• 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
  10. 10
    10
  11. 11
    11

rates of reaction

Free essay example:

Rates of reaction coursework

Introduction

The rate of reaction may be measured by following the loss of a reactant, or the formation of a product. The rate of reaction is just how fast it goes. We measure the rate of reaction by measuring the time taken for the reactants to be used up or products to be formed.

A chemical reaction can only occur between particles when they collide. There is a minimum amount of energy which colliding particles need in order to react with each other. The faster the particles are going, the more energy they have and they are more likely to react

Temperature

One of the things that affect rate of reaction is increasing the temperature of a reaction. At higher temperatures reactant particles move faster and collide more often and more violently and more successfully. This means they are more likely to combine this therefore increase rate of reaction.

image00.png

Concentration

Increasing the concentration of reactants also increases the rate of a reaction. This is because there are more particles in the same volume so more collisions are possible every second. If a solution is more concentrated it means there are more particles of the reactant knocking about between the water. The more collisions happen and the greater the rate of reaction.

Surface area

Breaking up solids into smaller pieces increases reaction rate because this increases the total surface area. Increasing the surface area must increase the number of particles of the solid in contact with the other reactant in solution. An increase in surface are must increase the number of particles of the solid in contact with the other reactant in solution so therefore the larger the surface are, the more collisions and the greater the reaction rate.

image01.png

Catalyst

Using a catalyst increases the rate of a reaction. Catalysts are not used up in a reaction. A catalyst is a substance that changes the rate of a chemical reaction without undergoing any permanent chemical change. A catalyst lowers the amount of energy needed so more particles will have the required energy for successful collisions. It is called a positive catalyst if it speeds up the reaction. A negative catalyst slows down the rate of reaction.

image03.png

Pressure

If the pressure is increased the particles in the gas are pushed closer. This increases the concentration and thus the rate of reaction.

Collision theory

When the solutions are reacting the collisions have sufficient activation energy. This is the minimum amount of energy that is required to activate atoms/molecules to undergo a chemical transformation. Increasing the temperature brings more collisions and an increase in rate of reaction.

Preliminary work

I carried out a preliminary test to practice so learnt how to improve on the real test we realized that we needed to do the test 3 times.

In a previous experiment we also carryout an experiment to show how concentration affects rates of reaction this is what my results where

Volume of sodium thiosulphate (cm³)

Volume of water (cm³)

Concentration

(mol/dm³)

Time for cross to disappear (sec)

Rate= 1/time

(sec6¹)

50

0

18.05

40

10

21

30

20

27

20

30

10

40

57.81

This previous experiment helped me to decide to do this experiment better by not wasting time and watching probably when the cross disappears because when we compared are work with other groups are one wasn’t correct and we didn’t get to finish it so I think on the next experiment we should improve on teamwork, observation and time.

Prediction

For my experiment I predict that as the concentration of sodium thiousulphate is reduced it will take longer before the solution turns cloudy. This is because in the first reaction it starts of with only sodium thiosulphate and hydrochloric acid colliding with each other and react forming the cloudy solution. But towards the end of the experiment where there will be a higher concentration of water and less sodium thiosulphate so there will be a longer amount of time before the molecules collide with each other per second to react. So as the concentration is decreased the rate of reaction will be slower, this is because when the concentration is decreased there are less acid particles to collide with the sodium thiosulphate particles. Increasing the concentration of a substance in a solution means that there will be more particles per dm³ of that substance. This is away of measuring the rate of formation of sulphur.

HCl + sodium thiosulfate image04.pngsodium chloride + sulfur dioxide + sulfur + water
HCl(aq)   +  Na2S2O3(aq)image04.png       NaCl(aq)      +    SO2(g)      +      S(s) + H2O(l)

image05.png

The plan

Aim

In the investigation I will carry out an experiment to measure how concentrating sodium thiosulphate affects the rate of reaction. I will also be measuring how fast sulphur forms and turns the solution cloudy. The reaction will be carried out in a flask placed on a piece of white paper which has a black cross on it. At the beginning of the reaction, the cross can be seen easily. As the flask becomes more and more cloudy, the cross gets harder to see. We will measure the time taken from the start of the reaction until the cross can no longer be seen. Decreasing the concentration of sodium thiosulphate means less particles will collide per second and so the rate of reaction decreases

The method

  1. First get a piece of paper with a cross placed on it and put it under the conical flask.
  2. measure out 50(cm³) of sodium thisulphate using measuring cylinders then
  3. pore into a conical flask
  4. measure  30(cm³) of hydrochloric acid using a different measuring cylinder                    
  5. Pure into the conical flask then swirl once to mix the solution.

      6)   Watch and measure the time from the start of reaction until the cross on the              

             Paper can no longer be seen.

      7)   Then we repeat the experiment 3* to make it a fair test.

      8)    Repeat again with different concentrations of sodium thiosulphate

             (40 sodium thiosulphate, 10 water)

             (30 sodium thiosulphate, 20 water)

             (20 sodium thiosulphate, 30 water)

             (10 sodium thiosulphate, 40 water)

In are second investigation we will continue this experiment 5 times but we will decrease the amount of sodium thiosulphate by a tenth each time and we will add 10 (cm³) of water and the volume of water will increase by a tenth.

The equipment list

  • 2 measuring cylinders
  • conical flask
  • stop watch
  • paper with x
  • beakers (x2)
  • 0.15m sodium thiosulphate
  • hydrochloric acid
  • water
  • goggles
  • HP pencil

 Diagram of equipment used

What I changed or kept the same?

