In my experiment I am going to find out how increasing the temperature of the hydrochloric acid and sodium Thiosulphate solutions affects the rate of reaction when they are mixed together, I am doing this as I want to see if the temperature has a large or small effect, and why this is.
Hydrochloric acid + Sodium Thiosulphate –>Sodium Chloride + Sulphur dioxide + Sulphur + Water
2HCl (aq) + Na2S2O3 (aq) –> 2NaCl (aq) + SO2 (g) + S (s) + H2O (l)
Preliminary
I did a preliminary of my experiment to check it would work and to make sure my hypothesis can be tested fairly and accurately.
For the preliminary, I decided to measure the amount of gas produced in two minutes as a product of the reaction dependant on the temperature. To keep the test fair the changes in the temperature were spread out equally and the only independent variable I used was the change in temperature, the only dependant variable was the amount of gas produced in a controlled amount of time (2min).
I kept all other variables; volume, time solutions were left to react, amount of time solutions were left to be heated, concentration, amounts of solutions, amount of times solution was mixed during reaction, amount of chemical used and amount of water in water bath, were all controlled. If I didn’t do this it wouldn’t be a fair test, for example, if I also had dilution as an independent variable in the experiment, the results wouldn’t show both the affects of temperature and dilution, which would make the results inaccurate.
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The method:
1. I filled a tray with water and set up the conical flask with a cork attached to a delivery tube on the top. This is used to keep the gas inside the flask, to travel through the tube to a measuring cylinder I will attach later to measure the gas produced.
2. I used measuring cylinders to measure 50cm³of sodium Thiosulphate and 10cm³ of hydrochloric acid and set up a Bunsen burner with a beaker filled with water on top; this will act as my water bath to evenly heat the solutions.
3. I put the solutions into separate test tubes and into the beaker, heating over the Bunsen burner to a certain temperature.
4. When the solutions rose to the temperature wanted, I took the solutions off the heat and immediately- so as not to change the temperature- put them both in the conical flask to react, putting the cork on top, so as not to let the gas escape, which would affect my results.
5. I used the tray filled with water to measure the amount of gas produced in 2mins, by filling a measuring cylinder completely with the water and turning it upside down, with the end of the delivery tube held inside it. The measurement of water left in the cylinder at the end of the experiment shows the amount of gas created in the experiment.
6. I used a stop watch to time the amount of gas that was produced in exactly two minutes.
equipment | reason |
conicalflask | to mix solutions in |
Cork attached to a delivery tube | to keep gas for measurement |
Measuring cylinders | to measure solutions accurately |
50cm³ of sodium Thiosulphate | To react in experiment |
10cm³ of hydrochloric acid | To react in experiment |
Beaker filled with water | To heat up solutions in-crude version of a water bath this allowed me to steadily heat my reactants, however a thermostatically controlled water bath would have been a lot more reliable |
boiling tubes | to put solutions in (separately) |
Bunsen burner | to heat up solutions |
Stop watch | to time reaction to 2mins- better than using clock as it uses milliseconds, so very precise, making the results more reliable |
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Tray | to fill with water for measuring amount of gas |
50cm³ measuring cylinder | to measure sodium accurately- should wear protective clothing + goggles to prevent irritation |
10ml³ measuring cylinder | to measure hydrochloric acid should wear protective clothing + goggles to prevent irritation |
tripod | to hold water bath and solutions over flame safely |
heat mat | Bunsen burner set up on top of this, it is inflammable, so Bunsen burner is kept on top of it whilst burning to avoid setting worktop alight |
50cm3 Measuring cylinder | To measure gas-dependant variableTo be more accurate I could have used a measuring cylinder going up in 1cm3 rather than 5cm3 |
Boiling tube holders | To take boiling tubes out of water bath without burning fingers as they would be very hot |
The results were as follows:
temperature ( ˚C) | Amount of gas produced in 2min (cm3) |
20 | 0 |
30 | 0 |
40 | 0 |
50 | 0 |
This data shows that as the temperature rises the amount of gas produced doesn’t change. This would imply that the temperature does not change the rate of reaction; however it also suggests that the two solutions don’t react at all, when I knew this wasn’t the case. I did some research into the products of this reaction, and found that the gas; sulphur dioxide, that is formed during the reaction, dissolves in liquid. This makes it impossible to measure the reaction through the amount of gas produced, so instead I chose to change my variables; although I kept the independent variable the same (temperature), I changed my dependant variable (what I measured) from amount of gas, to time taken for the solutions to completely react, so I could still measure the effect of temperature, but through a more effective way.
