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# Aim: To investigate how the concentration of sodium thiosulphate affects the rate of reaction.

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Introduction

By Alexander Claire 11A Investigate the effect of concentration on the rate of a chemical reaction Aim: To investigate how the concentration of sodium thiosulphate affects the rate of reaction. Worded equation for reaction: sodium thiosulphate + hydrochloric acid. Symbol equation for reaction: This is the symbol equation for sodium thiosulphate + hydrochloric acid ---> 2HCL+Na2S03. In the reaction the solution will go cloudy because sulphur is given off. We also tested out to see weather the concentration affects the rate, this makes the solution turns cloudy. Apparatus * Thermometer * Beaker * Burette * Paper with X on it * Timer * Flask * Measuring cylinder How the reaction will be monitored: There are four ways in which you can monitor the methods: 1. Collecting and measuring a gas product - record the volume at regular intervals, such as every 30 or 60 seconds. 2. Measuring the loss of mass as a gas forms - record the mass at regular intervals such as every 30 to 60 seconds. ...read more.

Middle

When the reaction has finished, you would have exactly the same mass of catalyst as you had at the beginning. http://www.chemguide.co.uk/physical/basicrates/catalyst.html The effects of surface area The more finely divided the solid is, the faster the reaction happens. A powdered solid will normally produce a faster reaction than if the same mass is present as a single lump. The powdered solid has a greater surface area than the single lump. http://www.chemguide.co.uk/physical/basicrates/surfacearea.html Methods: Step 1: First my group and I measured out 50.0 CM2 of sodium thiosulphate into a burette, we didn't need any water for this, so none was measured out. From the burette I poured the sodium thiosulphate into a flask. We placed the flask on top of a piece of paper with an x on it. We put a thermometer in the flask to measure the temperature. The stop watch was then started to time how long it took for the x to disappear, then we repeated it four more times. ...read more.

Conclusion

3.1 10 40.0 5.0 56 60 50 55.3 1.8 The results I got were made from me and my classmates by doing the experiment and recording the results. I got the rate by doing, 1 divided by the average time, times by one hundred. Make the answer to one decimal pace. I got the average by adding the times up and diving them by how many times there are (3). Equipment - Accuracy - 50cm3 measuring cylinder 2cm3 10cm3 measuring cylinder 1cm3 Burette 0.05cm3 250m3 measuring cylinder 2cm3 % Error=Accuracy of equipment x 100 Quantity of substance -We needed a burette to measure all three chemicals. The degree of accuracy of the burette is very high of 0.05. Conclusion: From my graphs I can say that there is a correlation, between the rates of the reaction and concentration of the sodium thiosulphate. I can say this because my graphs and my data support it; also my line on my graphs, gets steeper as the concentration of the sodium thiosulphate increases. My data is shown in my results table. ...read more.

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1. ## To investigate a factor that affects the rate of reaction and why?

Observe the contents of the conical flask, it should begin to turn a milky colour. 8. Stop timing when the cross can no longer be seen due to the sodium precipitate. 9. Repeat. 10. Repeat again. *Follow these instructions for each different molarity of hydrochloric acid; 0.2M, 0.5M, 1M,

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