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

The aim of this coursework is to investigate how the temperature can affect the rate of reaction. I will use sodium thiosulphate and hydrochloric acid as the reactants of the experiment, and then vary the temperature to see the speed at which they react.

Extracts from this document...

Introduction

Chemistry Coursework Rate of Reaction Candidate name: YangMei (Juliana) Plant 11K Candidate number: 8087 Rates of reaction Aim: The aim of this coursework is to investigate how the temperature can affect the rate of reaction. I will use sodium thiosulphate and hydrochloric acid as the reactants of the experiment, and then vary the temperature to see the speed at which they react. Scientific Background: The rate of reaction is the speed at which a chemical reaction takes place. The rate at which the reaction takes place cannot be worked out from its chemical reactions, but by measuring how much reactant is used up in a certain time, or how much product is formed at a certain time. Whatever the matter, the amount of product formed at the end of the experiment should always equal to the amount of reactants at the start of the experiment, because all chemical equations are balanced even when the product is invisible. The product of a chemical reaction is never disappeared but transferred to another state, such as from a liquid to a gas. The rate at which a chemical reaction takes place can vary greatly, such as from extreme explosions to slow rusting. ...read more.

Middle

* Use the same volume of concentration throughout the whole experiment. Prediction: Since the rate of reaction is the speed at which a chemical reaction takes place, I predict that if I increase the temperature of the reaction, the speed at which the reaction is going to occur will also increase. This is cause by the molecules becoming thermally active, which increases the collisions between particles and so the bonds breaks more quickly. This increase of speed at which the bonds break also increases the reaction, so the speed at which the reaction takes place in a given time accelerates. On the other hand, if the temperature decreases then the rate at which the reaction takes place will also decrease because there are no movement/ collisions amongst the molecules to create enough energy to break the energy barriers to start a reaction, in other words there is not enough kinetic energy to break the existing bonds between the molecules. In this case the reaction will only take place when hydrochloric acid is added to the sodium thoisulphate, as sodium is alkaline when it mixes with the hydrochloric acid an exothermic reaction takes place. ...read more.

Conclusion

disappear sec 20 1.08 25 35 30 25 35 17 40 15 45 13 50 12 Evaluation: I have added water to the solution to make it more dilute, the readings did indeed became more spread out. Since I have diluted the solution to a half, the time taken for the cross to disappear should now double, but according to the table only a few did e.g. at 20 c. This shows that some errors have occurred in the experiment, which is why the readings don't match. It could be that the stopwatch was started late or some careless mistakes made by me. I have to take this into account when I do my final experiment. The accuracy of the results could be improved further if I have recorded the readings to 2 decimal places instead of none at all. By recording it to 2 decimal places the results are more likely to be more accurate as it involves more detailed. Final Experiment Volume of concentration: 40 ml water 10 ml sodium thoisulphate Temperature c Time for cross to disappear sec 0 8.13 5 7.22 10 5.31 15 4.21 20 3.04 25 2.31 30 1.40 35 1.05 40 0.55 45 0.37 50 0.25 ...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. Marked by a teacher

    Rate of Reaction Chemistry Coursework

    4 star(s)

    We chose to use the burette for this as it was easy to read of. It has the numbers down the side so we can see how many ml we are losing. We have to put it into the water bowl to make sure we don't lose any water before we perform the reaction 4)

  2. Marked by a teacher

    In this project I am going to investigate rates of reaction of an indigestion ...

    3 star(s)

    I have noticed the graph has more points of interest than that of concentration (see page 2). I could do this in two different ways: * Measure how fast reactants disappear This can be measured either by weighing a solution before and after to check mass change, or by sight

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

    For the real experiment I will take 5 readings, and a repeat for each. I will take a reading at the following degrees, going up in 15: 5, 20, 35, 50, and 65.

  2. 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

  1. Does temperature affect the rate of reaction between Sodium Thiosulphate and Hydrochloric acid?

    I will then measure 6ml of Hydrochloric acid again with the aid of the measuring cylinder but then leave the acid in the cylinder until the Sodium Thiosulphate is heated to a certain temperature. I will then turn the gas on and light the Bunsen.

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

    A powder has the largest surface area and will have the fastest rate of reaction. This is why catalysts are often used as powders. A catalyst will change the rate of reaction. In most cases, the catalyst is used to make a reaction go faster.

  1. To investigate the effect of varying the masses of white sugar and yeast and ...

    As bakers know, before any dough can yield a light, aerated loaf of bread, it must be fermented for a sufficiently long time to permit the yeast to convert the assimilable carbohydrates into alcohol and carbon dioxide as the principal end products.

  2. Enzyme Coursework.

    When Hydrogen Peroxide and the yeast suspension solution are mixed, a very vigorous and exothermic reaction takes place. Oxygen is the product produced. Hydrogen Peroxide catalyse reaction water + oxygen H2O2 catalyse reaction H2O + O2 Hydrogen Peroxide is the substrate in this reaction.

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