To know when the solutions have reacted, I chose to test the amount of time it takes for the solution to become completely translucent, showing the reaction is complete. I did this by using a piece of paper with a black cross on it under the flask, so I stopped the timer as soon as the cross is no longer visible. Also by changing the time to being the dependant variable, temperature my independent variable and the volume, concentration, amounts of solutions, amount of times solution was mixed during reaction, amount of chemical used and amount of water in water bath being controlled. This will be a much more accurate way of carrying out the experiment, as the time on the stopwatch will be clearer and more exact then the measurement of the amount of gas made in a specific time. Other then this all the other controlled variables stays the same to keep a fair test. I tested my improved method with a second preliminary to make sure it worked and there weren’t any other flaws in the process that I chose.
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Method:
1. Measure 50cm³ of sodium Thiosulphate (0.15M) and 5cm³ of hydrochloric acid (2.0M) into two separate measuring cylinders. Pour into two separate boiling tubes.
2. Set up a Bunsen burner with tripod and safety mat, put a beaker with water on the tripod over the burner and put the boiling tubes in it.
3. Heat to certain temperature while placing the 100cm³ conical flack over the paper marked with a cross
4. When the solutions reach the correct temperature, pour in the sodium Thiosulphate, and then the hydrochloric acid ensuring that the stop clock starts timing the reaction immediately.
5. Repeat steps 1-4 changing the temperatures.
Results:
Temperature ( ˚C) | time taken for solution to react (s) |
30 | 32.56 |
40 | 23.71 |
50 | 12.1 |
The data collected by the second preliminary seems accurate as the results are accurately spaced out and as the temperature raises the reaction time decreases. As this method for my experiment has proved effective I will use it for my actual test. When I do the final experiment I will have a larger range of data to see the correlation accurately on a graph. The preliminary helped me decide how large the range between each temperature would be, by showing me that the experiment is very sensitive. Also as I changed the temperature by 10˚C for each test, the ranges between the results are very large, so I decided for my final experiment to raise the temperature by 5˚C for each test and to go up to 55, so I can see the pattern clearer when making my graphs and tables. I will also measure the reaction rate for each temperature more than once, so I know the measurements recorded are accurate, and so I can calculate the mean of the results.
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Final experiment:
Equipment:
equipment name | reason |
50ml³ measuring cylinder | to measure sodium thiosulphate accurately- should wear protective clothing + goggles to prevent irritation |
10ml³ measuring cylinder | to measure hydrochloric acid should wear protective clothing + goggles to prevent irritation |
pipette | to get measurements exact by transfer small amounts of each chemical which would not have been possible by hand |
laminated card with cross | to make test fair-the translucency of solution not guessed but could be clearly monitored, more likely to be same for each experiment laminated, so was not vulnerable to spills |
stop clock | to time reaction- better than using clock as it uses milliseconds, so very precise, making the results more reliable, however cannot always be stopped immediately |
500 beaker | To heat up solutions in-crude version of a water bath this allowed me to steadily heat my reactants, however an electric water bath would have been a lot more reliable as the temperature would be specifically set. |
100cm³ conical flask | to mix solutions in |
stickers | To label beakers + measuring cylinders to avoid confusion of which chemical was in which container, and starting the reaction which would cause an error in results. |
thermometer | To measure exact temperature to keep a fair test. The different thermometers may have different sensitivities due to them being worn out and used so many times which would affect my control variable (the temperature) making my data unreliable. |
boiling tubes | to put solutions in (separately) |
Bunsen burner | to heat up solutions |
tripod | to hold water bath and solutions over flame safely |
test tube holders | to hold heated solutions safely |
matches | To light Bunsen burner, quick and simple, however could only be used once, so I was not able to turn Bunsen off during the reaction time, meaning I had to refill the water bath each time I used it, otherwise it would have already reached the temperature I wanted. |
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Heat mat | Bunsen burner set up on top of this, it is inflammable, so Bunsen burner is kept on top of it whilst burning to avoid setting worktop alight |
Method:
1. Using the measuring cylinders, measure 50cm³ of sodium Thiosulphate (0.15M) and 5cm³ of hydrochloric acid (2.0M) into two separate measuring cylinders, which needs to be exact every time so the results are reliable. Pour into two separate boiling tubes.
