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

rate of reaction

Extracts from this document...

Introduction

Rate of reaction The rate of reaction is how quickly a reaction takes place and the rate of the transformation of a product throughout a chemical reaction. The rate of reaction is measured by dividing 1 by the time taken for the reaction to take place. If a reaction has a low rate, that means the molecules unite at a slower speed, than a reaction with a high rate. Aim The aim is investigating the rate of reaction between Sodium Thiosulphate and Hydrochloric acid, and the effects of changing the concentration have on them. The equation for the reaction between Sodium Thiosulphate and Hydrochloric acid is: The sulphur created appears in the form of very small particles of solid. This leaves a white/yellow precipitate. Safety There are a lot of safety issues that we have to be careful with, as things are very unpredictable. It is important to wear goggles throughout this experiment, as it will protect the eyes. We must be careful with the chemicals, and not eat or drink in the science lab as we can get chemicals on to our hands. We should also dispose the mixture of chemicals of down a well-flushed sink. ...read more.

Middle

* I will keep the volume of sodium thiosulphate at a regular amount throughout the experiment; otherwise this would make the results inaccurate. * I must make sure that the conical flask is rinsed well and clean before use; otherwise it could affect the results of the experiment. * I will make sure, that I add the sodium thiosulphate and the hydrochloric acid in the conical flask at the same order as usual. * I will laminate the cross and make sure that I keep the same one throughout the experiment. * I must start the stopwatch at the exact time as we put the sodium thiosulphate and hydrochloric acid into the conical flask. Reliability To make sure that my results are reliable, my measurements have to be precise and accurate. * I can do this by repeating the experiment 3 times. * I will be using the same measurement each time for deciding when the cross has disappeared. * I will also use a digital stopwatch, as it is more accurate than a manual stopwatch. * I will ensure to do the same experiment on the same day and in the same lesson so the temperature stays the same at 20�C and doesn't affect my results. ...read more.

Conclusion

This tells us that increasing the concentration would lead to more collisions and therefore the rate of reaction would occur faster. For example, by doubling the amount of concentration, it would double the amount of reactant particles. This would lead to more collisions taking place, and therefore the cross will disappear quicker. My results of my experiment support my prediction of the rate of reaction increasing, when the concentration of HCL acid is increased too. Evaluation I carried my experiment the way I intended to, and my results were accurate enough to prove the prediction. The points on my graph gave the accepted straight-line and curve to give an idea of a relationship; which means I did not get any anomalous results. However, they could be improved to drop on a straighter line as some points didn't drop on the line as it usually would. I could do this by: * Doing the experiment more times, to give more accurate results. * Measuring the solution more accurately. * Taking a more precise reading when deciding, that the cross has disappeared. * Using dry conical flasks for each experiment. I would be more precise with these points, as this would again improve accuracy. ?? ?? ?? ?? Yasmin Ramadan Year 11 Candidate No.: 3501 1 ...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

Here's what a teacher thought of this essay

3 star(s)

This report is well written but brief. The data collected covers the appropriate range with regular checks for reliability. There are specific strengths and improvements suggested throughout.

Marked by teacher Cornelia Bruce 17/04/2013

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

    Chemistry Coursework - How the concentration effects the rate of reaction between sodium thiosulphate ...

    I chose do six sets or recordings for each experiment for convenience as they numbers were all round and easy to use but partly also because of lack of time to conduct the experiment. We were limited to just only above one hour to conduct our experiment but we were given two separate occasions on what to do so.

  2. The effects of caffeine on reaction time

    I will then record the reaction time, no. of correct, wrong, and not attempted answers. Caffeine source: There are a variety of food products that I can use as a caffeine source. From the products available Red Bull the energy drink has the most concentration of caffeine but it has

  1. Factors Affecting the Rate of Catalytic Decomposition of Hydrogen Peroxide.

    For the first graph, the average value taken was 0.11g. For the second graph, the average total mass lost measured was 0.44g. This was done once per reading, so the experimental error for the top pan balance is: 0.1 (g)

  2. An Investigation of the Effect of Copper Sulphate on Catalase Activity.

    This air displaced by the stopper must not be measured as oxygen produced by the reaction. Record the volume of oxygen produced every 20 seconds for the following 3 minutes. Carry out two replications of this test. Repeat this process five more times but each time add a different concentration

  1. Investigation into the Effect Concentration has on Rate of Reaction.

    If the particles have less than this amount of energy, they simply bounce off each other and no reaction takes place. The faster the particles are going, the more energy they have. This is the collision theory. From this we know that the more collisions between particles in a given time, the faster the reaction.

  2. The effects of temperature on the rate of reaction ofsodium thiosulphate with hydrochloric acid.

    As stated above, depending on the reactants, there is a speed barrier which must be crossed in order for the reaction to take place. This is the minimum amount of chemical potential energy needed to cause a chemical reaction. This barrier is called activation energy.

  1. Rates of reaction between Magnesium and HCl.

    flask, rather than going into the burette, or the magnesium strip that reacted with the hydrochloric acid may have been used up and no further reaction could take place, so therefore the amount of hydrogen produced would have stayed the same.

  2. The reaction between sodium thiosulphate and hydrochloric acid:Looking at the graph the order of ...

    It is the energy that is needed to start breaking the bonds in the colliding molecules so that the collision can lead to a reaction. Calculating activation enthalpy from rates of reaction (refer to page11-12) Arrhenius equation: In k = constant -Ea RT Where k is the rate constant, R

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