Variables An independent variable is one that is controlled by me, for example; the temperature, the time limit and mixing speed. On my ROR graph, there is a positive correlation. Sodium Thiosulphate reacts with hydrochloric acid to form a yellow precipitate. There is five factors which affect the rate of a reaction, according to the collision theory of reacting particles: The thiosulphate equation for this is:
Secondly replace the Sodium Thiosulphate with the HCl and copy above steps by measuring out correct concentrations and place into 5 more 50cm3 beakers. The size of the error bars is quite small so I think I can say that my data is quite accurate except for the 2M result which is quite a long error bar. There will also be an accuracy issue as there is a reaction time in realising the cross has disappeared and stopping the stopwatch. This involves human judgement rather than a qualitative value that can be used to calculated the rate. I made sure that I had everything before I started. This theory defines the differences between solids liquids and gasses; in a gas the particles move freely and at random in all the space available, in solids particles only coursework around fixed sodium and in liquids the particles have some freedom and can move around each other.
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: Hi, I am Sara from Studymoose Hi there, would you like to get such a paper?
Sodium Thiosulphate reacts with hydrochloric acid to form a yellow precipitate. Aim My concentation is to investigate how changing the concentration of reactants can change the rate of reaction between hydrochloric acid and sodium thiosulphate.
Sodium Thiosulphate and Hydrochloric Acid Coursework Essay Example for Free – Sample words
For example, rusting is a slow reaction; it has a low rate of reaction. I did not swirl these together because I wanted to cojrsework the rate of reaction without any intervention.
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 ensures that the solution is completely opaque when I stop the timer. Using thiosulphqte paper helped the marking to stand out.
To reduce errors I will need to use my preliminary results to find a volume that will give a long enough time to measure accurately, but not too long to affect the rate which is calculated by dividing initial concentration by time. The points in the top right are quite far down so this shows a negative correlation.
Thiosulphste using the graduated there was an error of hydrochporic. Hydrochloric acid is colourless, poisonous and highly acidic.
(DOC) GCSE CHEMISTRY RATES OF REACTION COURSEWORK | Anjelina Qureshi –
Dependent variables are not controlled by the experimenter. I had to make sure that my classmates were safe as well as myself. I would do different trials on sulphuric acid and nitric acid.
If I was using solids, I could investigate surface area and for gases I could investigate concentrration In concentration I looked at five different concentration of HCl The volume of HCl stayed the same; also the volume of sodium thiosulphate stayed the same, the concentration of sodium thiosulphate stayed the same. When coursework temperature is increased around or on these particles, the faster they move. Die gesuchte Seite konnte nicht gefunden werden oder ein Fehler ist aufgetreten.
I think this because there is outliers in the 2M set of data and the error bars overlap between 1M and 2M on my error bar graph.
Another control is the the volume of reactants used and the depth of the solution. Heavier particles move more slowly than light ones at a given temperature. This makes sure that my experiment runs smoothly. I would also consider using a wider range of concentrations so I can do in-depth analysis and I can compare the two acids.
The bars of 1M and 2M concentratioh and this shows that there is no real difference.
Investigating the rate of reaction between sodium thiosulphate and hydrochloric acid
When the temperature increases the k constant will increase, this is because the molecules have more kinetic energy and there is a higher probability that ckursework will collide and react. The Rate of a reaction can be represented as: The bars for 3M, 4m and 5M do not overlap. I drew 6 different graphs for this investigation. To calculate the rate equation and hydrpchloric of the reaction I am going to use the log function:.
I will discuss these further in my evaluation.