2. Set up a Bunsen burner with tripod and safety mat to heat the solutions on. Put a beaker filled halfway with cooler than room temperature (under 25 ˚C) water- so the solutions can be heated accurately- on the tripod over the burner. Carefully place the boiling tubes in it and hold the solutions in using the test tube holders for safety.
3. Heat to the temperature wanted, I measure the temperature through the temperature of the water- of the water bath- rather than the specific solution. Place the 100cm³ conical flasks over the paper marked with a cross.
4. When the solutions reach the correct temperature, pour into the flask, first the sodium Thiosulphate, and then the hydrochloric acid ensuring that the stop clock starts timing the reaction immediately. Swirl mixture once, so the solutions are thoroughly mixed together.
5. Stop timing as soon as the solution becomes translucent so the cross can no longer be seen. Record time.
6. Repeat steps 1-6 changing the temperatures.
Possible factors that might affect the reaction include;
* Temperature- the independent variable that I changed for each test with equal spacing between temperatures e.g. 30, 35, 40, 45, 50
* Total Volume of solutions- controlled by using measuring cylinders to measure the volume and keep it exactly the same throughout the experiment
* Concentration of solutions- controlled by using the same dilution of sodium Thiosulphate (0.15M) and of hydrochloric acid (2.0M) throughout experiment. If they were changed throughout the experiment as well as another independent variable the results would not be reliable. This links to the collision theory, as there are more particles in a smaller amount of space, so they will a lot more collisions in a shorter amount of time.
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* Amount of chemical used- kept the same as if the ratio of chemical substances is changed as well as the temperature during the experiment the results would be flawed. This is because then the reason for the changes in temperature cannot be definitely identified, as there could be more than one cause.
* Same thermometer-to ensure the temperature; as the thermometers varied, there could be slight changes to the results because the reading could be slightly different each time, which could greatly affect the results. This is because, in collision theory, the more energy the particles have the faster they move, resulting in a faster amount of collision in a smaller amount of time. Because the temperature gives the particles more energy; heat energy is transferred into kinetic energy, this causes more collisions between particles.
* Laminated cross card-if the size and colour of cross were different at different points of the experiment it wouldn’t affect the rate of reaction, however the results wouldn’t be accurate as, for example, if the font size was smaller at one point, the cross would be covered by the reaction solution more quickly, then if the font size was bigger. I tried to use the same size cross throughout the experiment; however the choice of cards were limited.
* Amount of water in water bath- if there was very little water the solutions could be heated up unevenly and therefore not accurately at a specific temperature, which would affect the rate of reaction, as some particles will have more energy than others, so some will react quickly, and some will react a lot slower. I kept this controlled, by keeping the amount of water in the water bath at a constant of 250cm³ so it didn’t affect my results.
* The amount of times the mixture is swirled- I only swirled it once each time, and made sure it was only me who did it, so someone doing it differently to me wouldn’t affect the experiment. This variable, if changed throughout the experiment could greatly affect my overall results, as this is a sensitive reaction
* How the temperature of the water in the water bath would be slightly different then the temperature of the solutions, and as I measured the temperature of the water my results could have been affected by this. To keep this controlled I made sure the water in the bath was heated from room temperature to the correct temperature with the solution in the bath so they were heated as accurately as possible in this way. To improve I would measure the exact temperatures of the solutions, however to do that you need two thermometers (to be fair, to be sure they are both at this temperature), and there weren’t enough in the class to go around.
