• Join over 1.2 million students every month
• Accelerate your learning by 29%
• Unlimited access from just £6.99 per month
Page
1. 1
1
2. 2
2
3. 3
3
4. 4
4
5. 5
5
6. 6
6
7. 7
7

# Investigate the rate of the reaction between aqueous sodium thiosulphate and dilute hydrochloric acid.

Extracts from this document...

Introduction

My aim in this coursework is to investigate the ratee of the reaction between aqueous sodium thiosulphate and dilute hydrochloric acid. The ionic equation for the reaction betweem aqeous sodium thiosulphate and dilute hydrochloric acid is : 2h+ (aq) + S2O3 2- So 2 (aq) + H20 (l) + S (s) When a solution of sodium thiosulphate reacts with any acid a precipitate of sulphur forms. The reaction occurs between the hydrogen ions from the acid and the thiosulphate ions in the sodium thiosulphate. Backround information There are many variables, which affect the rate of the reaction between aqueous sodium thiosulphate and hydrochloric acid. These are ; The temperature at which the reaction is taken place at A Catalysy The concentration of the sodium thiosulpate The concentration of the hydrochloric acid The collision theory states that the rate of a rection simply depends on how often and how hard the reacting particles collide with each other. The basic idea is that particles have to collide with each other to react, and they have to collide hard enough as well. When the temperature is increased the particles all move quicker. If they're moving quicker, they're going to have more of a chance of colliding with each other. ...read more.

Middle

I also believe that as I double the concentration the rate would also double. Method Firstly I will draw a cross on a white tile using a marker pen. The using the burette I will measure out of 20 cm3 of hydrochloric acid and pour it in a conical flask. Then I will measure out the concentration of the sodium thiosulphate solution. Then I will pour the solution into the conical flask and as soon as the first drop of sodium thiosulphate drops on the conical flask I shall start the stopwatch. Looking directly above the conical flask I will wait until the cross disappears and then stop the stopwatch. Apparatus Conical flask Hydrochloric acid Sodium Thiosulphate Dilute water 3 Burettes white tile Per,manent marker Stopwatch 2 Beakers Diagram Results concentration of time taken for repeat 1 repeat 2 solution mol/dm3 cross to disappear seconds seconds 1 6.51 6.23 6.43 0.8 8.44 8.97 8.36 0.6 9.76 10.38 9.41 0.5 12.09 12.61 11.98 0.4 14.95 15.54 15.29 0.2 32.23 32.26 33.64 0.1 65.12 62.47 61.32 concentration of average of results solution mol/dm3 in seconds 1 6.39 0.8 8.59 0.6 9.85 0.5 12.23 0.4 15.23 0.2 33.01 0.1 62.97 concentration of Rate of reaction solution mol/dm3 1/time taken (s-1) ...read more.

Conclusion

This ould have made my experiment very reliable and would have made my graph more acurate. It would have made my graph more accurate as there would be more points plotted on it. Another way in which I could have had anomalous results was by stopping the stopwatch early or too late. I could have also meausref the wrong concentration, this would have either increased or decreased the rate of my reaction. I believe a more accurate way in which I could have carried out this experiment was by using the light sensor, which is attackes to the data-logging computer. The way in which it works is that the computer measures the percentage of light, which is picked up by the sensor. The reaction stops when the reading on the computer goes down to 0%. This is a more reliable way in which to carry out the experiment as there is no chance of a human error to be made andd practically no chance of there being a computer error. For my furhter work I could have also done this experiment at a higher temperature. This would have probably increased the rate of the reaction. This is because when the temperature is increased the particles all move quicker. If they're moving quicker, they're going to have more of a chance of a collisions to occur with eachother. ...read more.

The above preview is unformatted text

This student written piece of work is one of many that can be found in our GCSE Patterns of Behaviour section.

## Found what you're looking for?

• Start learning 29% faster today
• 150,000+ documents available
• Just £6.99 a month

Not the one? Search for your essay title...
• Join over 1.2 million students every month
• Accelerate your learning by 29%
• Unlimited access from just £6.99 per month

# Related GCSE Patterns of Behaviour essays

1. ## Experiment to Investigate the Rate of Reaction between Hydrochloric Acid and Sodium Thiosulphate, with ...

Higher Level- Richard Parsons), which effectively accelerates the rate of the reaction and therefore making the experiment unfair. However I will not be able to keep the temperature constant during this experiment, as I have no control over it, although it would more or less be constant as the external conditions were not altered much.

2. ## The aim of this coursework is to investigate the rate of reaction between sodium ...

The more particles there are in the same volume, means that the particles will be closer together. This means that the particles will again collide more frequently with each other and the rate of reaction will increase. A solid in a solution can only react when the particles collide with its surface.

1. ## Experiment to investigate how changing the concentration of hydrochloric acid affects the rate of ...

Effects of Surface Area An increase in surface area means that there is a larger area and therefore larger number of exposed reacting molecules to act. This increase in collisions causes an increase in rate of reaction. This is a factor that can optimize reaction rates.

2. ## Measuring the rate of reaction, when dilute sodium thiosulphate solution and dilute hydrochloric acid ...

* Empty the sodium thiosulphate in the conical flask and then place the conical flask over the piece of paper with the "X" marked on it. The next few steps we had to do fairly quickly. * Add the hydrochloric acid to the conical flask, as soon as the two

1. ## Investigate the concentration of Sodium Thiosulpate and see how it affects the rate of ...

This initial energy is known as the activation energy, as it is needed to break the initial bonds. The affect of temperature on rates of reaction is important. Raising the temperature makes the rate of reaction faster. Because the temperature increases, the pressure of the molecules causing them to move

2. ## Investigating the factors influencing the rate of reaction between Sodium Thiosulphate and Dilute Hydrochloric ...

This means that my mathematical relationship can only be an educated guess or estimation. Apparatus eye observing reaction stop clock conical flask containing reactants in a solution sheet with 'X' on it Method The reaction in the experiment is between Sodium Thiosulpahte solution and Hydrochloric acid.

1. ## Find out how the rate of hydrolysis of an organic halogen compound depends on ...

Two different experiments were carried out - both of different methods. The first involved the primary substances, and the second involved the tertiary substance. During the first experiment, the rates of hydrolysis of 1-chlorobutane, 1-bromobutane, and 1-iodobutane were compared. The equations for the hydrolysis reactions that occurred are as follows: 1-chlorobutane - CH3 ?

2. ## Investigate a factor which affects the rate of reaction in the reaction between sodium ...

Increases of 10� of the temperature will often double the rate of reaction. The complete opposite happens when the temperature is decreased. As the temperature decreases the atoms lose their energy, which means they will move slower, this will decrease the chances of colliding with other atoms.

• Over 160,000 pieces
of student written work
• Annotated by
experienced teachers
• Ideas and feedback to