Remember me on this computer. I did, however find some outliers in my results. My conclusion is justifiable because I have backed it up with points from my data and I have proved all the points that I made. This causes a quicker reaction. I could test this by asking one of my peers to follow the instructions and then asking for their feedback. This is because when there are more molecules in the solution, there are more molecules to collide so this will speed up the reaction, and therefore it is more likely they will collide with each other.
The points in the top right are quite far down so this shows a negative correlation. I could have use a colorimeter to identify colour changes in the products. When the solution is made more concentrated, there are a greater number of molecules in the same space. Conclusion In my investigation, my data and my graphs proved that my hypothesis was correct. The rate of reaction is the speed of a reaction.
I could have use a colorimeter to identify colour changes in the products.
(DOC) GCSE CHEMISTRY RATES OF REACTION COURSEWORK | Anjelina Qureshi –
I think that my method for my investigation is easy to follow. Background Research Chemical reactions are to do with changing the materials that form the base of sidium experiment.
I have highlighted the 2M results on my tables because it seems as though there is a problem with that set.
aci I have calculated the gradient of my line to support my hypothesis and found that: Sodium Thiosulphate in Hydrochloric Acid. My Error bar graph shows a negative correlation. This can help me identify any faults. I will be timing and watching: For every one M increase, the rate for reaction increases by 2.
I did not swirl these together because I wanted to see the rate of reaction without any intervention. The rate of reaction is the speed of a reaction. I then drew up graphs for my results Data Concentration Test Test 2 Test 3 M 1 s s s 1 2 3 4 5 Table 1: Use of rate of reaction in industry The chemical industry makes medicine and many other substances such as; Limestone – this is used for building Sulphuric acid — used to make other substances Ammonia – used to make fertilisers.
This energy gives the reactant particles enough energy to collide with enough force to break apart the bonds so that new products can be made from atoms. I stood up to allow more space for others hydrochlodic walk by between the rooms. I did have some outliers in my results; however I think that the experiment went fairly well overall. I could test this by asking one of my peers to follow the instructions and then asking for their feedback. There are a few mild outliers.
Rates of reaction of Sodium Thiosulphate with Hydrochloric Acid
This is because there will be more acid molecules in the same amount of solution, therefore more effective collisions with the sodium thiosulphate, and the rate will be higher. Click here to sign up.
This could have happened zcid of human error, wrong calculations or simply not enough activation energy on that particular concentration. Reactions that occur slowly have a low rate of reaction. On my ROR graph, there is a positive correlation. The conical flask and all other equipment must be clean as any impurities may contaminate my experiment.
This causes a quicker reaction. In my scatter graph with line of best coursewkrk, most of the points are close to the line. Graphs All of the graphs that I drew for this investigation show a negative correlation. When the solution is made more concentrated, there are a greater number of molecules in the same space.
Sodium thiosulphate is a colourless, crystal like compound and is used for dyes and is also a salt. I tied my hair back, tucked in my tie and pushed all stools and bags under the desk where there is no risk of anyone tripping. This could have happened because of calculation errors, human errors, recording errors or a fault with the equipment that we used.
In my investigation, there was the limitation of room temperature. The timer was stopped when in see the black cross through the cloudy solution could no longer. I am investigating the different factors courseowrk may speed up chemical reactions. Reactions that happen quickly have a high rate of reaction. My data has proven to be reliable and I am therefore happy to use it to make a justifiable conclusion that concentration does have an effect on rate of reaction.