Results:
temperature ( ˚C) | time taken for solution to react (s) |
| 1 | 2 | 3 | mean | range |
30 | 31.31 | 32.37 | 30.47 | 31.38 | (1.9) 30.47-32.37 |
35 | 28.01 | 28.59 | 27.13 | 27.91 | (1.46) 27.13-28.59 |
40 | 22.5 | 23.47 | 24.09 | 23.35 | (1.59) 22.5-24.09 |
45 | 18.41 | 19.06 | 20.04 | 19.17 | (1.63) 18.41-20.04 |
50 | 23.28- outlier | 13.13 | 12.34 | 12.74 | (0.79) 12.34-13.13 |
55 | 10.50 | 11.78 | 11.94 | 11.41 | (1.44) 10.5-11.94 |
The graph and table shows that the temperature increase of 5 ˚C decreases the time taken by approximately 4s- it is inversely proportional. It also shows as the temperature reaches the higher levels tested, the time drops greatly (45 ˚C-50 ˚C)
I have one outlier-temp 50 1st time- in my table, this could have been the result of many things, however I am sure it was due to how the temperature of the solutions was not correct. This was because the thermometer we used didn’t seem to be working very well, as it showed to different temperatures at once. We only used it for that one test, and after, when I saw the result didn’t fit with the rest of the data, I changed it for a different one, so no more of the results would be inaccurate. So this outlier wouldn’t affect my mean/range results, I didn’t include that measurement in calculating the mean or ranges for my graphs.
This data shows that the higher the temperature, the faster the reaction time. The graph I made (attached) using this data clearly shows this direct correlation; as the temperature rises, the time of reaction drops. I added range bars on to each plotting made which shows the data collected to be reliable, as they don’t overlap, showing that there is a real difference. However the range bars for a few temperatures are bigger then I would like, as this could show slight flaws of controlling external variables such as room temperature, which are hard to control. The plotting on the graph is also a bit more scattered then I would like, as this shows the tests were not very accurate; the more scattered, the less accurate the results were, and also the less accurate the line of best fit will be. To aid this I could do more tests and not use any outliers I record, to get a better mean, and range of data. I could also make improvements to the experiment so the same mistakes do not happen again; I would use an electric water bath so the temperature is exact, I would use the same thermometer and laminated cross card for each experiment, I would use a more accurate stop watch that can be stopped more easily. I have noticed that the last two temperatures -50, 55- the time results are a lot shorter, and don’t really fit well with my curve of best fit, they are also considerable similar to each other in terms of time, compared to the others. This could have been due to slight changes in temperature, or another factor which should have been controlled wasn’t controlled as wall. However it still clearly shows that temperature to have a significant impact on the time of reaction.
This is the result of collision theory; which shows that a chemical reaction can only take place when the particles collide together. When the particles collide they react, but there is a minimum amount of energy, or activation energy, that is needed for colliding particles to react with each other. If the colliding particles have less than this minimum energy, they just bounce off each other and no reaction occurs. The more energy they have, the faster the particles are going to move and these particles are more likely to react when they collide. When I raised the temperature of the solutions, the particles gained a lot of energy, making them move faster. So, when the separate solutions were put together, the particles collided together and made the reaction happen. The higher the temperature, the more energy used and therefore, the faster the collisions and reaction will be.
temperature ( ˚C) | rate of reaction (s-¹) |
30 | 0.032 |
35 | 0.036 |
40 | 0.043 |
45 | 0.052 |
50 | 0.078 |
55 | 0.088 |
The graph and table show every 5 ˚C rise in temperature, the rate of reaction rises by 11.2 s-¹. It also shows as the temperature reaches higher levels, the rate rises greatly.
I calculated the rate of reaction from my mean results of the experiment. This shows a correlation in the rise in temperature and an increase in the rate of reaction, because you can see that in both columns the numbers are getting bigger as they go down the table (gaining temperature).
I also made a graph (attached) so this correlation could be shown clearer in a slightly more detailed way. The data in my graph is quite scattered, as rate of reaction graphs should be very close to the line of best fit- practically resembling a line with the plotting. This means that this data is not totally reliable as the results are varied, this however I only did 3 tests for each temperature, and if I did more tests, I would be able to see clearer if the range was very varied or not. To make it more accurate I could have used a more precise thermometer, so the temperature was always exact. I could have also used the same equipment- thermometer, timer, cross card- in all tests, so any small irregularities would not make a change to the results, as they have been the same across all tests in the experiment.
