This means that both graphs drawn up in my analysis will have positive correlation, and will probably be curved as the increase in rate of reaction ill not be exactly the same as the counterrevolutionaries is increased. Next I will place the Chemistry coursework sodium thiosulphate conclusion flask on top of the cross, pour 5cm3 of hydrochloric into the hot sodium thiosulphate solution and time how long it takes for the cross to disappear.
This increases the probability of reactant particles colliding with each other.
There are 2 outliers Improvements and further investigations: I have chosen to investigate the effect temperature and concentration have on a reaction. I first picked the type of experiment I was going to do. I probably did not encounter any outliers because the precision and the accuracy I applied to my investigation during timing or measuring etc.
This would make my investigation more of a fair test because during my experiment I used a stronger concentration of the STS solution and so it would have been better if I used the stronger HCL solution. I stood up to allow more space for others to walk by between the rooms. Below are diagrams to illustrate and explain my method Fair Test To ensure that this experiment is fair I will control the variables, i.
I probably did not encounter any outliers because the precision and the accuracy I applied to my investigation during timing or measuring etc. Once I decided the concentration I then carried out my experiment. Strategy According to my results, as the concentration of STS solution increased the rate of reaction of my experiment was increased.
Taking temperature into consideration if I did not control this my results would be inaccurate. This ensures that the solution is completely opaque when I stop the timer. By doing so it made my experiment a fair test as I was controlling other variables such as HCL. The water is placed on top of a Bunsen on a blue flame and the two measuring placed inside the water bath.
This might have occurred for several different reasons, such as the fact that the temperature control might not have been exactly the same or that my judgement of when the cross may have disappeared might not have been exactly the same for each one.
Below is a table to show the effect of changing different variables. A small increase in temperature greatly increases the number of particles with energy greater than the activation energy.
If by chance I found an outlier I would not count it with the rest of my results and I would repeat that test again. However in the 2 molar STS solution the rate of reaction was quick. I am investigating the different factors which may speed up chemical reactions.
In my experiment I applied H20 so that I could see the rate of reaction through a more dilute solution. I also feel very confidant that my investigation went well.
I recorded my results using a timer just to see if the experiment worked. I will keep everything constant apart from the variable I am changing-temperature. In addition the safety rules made my experiment a fair test.
I will then put 40cm3 of sodium thiosulphate into a conical flask and place it on a tripod and gauze. An increase in the frequency of collisions can be achieved by increasing the concentration, pressure, or surface area.
Evaluation All of my results were accurate and fitted the pattern of results. The variable I changed was the volume of STS and the volume of water.
This is because as the temperature increases, the reactant particles move more quickly. These are circled on my graphs. This causes a quicker reaction. Therefore the data I obtained looks very reliable. The peak is at a higher energy. Where as when the STS was at 40ml the average time was 32 seconds which shows a very big relationship between the amount of STS and the time taken.
I am very confident with my results and I can feel that my investigation was very precise, accurate and my results were extremely reliable. Collisions between reacting particles are therefore more likely to occur.
This makes sure that my experiment runs smoothly. This is because as the temperature increases, the reactant particles move more quickly.GCSE SCIENCE COURSEWORK (CHEMISTRY) PLANNING: Skill Area P.
Write down the aim of your Investigation. To investigate the effects of change in concentration on the rate of reaction between Sodium Thiosulphate and Hydrochloric Acid/5(4).
Chemistry Plan I am going to produce a piece of coursework investigating the rate of reaction, selecting a variable to see how this affects the rate. The rate of reaction is the rate of loss of a reactant or the rate of formation of a product.
The rate is measured by dividing one by the time the reaction took to take place. Sodium Thiosulphate CourseworkThe Coursework on Concentration Of Acid Reaction Magnesium Rate.
5 cm of HCl (at concentration 1 mol. /dm3) and 15 cm of sodium thiosulphate (at varying concentrations 10 to 35 g/dm3) are poured out into two measuring cylinders.
sodium thiosulphate + hydrochloric acid sodium chloride + water + sulphur dioxide + sulphur The sulphur produced makes the reaction mixture go cloudy. The faster the reaction, the faster the reaction mixture goes cloudy. You will investigate the effect of changing the concentration of sodium thiosulphate on the rate of reaction.
Vitamin C Chemistry Coursework. Uploaded by SiwelEitak. Related Interests. Chemical Reactions; Activation Energy; Redox; Iodine; producing iodine. The iodine that is produced is then titrated against sodium thiosulphate, to find how much iodine was produced by the reaction of the oxidising agent with potassium iodide.
In conclusion 5/5(5). Sodium thiosulphate is a colourless, crystal like compound and is used for dyes and is also a salt. Hydrochloric acid is colourless, poisonous and highly acidic. It is often used as a chemical intermediate and in petroleum production, food processing, pickling, and .Download