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

Investigate the effect of changing the hydrogen peroxide concentration on the rate of reaction of the break down of hydrogen peroxide by catalase.

Extracts from this document...


Planning Sheet for Science Investigation Problem/Aims My aims for this experiment are to investigate the effect of changing the hydrogen peroxide concentration on the rate of reaction of the break down of hydrogen peroxide by catalase. Background Information Predictions I predict that the higher the concentration of hydrogen peroxide is the more it will react with the catalase and therefor producing more oxygen. This is due to the fact that as the concentration of hydrogen peroxide is increased, the number of collisions between the enzyme (yeast) and substrate (hydrogen peroxide) increases. I believe that if I double the concentration of hydrogen peroxide, the rate of reaction will also double. Key Factors *The main factors that I fell will influence the experiment are: 1) Temperature of the catalase and hydrogen peroxide. As the more heat there is the more kinetic energy the enzyme and substrate will have causing them to move faster which will then cause more collisions and faster reactions rates. 2) The concentration of hydrogen peroxide. The higher the concentration of hydrogen peroxide the more substrates there will be, which will enable more collisions between the hydrogen peroxide and catalase, therefore the reaction rate will increase. ...read more.


This is where the reaction of the break down of hydrogen peroxide by catalase is going to take place. 9) I placed the conical flask in a large water container. This is going to be filled with water and have a thermometer in it. This will act as a water bath to try and keep the temperature of the solutions constant. 10) The burette is turned upside down and clicked on to it's stand, this is where the oxygen produced from the reaction is gong to be collected and record. This is to help me find out how much oxygen is produced in two minutes. (I must make sure the bottom of the burette is closed completely to make sure no oxygen will enter or escape.) 11) The opening of the burette will stand in another container of water. I must make sure the water level is over the top of the opening of the burette or my results will not be reliable. The burette must be filled with water, but again I must make sure the water stops on one of the markers so I can make an exact result of where the starting measurement of the water in the burette will be. ...read more.


To find out the process data I used the same formula as in table one, which is; Starting measurement - 5cm3 - Final measurement = Total oxygen produced Beaker number Concentration of H2O2 / M Volume of h202 / cm3 Volume of distilled water / cm3 Volume of catalase used / cm3 Starting measurement / cm3 Final measurement /cm3 Total oxygen produced / cm3 1 1.0 5 0 5 48.2 29.6 13.6 2 0.9 4.5 0.5 5 46.3 28.3 13.0 3 0.8 4 1 5 47.1 29.3 12.8 4 0.7 3.5 1.5 5 49.3 31.9 12.4 5 0.6 3 2 5 48.7 32.4 11.3 6 0.5 2.5 2.5 5 47.1 31.3 10.8 7 0.4 2 3 5 48.7 34.3 9.4 8 0.3 1.5 3.5 5 48.4 36.6 6.8 9 0.2 1 4 5 47.3 38.8 3.6 10 0.1 0.5 4.5 5 49.7 43.9 0.8 11 0.0 0 5 5 47.3 42.3 0.0 Table 3 - this table shows the averages of tables 1 and 2 on the total oxygen produced for each concentration of hydrogen peroxide. Number Beaker Concentration of H202 / cm3 Average total oxygen produced / cm3 1 1.0 14.0 2 0.9 13.4 3 0.8 13.0 4 0.7 11.8 5 0.6 11.1 6 0.5 10.4 7 0.4 9.3 8 0.3 6.9 9 0.2 3.8 10 0.1 1.1 11 0.0 0.0 *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 Aqueous Chemistry 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 Aqueous Chemistry essays

  1. Marked by a teacher

    To investigate the effect of temperature on the rate of reaction

    4 star(s)

    Variables Variable Why does it need to be controlled? How will it be measured/controlled? Dependant Amount of CO2 The more CO2 produced in less time, the faster the rate of reaction. This is not controlled. It is what we are measuring and will be measured using a gas syringe.


    Therefore, by increasing the temperature the molecules will move faster and collide with each other more quickly. This will increase the rate of reaction and so the temperature will be kept constant throughout the experiment by carrying it out under room temperature.

  1. to investigate how the concentration affects the rate of the reaction

    48 220 58 52 49 240 59 53 49 260 59 55 Stopped 280 stopped 56 300 56 320 Stopped These are all the readings for my experiment. I followed all the necessary procedures and safety measures needed. I included all the units of measurements used in the course of this experiment.

  2. Plan an Experiment to Investigate the Effect of pH on Immobilised Yeast Cells on ...

    In my experiment I am going to do I am using dried yeast, which contains a suitable enzyme 'catalase'. So therefore I am using the catalase in the yeast to speed up the reaction, the products being produced and the overall results.

  1. To investigate the effect of concentration on the temperature rise, heat evolved and heat ...

    Procedure Measure 50 ml of 1 M NaOH using a burette and fix it on a stand. Measure 25 ml of 1 M HCl in a pipette and pour completely into the polystyrene cup. Place this cup under the nozzle of the burette so that when alkali drops from the burette it doesn't spill out.

  2. The Effect of Concentration on the Rate of Reaction.

    Thus the rate of reaction increased. However, the experiments using 10g of marble chips reacted too quickly and so it was decided that 5g of marble chips should be used in the actual investigation. The 10g of marble chips reacted so quickly because there were more chips and so this meant that there was a greater surface area.

  1. Determine the concentration of lime water.

    The pipette that I used was also holding back some of the solution so not all of the solution was transferred. This problem also occurred when measuring the chemicals because some chemicals were carried over to the next experiment. This could be avoided by drying out the beakers and measuring cylinders or by using separate apparatus.

  2. How Does Changing the Concentration of a Substance Affect the Rate of Reaction?

    Then, using the line of best fit I will calculate the rate of reaction by, if the line of best fit is a curve, I will draw a tangent on my line of best fit and then draw a right-angled triangle from the tangent.

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