• Join over 1.2 million students every month
  • Accelerate your learning by 29%
  • Unlimited access from just £6.99 per month

An investigation to find out the factors affecting the rate of reaction of Hydrochloric acid with Sodium Thiosulphate.

Extracts from this document...


An investigation to find out the factors affecting the rate of reaction of Hydrochloric acid with Sodium Thiosulphate. Aim: I am going to discover how the concentration influences the rate of reaction of Hydrochloric acid and Sodium Thiosulphate. There are four factors that influences the rates of reaction, they are: > Concentration(for gases it is pressure) > Temperature > Surface Area(Size of particles) The rate of reaction is owed to the collision theory. For a reaction to take place, particles must collide with great strength. If they do not collide with great strength, the reaction will not take place. Consequently, the rate of reaction is dependant on the collision of the particles. Method: 1. Set up the apparatus. 2. On a piece of paper, draw a dark cross. 3. Put 25ml of Sodium Thiosulphate. This is known as 1 Mole. 4. Place the beaker on top of the piece of paper, with the cross marked on it. 5. Check the temperature using a thermometer. 6. Add the Hydrochloric Acid to the Sodium Thiosulphate. As soon as the Hydrochloric acid touches the Sodium Thiosulphate start the time, using the stopwatch to see how long it takes until the cross is no longer visible. 7. Repeat this, however this time use 25ml of Sodium Thiosulphate and 5ml of water. 8. Keep repeating this; however change the concentration to 0.6M, 0.4M and 0.5M. ...read more.


Below is a picture of a beaker. The experiment shall be carried out three times. There is a reason for carrying out the experiment three times; this is to enable us to gain results that are more reliable. With these results, I can then take the average and show this on my graph. This will also help me to draw a better conclusion. As soon as I have my results, I shall work out the rate of reaction. I shall do this by using a formula: Rate= 1 Time taken for the cross to disappear For each result, the rate shall be calculated. This will help me to find out whether they match my prediction. I feel that as the concentration increases, the rate shall also increase. I must also make sure that the temperature is consistent throughout the experiment. Temperature is a vital factor as it can affect the rate of reaction. I must make sure that each time I carry the experiment out the temperature is the same. It is known that when temperature rises the particles gain energy, this is kinetic energy. This makes the particles move faster. This raises the possibility of particle collisions. Results Concentration of Sodium Thiosulphate(M) Time for cross to disappear(m & s) 1 2 3 Average (m & s) 0.2 1.56 2.0 1.58 1.71 0.4 1.04 1.06 1.06 1.05 0.6 3.9 42.63 44.84 30.46 0.8 30.26 28 31.76 30 1 21.33 19 23.46 21.26 Rate of reaction Concentration of Sodium Thiosulphate(M) ...read more.


For example, the measurements on the beaker may have been inaccurate, or the measurements on the thermometer may have been inaccurate. However, I could not help it if the readings were inaccurate. Looking at my results, it seems as if there was not an error. Things could be changed to make my results different. The cross underneath the beaker could have been darker. This would have made the time for the cross to disappear longer. I would have kept the cross the same for each experiment as it would need to be a fair test. The person who had the best vision could have carried out the experiment, as they would be able to judge when the cross disappeared more accurately. There are always ways in which to improve an experiment. I could have taken readings for 0.1M, 0.3M, 0.5M, 0.7M and 0.9M as well as 0.2M, 0.4M, 0.6M 0.8M and 1M. This would have given me better results as well as a better graph. To make my results even better I could have gone past 1M and gone up to 3M. To make sure the temperature was the same I could have used an electronic thermometer instead of a manual one. I could also have used a water bath. I could the have placed a white ceramic tile at the bottom with a cross on there to see when it disappeared. Overall, the experiment went very well and this is reflected by my results made and by the rate of reaction graph and concentration graph. ...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

See related essaysSee related essays

Related GCSE Patterns of Behaviour essays

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

    This explains why the temperature increased during the reactions. Using the collision theory I have come to the conclusion that for a reaction to take place two reactant particles must collide with sufficient energy. In order to do this they must overcome an energy barrier called activation energy, which is

  2. Factors Affecting the Rate of Reaction between Hydrochloric Acid and Sodium Thiosulphate.

    - increasing the temperature of particles increases their amount of energy. This means they move around more and have an increased chance of colliding together and reacting. Also, by increasing the amount of energy the reactants have you increase the chance that the certain activation energy point has been reached.

  1. The reaction between Sodium Thiosulphate and Hydrochloric Acid.

    I would try to determine the effect of changing the temperature and the effect of changing the concentration of sodium thiosulphate on the rate of reaction between hydrochloric acid and sodium thiosulphate. Again, I would time how long it took for the reaction to complete by using light gates with a sensor attached to a computer.

  2. Investigating Factors Affecting the Rate of a Chemical Reaction

    I wore goggles at all times to protect my eyes. I used a heatproof mat and tripod when using the Bunsen burner and took extreme caution when turning it on and off. I took the same extreme caution when I repeated the results.

  1. An Investigation into the factors affecting the rate of reaction between magnesium and hydrochloric ...

    This could have been because some of the magnesium had corroded forming a magnesium oxide layer which would have affected the rate of reaction. Other factor which could have given me unreliable results could have been that the gas syringes were wet causing them to jam and so not giving

  2. Factors Affecting Enzyme Activity

    Time (s): 0.0 5.0 10.0 15.0 20.0 25.0 30.0 35.0 Amount of gas given off using 1cm3 of liver suspension and 1cm3 of hydrogen peroxide (cm3) 0.0 Amount of gas given off using 2cm3 of liver suspension and 3cm3 of hydrogen peroxide(cm3)

  1. 'Carry out an investigation to determine a factor affecting the rate of digestion of ...

    2, this means that for every ten degree rise in temperature the rate of reaction will double. For example if the rate of reaction is X at 30o then at 40o it will be 2X. This is my prediction, I have predicted this because when the temperature rises the molecules

  2. An Investigation of factors affecting rate of reaction between an acid and a metal.

    This is because doubling the temperature will double the speed of the acid particles and so double the number of collisions. At higher temperatures, more particles will carry the activation energy. This too means that the reaction will be faster because there will be more successful collisions.

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