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

Lab - Measuring an Activation Energy

Extracts from this document...


LAB: MEASURING AN ACTIVATION ENERGY Activation Energy: Defined as the amount of energy required to initiate a chemical reaction or the difference in energy of the reactants and the energy of the activated complex (Ea). Objective: To examine the effect of changing temperature on the rate of the reaction of permanganate ions with oxalic acid according to the equation: 2MnO4- + 5H2C2O4 + 6H+ 2Mn2+ + 10CO2 + 8H2O Objective: To determine the activation energy for the reaction. Procedure: See attached. Note that due to time constraints, multiple trials were not able to be performed. Data Collection: Quantitative Data Trial Temp (�C � 0.3) Temp (K) 1/Temp (K) Time (sec � 0.5) 1/Time=Rate ln(Rate) 1 38.8 311.8 0.00321 349 0.00287 -5.85507 2 63.5 336.5 0.00297 45 0.02222 -3.80667 3 70.3 343.3 0.00291 29 0.03448 -3.36730 4 86.1 359.1 0.00278 12 0.08333 -2.48491 5 94.2 367.2 0.00272 6 0.16667 -1.79176 Qualitative Data The permanganate liquid was an extremely deep shade of purple, and the oxalic acid was virtually transparent. For the first trial, after heating both the permanganate and acid up to about 40�C, when I proceeded to mix them, the reaction almost never took place. ...read more.


No smell was derived from this process, and the beaker did feel a little warm on the outside, thus it was an exothermic reaction. Data Processing: Graph 1: Temperature (K) vs. Time (sec) As we can see from the above graph, the relationship between temperature (K) and time (sec) is clearly not of a linear nature. This makes sense, because when we take the tangent to the curve on the graph above, we will have the rate of each reaction. We know that by increasing the temperature, since temperature is proportional to the average kinetic energy of the particles, the number of collisions will increase as well as the energy of the particles themselves - so more particles have sufficient energy to overcome the activation energy barrier and undergo successful collisions. This in turn means that the rate of reaction will increase with the temperature. Because of this presumed knowledge, if the graph of temperature vs. time was indeed linear, then the tangents would all be equal (meaning the rates would all be equal) and we clearly know this is not the case. ...read more.


I was also able to learn, from the Arrhenius equation, a graphical interpretation of the relationships between temperature and time and temperature and rate. Although I did not calculate a percent error for this experiment, the uncertainty evident in my raw data collection still serves to show that there were sources of error. Firstly, in terms of systematic error, one was the equipment, specifically the test tubes used. They were varying in size, and inside some of them there was still leftover "gunk" from other experiments - despite our best efforts to clean them. Another source of error could be the accuracy of the thermometer: even though we were consistent in the thermometer we used, we had to share 1 between 3 water baths, therefore maybe we didn't allow enough time for it to absorb or readjust to the varying temperature conditions. A source of random error could be the heat loss between the time we took the test tubes out of the water bath to when we actually mixed them: even though we heated them to a constant temperature, in the time that it took to mix the two contents together and stir, some heat was probably lost. ?? ?? ?? ?? ...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. Determining the activation energy of a reaction, By using the experimental data and the ...

    There are many sources of uncertainties. Firstly, the solutions used in this study were prepared by lab equipments such as measuring cylinders and mass balance, which all have degrees of accuracy associated with them (for example, a mass balance's accuracy is g�0.001).

  2. Aim: To calculate the activation energy (EA) for the reaction between Br- and BrO3- ...

    Experiment data can thus be used to generate this straight line and use it to calculate activation energy. Hypothesis: As the temperature increases (with the concentration kept at a constant) the rate of the reaction increases, as the temperature decreases (with the concentration kept at a constant)

  1. Determining the Activation Energy of a Reaction

    Inserting all values (10) into a list. Finding Statistics on list (L1) Statistics Statistics cont. Since Q1 and Q3 have been found, any outliers may be found. All values are in kJ Interquartile Range = Q3 - Q1 = 58 - 50 = 8 Therefore, outliers would be found below: Q1 - (1.5 x IQR)

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

    * Beakers * Dropper * Tripod Stand * Bunsen Burner * Distilled Water * pH meter * Connecting Wires * Battery * Mili-Ammeter * Light Emitting Diode (LED) * * Benedict's solution * Silver Nitrate (AgNO3) solution Variables: There are not many variables in our experiment because of the fact that there is no quantitative data.

  1. Change of Potential Difference in Voltaic Cells Lab Report

    The most diluted concentration of copper sulfate (0.2 M) shows the lowest potential difference (voltage) between the two half-cells. In contrast, the most concentrated copper sulfate solution (1.0 m) shows the highest potential difference between the two-half cells. However, potential difference remained constant (0.83 V)

  2. Rates of Reaction Lab

    Place the 0.2g of zinc dust in the conical flask. 6. Using a 100 ml measuring cylinder, measure out 20 ml of 1M hydrochloric acid. 7. Pour the 20 ml of hydrochloric acid into the conical flask with zinc dust and re-insert the stopper immediately.

  1. Dissolving and Energy Changing

    Secondly, instruments hygiene; we must clean thermometer with water and dry it off with tissues to avoid other solutions to be contaminated and clean the instruments afterward with clean brush and soaps to avoid serious damage. Conclusion: This experiment thought us more about exothermic and endothermic reaction.

  2. Reaction Rate

    Total volume of H2SO4 solution per trial (mL) Mass of Mg ribbons added to reaction each trial (g) Amount of Hydrogen gas produced per trial (mL) 0.5 10 0.05 20 Average time taken by reaction to produce 20mL of H2 gas =T1+T2+T3 3 1 10 0.05 20 1.5 10 0.05 20 2 10 0.05 20 Method: 1.

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