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Sodium thiosulphate is a colourless liquid that reacts with hydrochloric acid as follows:

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Introduction

Sodium thiosulphate is a colourless liquid that reacts with hydrochloric acid as follows: Sodium thiosulphate + Hydrochloric acid ( Sulphur + Sulphur dioxide + Sodium chloride The Sulphur produced is a yellow powder. We want to in investigate factors that increase the rate of this reaction. Background information-Explaining rates A closer look at a reaction: Iron + Hydrochloric acid ( Iron chloride + Hydrogen Fe + 2HCl ( feCl2 + H2 In order for the iron and hydrochloric acid particles to react together: 1. They must collide with each other. 2. The collision must have enough energy. The particles in the liquid If the collision has enough If the collision move around continually. energy, reactions take does not have Here an acid particle is place. Iron chloride and enough energy, about to collide with an iron hydrogen are formed. no reaction atom. occurs. The acid particle bounces away again. The rate of the reaction depends on how many successful collisions there are in a given unit of time. How do you measure rate of this reaction? The rate can be followed like this: 1. A cross is marked on a piece of paper. 2. A beaker containing a volume of Sodium thiosulphate is placed on top of the paper. 3. Hydrochloric acid is added quickly, and a stopwatch is started at the same time. ...read more.

Middle

Start 1. Set up equipment. 2. Measure enough Hydrochloric acid, water and Sodium thiosulphate into 3 beakers. 3. Mark a cross on a piece of filter paper, place under conical flask. 4. Measure 50cm of Sodium thiosulphate into the conical flask. Measure 20cm of hydrochloric acid, and no water. Add hydrochloric acid to conical flask. Start stop watch immediately. Stop the stopwatch when cross disappears. Record time in table. Repeat once more for accuracy. Record in table. Get rid of mixture safety. 5. Measure 40cm of Sodium thiosulphate into the conical flask. Measure 20cm of hydrochloric acid, and 10cm water. Add water and hydrochloric acid to conical flask. Start stop watch immediately. Stop the stopwatch when cross disappears. Record time in table. Repeat once more for accuracy. Record in table. Get rid of mixture safety. 6. Measure 30cm of Sodium thiosulphate into the conical flask. Measure 20cm of hydrochloric acid, and 20cm water. Add water and hydrochloric acid to conical flask. Start stop watch immediately. Stop the stopwatch when cross disappears. Record time in table. Repeat once more for accuracy. Record in table. Get rid of mixture safety. 7. Measure 20cm of Sodium thiosulphate into the conical flask. Measure 20cm of hydrochloric acid, and 30cmwater. Add hydrochloric acid to conical flask. Start stop watch immediately. ...read more.

Conclusion

10 40 20 20 2min 47 sec 2 min 40 sec 2 min 43.5 sec 0.006116207 (0.006) Conclusion and Interruption The reaction went faster, as the concentration of sodium thiosulphate is increased. This is shown in table 2, where the reaction went faster as the volume of sodium thiosulphate was increased. This is also shown in both graphs. There seams to be no strange results. But if there was it could be for a number of reasons including: 1. Solution came from different flasks. 2. Measurements were not accurate. 3. Conical flask was not cleaned after each test. Improvements. 1. Use solution from same flask. 2. Clean conical flask after each use. 3. Repeat experiment for accurate results. 4. Made better control of temperature. Evaluation As my prediction was right, this is what happened in my experiment. My graphs also show that my prediction was correct. In the experiment the diluted Here the acid is more concentrated. acid had not so many particles, there was more acid particles in it as I said there is not much chance therefore there was a greater of an acid particle hitting an iron chance of a successful collision. atom AS TIME WENT ON......... At the start there were plenty After a time, there are of iron atoms and acid particles, fewer iron atoms, and the but they got used up during acid is less concentrated, successful collisions so the reaction slowed down ...read more.

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