The ranges could be large because of small variations, such as the difference in temperature of the water bath and solutions- as I took temperature from water. These small variations can have a big impact on such a sensitive test.
Evaluation
Procedures:
There were some practical difficulties I encountered during the experiment, such as getting the temperature exact, as it would rise quite fast. Also timing accurately was also difficult as I had to make sure as soon as I couldn’t see the cross through the reaction that the timer was stopped. As there is a hesitation period between seeing the finished reaction, and stopping the time, sometimes it would be stopped quicker than other times. To make sure this has as little effect on the results as possible, I would have the same person stop and start the clock each time, and have the same person to decide when the reaction is fully opaque, making it less likely for there to be a great difference in the reaction time. This could strongly affect my results as the mean that was calculated for each temperature, would not be accurate if all times included were not exact. This could be the case with the large time difference between the results from the 45˚C and 50˚C temperatures. Also the ranges could have been part of the problem.
Also it was difficult to control all variables as there were some external factors such as the temperature of the room which couldn’t be controlled at all. This could affect the results greatly, as the temperature of the solutions during the reaction could rise or-more likely- will drop due to the room temperature. This will either quicken or slow down the reaction time.
It was also rather difficult to shake the solution only once, as the solution will continue to move after I stopped swirling it, making it hard to control, which could affect the reliability of the data. To improve the experiment I would use a thermostatic water bath to heat my solutions, as this will be a lot more precise, giving me more accurate results. I wouldn’t shake the reaction at all, as the differences in movement each time I shake the solution could greatly affect my results. However if I chose to stir the mixture -as it would make sure the solutions are thoroughly mixed- I could use a magnetic stirrer to make sure the solutions are evenly mixed, and will be mixed the same amount for each test, keeping the variable controlled to make my experiment results accurate. I could use a data logger to record the temperature of my solutions which would make my results more accurate, as the temperature would be exact, rather than rounded to the nearest ˚C. I could also use a light sensor which would also make my results more accurate by telling me exactly when the reaction turned cloudy-translucent-showing that the reaction was complete.
Reliability of evidence:
My data was quite consistent across all the temperatures; however for individual ranges- showing closeness of repeat measurements- the temperature is varied slightly. To improve on this I would make more tests for the same temperatures, to make the data more reliable, as some of my results are varied by 2˚C, by adding more tests to get a more accurate mean would be mainly to adjust the rate of reaction, so the line of best fit is more accurate. This means that there will not be as many issues with slight differences in equipment, as the variations will not be as big if I have more similar results from doing it a lot more.
There is a small amount of scatter on my time/temperature graph so makes the results seem precise. However my rate of reaction/temperature graph shows a larger scatter, so there are some faults in my results. To show a more direct correlation, I would need to make sure that all of each set of temperatures I tested (e.g. attempt 1: 30, 35,40,45,50) were all tested with the same equipment, and around the same time (so room temp will be the same).
Doing this would ensure my results to be a lot more reliable.
I did record one outlier during the experiment. It was very different to my other results and could have been caused by problems in controlling temperature, or amount of times the solution was swirled. However could have been effected by a tiny change in one of the controlled variables, as it is such a sensitive reaction. I left this figure out of mean calculations, ranges and my graphs, so it didn’t affect my overall results.
Summary:
I feel that my conclusion is quite strong as my results are generally accurate, however were not always entirely precise, due to slight changes when carrying out each experiment, therefore making my conclusion not completely secure. Also the fact my ranges were sometimes varied, shows there to be areas of weakness in my method, or how I handled the controlling of variables. It would be easier to see specific flaws if I did more repeat experiments with the same temperatures to ensure accuracy. Also having more time so I could do all of the experiments- or all of 1st attempt, 2nd attempt or 3rd attempt- at once, to ensure no external variables are being changed; as if I take the same temperature on different days and get different results I will know that changes in difficult to control factors are the cause of the changes.