reaction and how I can explain this using collision theory.
My Prediction: I predict that the greater amount of concentration the faster the reaction will take place. Therefore, particles in the two compounds will collide faster. Due to my prediction if it is correct, I expect to see the cross on the paper disappear faster. As I already know that increasing one quantity will speed up the reaction as the particles are more likely to collide.
In this investigation several measures will need to be done to make sure that the results I get will be precise. From the planed method I can work out what will need to be done to achieve the best results possible. I will also need to think about what other factors may vary my results to someone else’s and how this could be improved.
Equipment Needed:
· Beaker
· Test-tube
· Piece of paper with a cross on
· 25ml² of Sodium Phiosulphate
· 5ml² of Hydrochloric Acid
Factors about the equipment that may affect the results:
The amount of one particular quantity, or concentration of the acid. The type of acid that was used may either slow down or speed up the reaction. Also, another factor maybe that the time it take until I begin to start the stopwatch. To control the problem of affecting results I would have to swirl the mixture for e.g.: every 2 seconds. However, this would have to be done in every type of concentration and experiment.
Diagram of method:
Method: Draw a cross on a piece of paper and place a beaker on top of the paper. This is because once the cross disappears I know the reaction has completed as the compounds have now become one solution.
Secondly, measure as accurately as possible 25ml² of Sodium Phiosulphate and 5ml² of Hydrochloric acid.
Thirdly, pour the measured amount of Sodium Phiosulphate into the beaker and then add the Hydrochloric acid. Once this is added start the timer.
Finally, once the cross has completely disappeared stop the clock and make a not of the time it took for the mixture to become one.
NOTE: This procedure was produced with different concentrations. This was so that I could see whether the concentration had an affect on experiment’s time limit.
Results:
Before doing our experiment we saw a trail run on the computer known as:
Objective: The objective of the experiment is to determine what factors cause a change in speed of a reaction. It is also to decide if the change is correlated with the balanced equation of the reaction and, therefore, predictable. To obtain a reaction, permanganate, MnO_4^(1-), must be reduced by oxalic acid, C_2 O_4 H_2. The balanced equation for the reaction is:
Input variables In this experiment there are two main factors that can affect the rate of the reaction. These key factors can change the rate of the reaction by either increasing it or decreasing it. These were considered and controlled so that they did not disrupt the success of the experiment. Temperature-
The objective of this experiment will be to combine various substances, liquids and metals, and to observe their behavior when they are combined. The types of reactions observed shall determine the nature of these reactions: physical or chemical.
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 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.
If the number of collisions per second increases then the reaction rate will increase. This is demonstrated in diagram 2 of appendix 2. In order to gain perfect results I would have to use the following weights of each component of the formula and introduce nothing else into the equation. All of the weights are in grams CaCO3 + 2HCl Þ
Two catalyst reactants are used in the experiment, thiosulfate and starch, to dictate the time of reactions.
$ 3. Allow the zinc d hydrochloric acid to set over night to make sure that the reaction reaches completion.
Do all trials in the experiment on the same in order to make everything as similar as possible prior to beginning testing.
2. In the large beaker, put water and boil it completely. After that, remove the beaker from heat. 3. Sample tubes (A-D) should be labeled and capped tightly.
In a 100ml beaker place 50mls of water, measure the temperature of the water and record this initial temperature onto a table. Set the timer and add one teaspoon of Ammonium Nitrate to the water, stir this continuously until the Ammonium Nitrate has dissolved.
We have no gases and solids involved, therefore it is easy to deal with solutions. Similarly, the use of a catalyst complicates things, and if used incorrectly could alter the outcome of the experiment. The theory behind this experiment is that increasing the concentration can increase the rate of the reaction by increasing the rate of molecular collisions. GRAPH I will place the reaction mixture on a paper with a black cross drawn on it. When the cross is completely obscured, the reaction will be finished.
There are many issues which may arise in regard to cross-cultural conflict, from both sides of the interaction. It is acknowledged, for instance, that this writer, like everyone else, has his own preconceptions that will influence how he processes data and behave, and which are primarily due to the ‘accident’ of his cultural up-bringing. These ‘prejudices’ may influence the way he works with others, especially if they go unrecognised by him.
made in a certain time. The rate of reaction can be made faster by an