This means more of the particles collide and more of the collisions result in a reaction, so the rate of reaction increases. In addition to this, more particles have activation energy.
The independent variables will be the initial volume and concentration of sodium thiosulphate, and the initial volume and concentration of hydrochloric acid.
However the overall order for the reaction cannot be calculated using the stoichiometry in the overall equation. To control the temperature I could use a large water bath which could control the temperature throughout the reaction.
Also from my table of results for changing the concentration of HCl, where all the rates must be the same for difference concentrations, there is a anomaly with the 2. This is because as the temperature increases, the reactant particles move more quickly.
As well as environmental variations in temperature the reaction was exothermic and heat is produced. I could also change the initial volume of either the hydrochloric acid or sodium thiosulphate solution and see if I get a similar pattern of results.
I will then put 40cm3 of sodium thiosulphate into a conical flask and place it on a tripod and gauze. I did not have any problem whilst carrying out my investigation apart and do not believe I could have done it any better without specialist equipment with plenty of time.
As the temperature increases, the time taken for the sodium thiosulphate solution to become cloudy decreases. This involves human judgement rather than a qualitative value that can be used to calculated the rate.
There is a time error in the time taken when the cross disappears and the delay in stopping the time.
My results do support the first part of my prediction. I will also try to make my timing and the heating of the sodium thiosulphate solution as accurate as possible. I will keep everything constant apart from the variable I am changing-temperature. For example if 2 molecules must collide to for one product the reaction will be 2nd order.
When using the graduated there was an error of 0. The quality of my evidence is good. The reason why the actual rate constant, k, can be calculated is because in the experiments the change in concentration cannot be calculated.
Instead of using the cross method I would use a light intensity machine that could measure the change in colour over a period of time and stop and start timing when it had reach a certain value.
I am going to draw a graph analyse by results properly.Sodium Thiosulphate + Hydrochloric acid, Water + Sodium chloride + Sulphur dioxide Because the solution turns cloudy we observe the rate of reaction by putting a black cross under the flask and watch and time the reaction until the cross disappears.
sodium thiosulphate + hydrochloric acid sodium chloride + water + sulphur dioxide + sulphur Na 2 S 2 O 3 (aq) + 2HCl(aq) 2NaCl(aq) + H 2 O(l) + SO 2 (g) + S(s) Your teacher will demonstrate a simple way to measure the rate of this reaction.
- Rate of Reaction of Dilute Hydrochloric Acid and Sodium Thiosulphate To investigate the change in rate of reaction between DILUTE HYDROCHLORIC ACID and SODIUM THIOSULPHATE as the concentration varies. PLAN A chemical reaction takes place over a specific period of time i.e.
which is the time for the reactants to be formed into the. Rates of Reaction Coursework Aim: To find out how different concentrations of sodium thiosulphate (Na S2 O3) affects the speed of its reaction with Hydrochloric acid (HCL).
In this experiment I will be seeing how the concentration of Sodium Thiosulphate, Na2S2O3, and Hydrochloric Acid, HCl, affects the rate of the reaction. In this reaction the solution turns milky yellow as sulphate is displaced and forms a solid precipitate.
Chemistry Rates of Reaction Coursework: Sodium Thiosulphate and Hydrochloric Acid Essay Add hydrochloric acid and sodium thiosulphate, and record the amount of time taken for the cross to disappear through the solution from the top of the flask.Download