• 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

Science Investigation (Chemistry) - Rate of Reaction Planning: Outline: I will investigate the relationship between the rate of a reaction and the amount of catalyst added to the reaction. I will use hydrogen peroxide and speed pu the decomposition of it by adding manganese(IV), MnO2 as catalyst. Fair test: In order to maintain fair test conditions I will control variables that will affect the rate of reaction. The factors that are able to affect the rate of reaction include: * Temperature * Surface Area * Concentration * Catalyst Since I am investigating the relationship between rate of reaction and catalysts, the other 3 factors will remain constant throughout the experiment. Temperature: At higher temperatures, the faster moving particles have more kinetic energy. This means they are moving quicker and will collide more often and with more energy, causing an increase in the number of effective collisions. Surface Area: If more surface area is available, the number of particles of the solid reactant available for collision will increase. However, I am dealing with hydrogen peroxide (liquid) then there isn't a surface area for me to control. Concentration: More concentrated solutions contain more particles in the same space, making them more likely to collide. The increase in the number of collisions with sufficient energy increases the rate of reaction. These explain why I would need to control those factors because they would affect my results dramatically. ...read more.

Middle

12 11.00 4.00 40 14 15 15 14.67 3.67 50 20 19 20 19.67 5.00 60 23 23 24 23.33 3.67 0.04g catalyst used Amount of gas produced (cm�) Time (sec) Trial 1 Trial 2 Trial 3 Average Average Gain in gas produced from previous (cm�) 0 0 0 0 0.00 0.00 10 5 8 7 6.67 6.67 20 13 14 13 13.33 6.67 30 20 19 19 19.33 6.00 40 29 30 28 29.00 9.67 50 35 35 36 35.33 6.33 60 42 41 40 41.00 5.67 0.06g catalyst used Amount of gas produced (cm�) Time (sec) Trial 1 Trial 2 Trial 3 Average Average Gain in gas produced from previous (cm�) 0 0 0 0 0.00 0.00 10 10 11 11 10.67 10.67 20 22 21 20 21.00 10.33 30 32 30 33 31.67 10.67 40 40 39 41 40.00 8.33 50 46 48 46 46.67 6.67 60 51 50 50 50.33 3.67 0.08g catalyst used Amount of gas produced (cm�) Time (sec) Trial 1 Trial 2 Trial 3 Average Average Gain in gas produced from previous (cm�) 0 0 0 0 0.00 0.00 10 18 18 16 17.33 17.33 20 31 30 29 30.00 12.67 30 40 41 41 40.67 10.67 40 48 47 45 46.67 6.00 50 55 54 55 54.67 8.00 60 62 61 62 61.67 7.00 0.10g catalyst used Amount of gas produced (cm�) Time (sec) ...read more.

Conclusion

Looking back on experiment I believe that there are many ways to improve it. One way is the accuracy of the measuring of the catalyst this can be done by requesting a new scale which should not have any chances of any faulty measurements. This would make every measurement of catalyst I take virtually no faults at all. My graph is very basic and one way to improve this will be to increase my range of tests, this will allow me to know where exactly the point where no more oxygen can be created is. Maybe doing until 2 minutes (120 sec) will allow me to locate where it is. I think the timing was as accurate and reliable as it could be, but only a second or third experiment would back that up fully. The equipment we used was reasonable but not the best, but for the conditions we were based in it was the best we were going to get. I could investigate on what type of catalysts is more effective for the speeding up of the decomposition of hydrogen peroxide. Possible catalyst selections include: * Manganese IV oxide (MnO2) * Zinc oxide (ZnO) * Lead IV oxide (PbO2) * Aluminium oxide (Al2O3) * Iron III oxide (Fe2O3) * Copper II oxide (CuO) * Copper III oxide (Cu2O) This might help me understand more about catalyst and what type of metals are best for catalysts, such as: transition metals. I could investigate on the concentration of hydrogen peroxide and keeping the catalyst constant, and also I can investigate on the effects of pH with rates of reaction. ...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. Investigation of the effect of the concentration of hydrogen peroxide on the rate of ...

    This process was repeated seven times, except with different concentrations. This was to obtain a good set of results. The concentration however was changed in all these experiments to observe the affect of it on the rate of the reaction.

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

    particles, and therefore twice as many collisions should occur. This means that when the concentration doubles, twice as many collisions between the H202 and Mn02 particles occur and the rate of the reaction also doubles. My Prediction: If there are double as many particles, there is double the chance of a collision between the hydrogen peroxide particles and the manganese dioxide (catalyst)

  1. The Effect of Catalase in the Breakdown of Hydrogen Peroxide

    Do to this a gas syringe can be used in placed of the bung, on top of the conical flask and connected to the delivery tube. It would apply to the collection of any fluid or gas - almost like a filter.

  2. To Investigate the Effect of Manganese IV Oxide on the rate of decomposition of ...

    Rory Good Description of Method The above apparatus will be set up. The bung will then be removed temporarily and the catalyst dropped into the hydrogen peroxide. The bung will then be replaced immediately and the stopwatch started. As soon as the test tube is filled with oxygen the stopwatch will be stopped and the time recorded.

  1. Magnesium Oxide

    Crucible and Lid * Digital Balance - 0.01g * Goggles * Heat Proof Mat * Magnesium Ribbon (200cm) * Pipe-clay triangle * Tongs * Tripod Safety We used the crucible and lid because it won't crack which means there would be no injury to anyone.

  2. Investigation into the effect of increasing the concentration of hydrogen peroxide on the decomposition ...

    If there are not many, its rate is low. The rate of reaction depends on how many successful collisions there are in an amount of time. To change the rate of reaction the concentration of the acid should be increase and the reaction will happen faster. In dilute acid, there are not so many acid particles.

  1. To investigate one factor that will affect the rate of decomposition of hydrogen peroxide.

    Now I am in a position to answer the question "How does the rate of reaction depends on the concentrations of hydrogen peroxide ?". I will plot the initial rate of reaction against concentration of hydrogen peroxide and I can arrive at the effect that it is a straight line graph.

  2. Investigating the factors that affect the rate of hydrogen peroxide.

    The enzyme combines with the substrate, allowing the reaction to take place with a much lower activation energy. The activation energy is the energy required to break the chemical bonds in reactants. With a lower activation energy the reaction takes place higher.

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