I kept the volume of hydrochloric acid the same and I changed the amount of sodium thiosulphate from 50, 40,30,20,10 and I changed the volume of water by 0, 10,20,30,40

I kept the same temperature, surface area-liquids, equipment, cross and concentration of acid.

The fair test

To make my experiment a fair test I will repeat the experiment 3x

I will only change the concentration of sodium thiosulphate, the same amount of hydrochloric acid will be used and the conical flask will be washed out after each experiment with water. I will use a stopwatch because it’s more accurate than using my own judgement to sate when the cross is no longer visible

The safety issues

To carryout this experiment safely I will wear goggles throughout the experiment to protect my eyes from any possible splash from hydrochloric acid because it is corrosive also any splash from sodium thiosulphate because it can be harmful, because these chemicals can be hazardous. While measuring and using the acid I will be cautious and take care, as it is a dangerous chemical, I will also carryout laboratory rules such as no running. I will keep bags coats and any clutter out of way to keep the work surface neat, tidy and uncluttered

The observation

Volume of sodium thiosulphate (cm³)

Volume of water (cm³)

Time for cross to disappear in seconds (sec)

Average

(sec)

Rate

1/time

(sec6¹)

1

2

3

50

0

56

59

109

109

0.67

40

10

61

58

70

156

0.51

30

20

81

66  

68

113

0.65

20

30

118

111

103  

119

0.66

10

40

313  

303  

296  

336

0.20

ANALYSIS

image06.png

I have processed my results on to a line graph because a line graph can show you much more clearly what you want to find out and what I have found it that my experiment went wrong somewhere  when it comes to investigating the volume of 40 of sodium thiosulphate.

this graph obviously means something went wrong because it show that as the concentration of sodium thiosulphate increased the time taken decreases and then around 30 concentration of sodium the time increases then decreases, this is clearly wrong because the graph should be showing as the concentration of sodium thiosulphate gets higher the time taken decreases and the cross becomes harder to see.

image07.png

My graph shows that if the concentration of sodium thiosulphate increases the rate increase, then deceases then proceeds to increase, this is also wrong because it should just show that as the concentration of sodium thiosulphate increases, the rate increases

Both of my experiments should of told me that , as you increase the water and decrease the sodium thiosulphate the time increases which means that it took longer  for the cross to disappear the reason for this is that as the

Concentration of sodium thiousulphate is increased it will take a shorter time for the solution to turn cloudy. This is because when the concentration is decreased there are less acid particles to collide with the sodium thiosulphate particles. But because of human errors my results do not show this. Also my second graph shows me that the greater the concentration of sodium thiosulphate the greater the rate.

THE EVALUATION

I believe the experiment could have worked better because

My results don’t look reliable or accurate and it is not showing what I predicted. I should have taken more readings. The me and the people in my group weren’t concentrating enough to when the cross disappeared and their was arguments about when it had actually disappeared and people came off task easily because some people forgot to start the stop watch as soon as the chemicals started reacting and some people forgot to stop the stop watch when the cross could no longer be seen. Also people may not have washed out the residual of water, sodium thiosulphate and hydrochloric acid out of the conical flask. Also maybe a person might not have measured the right amount of sodium thiosulphate, hydrochloric acid and water, or never kept the same amount of hydrochloric acid not all my results fit the pattern because of human error.  

My predictions would have been correct if the experiment was carried out probably. My experiment should have concluded that when the concentration of the sodium thiosulphate has gone up, as the first part of the experiment shows, the rate of reaction goes up. This is what was expected but are results have mistakes, and therefore obviously not perfect. There are two graphs for our results table to show the difference in time taken and rate of reaction i.e. by drawing a line of best fit on the rate of reaction graphs; we can see that there is s few results that are obviously completely wrong. Our procedure was not that good and needed to be improved, there was one odd result so everything came out not as expected. This means that the experiment was done not so well. If we could have done more repeats there would have been a better outcome. My results are not reliable. When it comes to my next experiment I will make sure the same people:  do the stop watch, and watch the x disappear. Make sure that when it comes to washing out the conical flask that there is no excess water, acid, or sodium left in it.

                                                                                                                  Abisoye Alakija         image08.png

image02.png

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

(?)
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 Science Skills and Knowledge Essays

See our best essays

Related GCSE Patterns of Behaviour essays

  1. Sodium Thiosulphate - investigating the rates of reaction.

    mat 1 stopwatch 1 Bunsen burner X board 1 pair of tongs 1 pair of goggles 1 apron Method: - Experiment 1 - Changing the concentration 5 cm3 of HCl (at concentration 1 mol./dm3) and 15 cm3 of sodium thiosulphate (at varying concentrations - 10 to 35 g/dm3)

  2. Free essay

    Close Your Eyes

    he said seriously. "Er thanks?" I questioned. Not knowing whether to take this as a compliment or whether to be worried. This conversation was obviously going nowhere so I got up and started walking out of the room. Then Dougie started talking again.

  1. Investigation exploring rates of reaction, using the reaction between sodium thiosulphate and hydrochloric acid ...

    When acid is more concentrated, there are more acid particles in it. The chance of a successful collision occurring is increased. Although higher concentration means a faster rate of reaction, kinetic theory is relevant. The molecules in the reaction mixture have a range of energy levels, so successful collisions only happen if the molecule has enough kinetic energy.

  2. How Does The Concentration Of Sodium Thiosulfate Affect The Rate Of This Reaction?

    I believe this will happen because, according to the collision theory, as the concentration of a solution is increased the number of particles inside the solution increases. If the number of particles inside the solution is increased it makes collisions with reacting particles more likely.

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