• 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

Investigating Factors that Affect the Rate of Reaction of the Decomposition of Hydrogen Peroxide (Only method and tables no calculations0

Extracts from this document...

Introduction

ï»¿Investigating Factors that Affect the Rate of Reaction of the Decomposition of Hydrogen Peroxide Emilio Lanza Introduction- In this experiment, the rate of reaction, calculated in kPa sec-1, of the decomposition of hydrogen peroxide will be investigated to see how the change in concentration of hydrogen peroxide and the change in temperature affect the rate of reaction. The data will be collected by measuring the gas pressure. The product of Hydrogen Peroxide is oxygen in a gas state thus it is mandatory to use the gas pressure sensor. By calculating the difference of the gas pressure divided by the amount of time from the raw data collection it is able to find the rate of reaction of the decomposition of hydrogen peroxide. Control Variable- 1mL of yeast (catalyst) is being used in every trial. The volume of H2O2 is always 4 mL, even though the concentration changes and the sizes and type of test tube was the same because it can change the pressure. Independent Variable- Concentration of H2O2 (M) and the temperature (°C) Dependent Variable- The rate of reaction of the decomposition of hydrogen peroxide → rate of reaction = . ...read more.

Middle

Transfer the yeast solution from its test tube into the test tube containing H2O2 solution and shake lightly to mix the two solutions together. As quick as possible seal the test tube with the one-hole stopper connected to the Gas Pressure Sensor and place the test tube back into the water by holding the test tube with the test tube holder. Next click collect data on the LoggerPro Program to begin collecting data. (THE LAST TWO STEPS ARE CRUCIAL AND MUSTBE DONE AS QUICK AS POSSIBLE TO AVOID ANY EXTERNAL INFLUENCES). It is needed to collect the data for three minutes once three minutes is up, carefully remove the test tube from the water by holding onto the test tube holder and set it in the test tube rack. Next slowly and carefully begin to tale out the stopper from the test tube allowing the gas pressure to escape. Store the results from the first trial by selecting Store Latest Run from the Experiment menu. After doing this a table of data and the graph will be saved. Then make sure to clean and trash the solution that is in the test tube. ...read more.

Conclusion

Make sure to find the average temperature (°C) and include it in the analysis table. Then compare and contrast the different effects the rate o reaction caused by the change in concentration of H2O2 and in the change of temperature. (The data table is an example of the data table that will be printed from the computer after each trial and part is done from LoggerPro Progam. The only thing is that it will record the gas pressure until 3 minutes. Again only an example how it should look like). The Gas Pressure from the Decomposition of H2O2 After Every Second Time (sec) Gas Pressure (kPa) 1 2 3 4 5 6 7 8 9 10 Data Analysis Table for the Decomposition of H2O2 Part # Average Temperature (°C) Average Rate of Reaction (kPa sec-1) Concentration of H2O2 in % Concentration of Yeast (M) Part 1 Part 2 Part 3 Part 4 Part 5 The Temperature (°C) of the Water During Each Part of the Lab and Each Trial Parts of Experiments Trial 1 Trial 2 Trial 3 Part 1 Temperature (°C) Part 2 Temperature (°C) Part 3 Temperature (°C) Part 4 Temperature(°C) Part 5 Temperature (°C) ...read more.

The above preview is unformatted text

This student written piece of work is one of many that can be found in our International Baccalaureate 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

Related International Baccalaureate Chemistry essays

1. THE CATALYTIC DECOMPOSITION OF HYDROGEN PEROXIDE

Concentration of hydrogen peroxide (3%) Temperature at which the reaction occurs (room temperature 260C) Pressure at which the reaction occurs (1 atm) Apparatus List: 1. Manganese (V) Oxide - 100g 2. Hydrogen Peroxide (3%) - 500cm3 3. Conical Flask X1 4. Beaker (100cm3) X1 5.

2. Investigate the rate of reaction of luminol in various factors. The objective was to ...

This can be explained by the Maxwell-Boltzmann distribution(2). Catalysts are substances help to lower the activation enthalpy, using an alternative route. They are also not used up after the reaction. For luminol reactions, the catalysts used can only be metal catalysts, e.g. CuSO4 * 5H2O and K4[Fe(CN)6](4). The smaller the substance, the larger the surface area, which means it has more site for reaction to take place.

1. Aim: Using an iodine clock reaction to find the order of hydrogen peroxide and ...

3.19 is the time taken for the quickest reaction, and 1 is the uncertainty. This uncertainty is the greatest of all and is applied to all experiments. As the graph above demonstrates, the rate becomes proportionally slower as the volume of H2O2 is increased, showing that it is most likely 1st order.

2. DCP+CE Analysis of a Hydrogen Peroxide Solution

Processed Data - Amount of KMnO4 Added in Both of the Titration Trials Titration 1 Trials Calculations Amount of KMnO4 (ml � 0.15ml) 1 (Final reading) - (Initial Reading) = 23 - 0.0 23.00 2 24.2 - 0.0 24.20 3 26.5 - 0.0 26.50 4 22.55 22.55 5 26.5 26.50

1. Investigate one factor affecting the rate of enzymatic decomposition of hydrogen peroxide by catalase. ...

There was a direct relationship between the volume of the potato and rate of reaction and the rate of reaction increases with the size of the liver piece. In graph 2, the equation found out, y=0.0391x+0.077, with a R2 value of 0.9891 shows that the line of a increasing function.

2. Reaction Rate

Pre-determining a target volume is vital for us to be able to effectively compare and form a relationship between the concentrations of H2SO4 and time taken to produce the same amount of hydrogen gas. * The same person handling the stopwatch during the experiment.

1. The chemistry of atmospheric and water pollution.

The following are factors which determine the concentrations of particular ions in a body of water such as a river or ocean: Natural sources of ions Depending on the natural body of water?s location, there are different possibilities of ions which could be present in that particular water system.

2. Investigating the Effects of Surface Area on the Rate of Reaction

Add the magnesium ribbon 5. Seal the flask with a rubber stopper as quickly as you can, at the same time have someone else present to start the stop watch once the magnesium ribbon has been added to the hydrochloric acid 6. As the reaction takes place, note down the time it takes for the gas collected to reach a multiple of 5 (i.e.

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