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

Decomposition of Hydrogen Peroxide Lab

Extracts from this document...

Introduction

Purpose To find the activation energy of the following reaction: Data Collection Part 1 Element Molarity 0.88 M (3%) 0.5M Volume Temperature Table 1-Increase in Pressure over Time as 0.88M and 0.5M react at 21.5 Time (s) Pressure (kPa)�0.2% 10 103.6 20 104.0 30 104.0 40 104.0 50 104.5 60 105.4 70 105.9 80 107.0 90 108.6 100 109.7 110 111.1 120 113.4 130 115.4 140 117.2 150 119.3 160 121.8 170 124.0 180 125.9 * Uncertainty of pressure based on instrument stated uncertainty. Sample Calculation Converting Concentration of into Molarity Part 2 Element Molarity 0.88 M (3%) 0.25M Volume Temperature Table 2-Increase in Pressure over Time as 0.88M and 0.25M react at 21.5 Time (s) Pressure (kPa)�0.2% 30 102.0 40 102.2 50 102.7 60 102.9 70 104.5 80 104.5 90 104.7 100 105.6 110 106.3 120 106.5 130 107.0 140 108.1 150 108.8 160 110.0 170 110.6 180 111.3 Qualitative Observations In general for the 4 trials, the following observations were made: * Liquid turned a dark shade of yellow once the reactants were mixed * Once the reactants were mixed, there was a steady increase in bubbling Part 3 Element Molarity 0.44 M (1.5%) ...read more.

Middle

Conclusion In conclusion it was found that the activation energy of the decomposition of hydrogen peroxide with the help of the catalyst KI is . When compared to an actual value there was a percent difference of 43%. In fact the actual value that was used is the activation energy of hydrogen peroxide in the absence of a catalyst. So in reality it is likely that a catalyst would cause the activation energy to be even smaller, and the percent difference would be even greater. The only reasonable explanation as to why the calculated activation energy is so much greater is that somewhere during the experiment a random error occurred but since only two trials were done, it is impossible to pinpoint where it exactly occurred. When looking at graphs 1-4 it can be seen that as time went on the pressure increased exponentially. This makes sense because over time the amount of gas increased, and so the pressure would increase too. In addition in graphs 1-4, if a curved line of best fit were to be plotted, than the y-intercept would show the pressure of the room at the moment the experiment was conducted. ...read more.

Conclusion

Lastly, when the test tube was put in the water bath, the temperature of the water bath was constantly changing because the temperature of the water was relatively lower than the room temperature. This in turn is what caused fluctuation in the temperature readings. This in turn could have also caused the initial rate to vary because as discussed earlier, even the slightest change in temperature causes the initial rate to change. This experiment can be improved in many ways. One of the main things that can be done is that the experiment should be conducted at different temperatures so that at least a minimum of 5 k values against 1/T can be plotted on graph 5. In addition, the temperature increments should have a relatively broad range, which in turn will make the data and the trends clearer. In addition, the experiment should be conducted on the same day so as the temperature can be kept constant for certain k values. In order to keep the temperature of the water bath constant, the experiment should be conducted in a closed environment so that less energy is lost to the environment. ...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

See related essaysSee related essays

Related International Baccalaureate Chemistry essays

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

    Balance A balance is used for fast and accurate weighing. The error of 3-decimal-place balance is ?0.001g while that of 2-decimal-place balance is ?0.01g. The 3-decimal-place balance gives a more accurate weighing. Beaker Beaker is used to hold solution, in this case, dissolve the solid and dilute solution.

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

    When graphed, five experiments were sufficient enough to notice that there was a clear trend line for each of the experiment sets, and so further experiments did not need to be carried out.

  1. Change of Potential Difference in Voltaic Cells Lab Report

    From the molar mass of copper sulfate pentahydrate, CuSO4.5H2O and the number of moles we can find the mass in grams of solute needed. Mass of copper sulfate pentahydrate = 1 249.71 = 249.71 g This mass is required to prepare 1L of 1M copper sulfate solution.

  2. In our research project, we will try to compare the qualitative contents of some ...

    However, this drink is carbonated. It has a natural lemon essence added to it. UC 1000 (Lemon) Electrolyte Test Chloride Test Test for Reducing Sugars pH Test Result Positive Positive Positive Acidic Remarks The solution contains electricity. It is a mild electrolyte and can conduct currents up to 10 mA.

  1. DCP+CE Analysis of a Hydrogen Peroxide Solution

    � (0.15+0.15+0.15) = 62.0ml � 0.45ml (62.0�0.45ml) / 3 = (62.0ml�0.73%) / (3�0%) = (62.0/3) � (0.73% + 0%) = 20.7 � 0.73% = 20.7ml � 0.15ml Table 6. Summary Data of Processed Calculation Processed Data Calculations Average of the 1st Titration Average amount of Na2C2O4 is 0.0024mols � 1.44x10-8mols

  2. Investigating Factors that Affect the Rate of Reaction of the Decomposition of Hydrogen ...

    Make sure that the majority of the test tube is submerged in water. Using the other 10 mL pipette, transfer 1 mL of 0.5 M Yeast into the other 10 mL graduated cylinder. From this graduated cylinder, transfer the 0.5 M Yeast to a new 10 mL test tube; seal the test tube with a new solid rubber stopper.

  1. Chemistry lab reort-molar volume of hydrogen

    Calculation The number of moles of hydrogen gas produced is calculated through the reaction that it undergoes: The molar volume of hydrogen gas at STP is calculated using the combined gas law: According to the combined gas law: The molar volume of hydrogen gas at STP is Theoretical value: Molar

  2. Reaction Rate

    ALL EQUIPMENT IS TO BE KEPT CONSTANT TROUGHT THE EXPERIMENT TO OBTAIN CONSISTENCY EXPERIMENTAL PLAN Materials/Equipment: * 1x Test Tube * 1x Delivery Tube * 1x Rubber Stopper * 2x 50mL Measuring Cylinders * 1x Plastic Container * 1x Retort Stand and Clamp Set * 1x Laptop * 1x Desk

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