• 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
  8. 8
    8
  9. 9
    9

How does temperature affect the rate of reaction between either; a) 250 cm ³of sodium thiosulphate solution and 50 cm ³ of hydrochloric acid, or b) 20 cm of magnesium ribbon and 250 cm ³of hydrochloric acid?

Extracts from this document...

Introduction

How does temperature affect the rate of reaction between either; a) 250 cm � of sodium thiosulphate solution and 50 cm � of hydrochloric acid, or b) 20 cm of magnesium ribbon and 250 cm � of hydrochloric acid? Background knowledge. There are many factors, which can affect the rate of reaction; these include the effect of temperature, concentration, surface area, pressure of gases and the effect of a catalyst. Temperature: In a cold reaction the particles move slowly so they don't collide with each other as much. When they do collide the collisions will be less successful as they have less energy. If the reactants are heated they will have more energy, the particles will move faster and collide more so more collisions will be successful. LOW TEMPERATURE. HIGH TEMPERATURE. Concentration: If the reactants are in low concentration the particles are spread out and will collide less often and less successfully. When the reactants are in high concentration the particles are close together and will collide more often and so more are successful. Surface area: Large particles have a smaller surface area in relation to their volume, less particles are exposed and available for collisions. This means there will be less collisions and a slower reaction. Small particles however have a larger surface area in relation to their volume- more particles are exposed and available for collisions, this means there are more particles colliding with one another and so a faster rate of reaction. ...read more.

Middle

Apparatus: 250 cm � Na2S2O3, 50 cm � HCl, beaker, thermometer, paper, measuring cylinder, stopwatch, tongs, gauze, tripod, Bunsen burner, safety goggles, stirring rod, bench mat. Method. 1) Collect your equipment (as shown above) and set it up as shown in the diagram. 2) Use 30 cm � of Na2S2O3 and place the beaker on top of the paper with the 'X' marked on it. Add the 5 cm � of HCl and time how long it takes for the 'X' to disappear. Record the time and the accurate temperature. 3) Heat 30 cm � of Na2S2O3 until it reaches your next target temperature (approx.) then place the beaker on the paper and add another 5 cm � of HCl. 4) Time how long it takes for the 'X' to disappear, remember to take the accurate temperature and record your results. 5) Keep repeating this until you get a full set of results, making sure you keep the volume of acid and thio the same. My results. Conclusion. Target temp. (� C) Actual temp. (� C) Time taken (secs) 20 26 21.44 30 35 12 35 37 10.47 40 40 9.40 45 46 7.32 50 52 5.78 60 60 3.69 My results show me that as the temperature increases, the rate of reaction increases too. ...read more.

Conclusion

If the beaker wasn't rinsed out thoroughly enough this may have caused contamination and lead to a mistake in my results. As I was using a measuring cylinder with a capacity of 25 ml and I needed 30 ml of sodium thiosulphate - I had to measure it out twice and this could easily have made my point slightly of the graph. I think my method was a good but I could improve it by making the instructions slightly clearer although I found it easy to follow. If I were to do the experiment again I would improve it by taking more results to ensure it was accurate, I would do the experiment twice and then find my average results which would make the experiment better. I would also use a larger measuring cylinder to avoid mistakes whilst measuring out the substances. I think my experiment was good enough to give the conclusion that temperature affects the rate of reaction between Sodium Thiosulphate and Hydrochloric Acid. This is because my experiment was as fair as possible and I didn't make many errors. There are other experiments, which could be done to support my conclusions and to extend the investigation. The temperature, concentration, surface area, pressure of gases and the effect of a catalyst are all other factors which affect the rate of reaction so I could base another experiment on one of these to obtain more evidence and make the investigation more accurate. ...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. How does temperature affect the rate of reaction between sodium thiosulphate and hydrochloric acid?

    * I then placed a thermometer in each test tube and heated it up to the required temperature * I will draw a black cross, with the marker pen, onto the piece of paper. * I will measure out 5cm3 of hydrochloric acid, using a measuring cylinder, while the water and Sodiumthiosulphate is being heated.

  2. The effect of temperature on the rate of reaction between magnesium ribbon and hydrochloric ...

    of the acid so that the acid will fully be cooled or heated. 6. When the temperature of the acid reaches the proposed temperature, put the magnesium ribbon into the acid. Start timing using a stopwatch and record the starting temperature.

  1. Investigating the rate of reaction between Magnesium Ribbon and Hydrochloric Acid.

    Then the other end of the delivery tube will be placed into the bowl of water and under the 100cm3 Measuring Cylinder, so that any gas given off in the reaction displaces the water in it, so that I can see how much gas is given off.

  2. How does temperature affect the rate of reaction between Magnesium and Hydrochloric acid.

    We will record our results in a table, and from this, we will be able to work out the rate of reaction for each temperature. Prediction: I predict that as the temperature increases so will the rate of the reaction.

  1. Investigating the effect of temperature on the rate of reaction between Sodium Thiosulphate and ...

    For the time period that I had in which to conduct my experiment I felt that the range was suitable, but that more temperatures in between could improve the evidence and its solidarity. It would also help to single out anomalous results with more ease.

  2. Finding the effect of concentration on the rate of reaction of magnesium ribbon with ...

    The increased chance of higher energy collisions greatly increases the speed of the reaction. Activation Energy simple definition "Amount of energy that must be absorbed by reactants in their ground states to reach the transition state so that a reaction can occur."

  1. How does temperature affect the rate of reaction between Hydrochloric acid and sodium thiosulphate ...

    The graph made also supports this reasoning with a line of best fit showing strong negative correlation and the pattern that with a higher temperature the rate of reaction is faster. There is also a definite pattern demonstrated on the graph that as the temperature gets lower the points become

  2. Rate of reaction between magnesium ribbon and hydrochloric acid.

    In my investigation I will be using between 1M and 2M, in the higher concentration acid there are more particles per ml, therefore more reactant particles and more chance of a reaction-taking place. In more dilute acid, there are not as many acid particles, which means there is less chance of the acid particles colliding and reacting with magnesium.

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