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

Calculating the temperature of a Blue Bunsen Burner Flame

Extracts from this document...


Ali Dakik Physics Lab Calculating the temperature of a Blue Bunsen Burner Flame Date of Lab: 20 September 2005 Aim: To calculate the temperature of a Blue Bunsen Burner Flame using the concept of thermal heat transferred from one material to another. In this case, we will use the heat gained by a copper coin when burned by the Bunsen burner to calculate the flame's temperature. Background information: The temperature of the Bunsen burner is expected to be around 600-800 ?C. Thus, we cannot use a normal mercury thermometer to measure the Flame's temperature directly. This is because the maximum range of a mercury thermometer is 100?C. As a result, we have to find the flame's temperature using other methods. Materials Needed: * A steel Calorimeter * A 250 cm� beaker * A mercury thermometer * Mass balance * A small copper coin * A heating water kettle * A Bunsen Burner Method: 1) ...read more.


Data Collection: 1) To find the heat capacity of steel (Calorimeter), the following data was obtained: Initial Temperature of water at room temperature (Before heating): 25.6?C Mass of steel Calorimeter: 42.87g=0.04284 kg Mass of water: 92.34 g=0.09234 kg Final Temperature of water (After heating): 77?C Final Temperature of Water and Calorimeter: 66?C Temperature Drop: 10?C 2) Finding the temperature increase when the heated copper coin is put in water: Number of trials Mass of water m/g Mass of Copper m/g Initial Temp. of Calorimeter and water T/?C �0.1 Final Temp. of Calorimeter and water T/?C �0.1 Temperature increase T/?C �0.1 1st trial 137.36 4.60 17.8 19.0 1.20 2nd trial 137.36 4.60 21.1 22.7 1.60 3rd trial 137.36 4.60 25.1 26.6 1.50 Average Temperature Increase 1.43 Data Processing and Presentation: 1) Finding the exact heat capacity of Steel (Calorimeter): We assume that no heat is lost to surroundings. The Law of conservation of energy states that: "Energy is neither lost not created. ...read more.


This obtained value is reasonable, and although not very exact, it is satisfactory. We have assumed that heat is not lost to surroundings, and thus, the temperature is realistic. However, the real value should be between 600 to 700 ?C. Improving the Experiment: * For values of Specific heat capacity of water and copper, we used the Physics Data Book. However, these values vary according to pressure, density...etc. Thus, they were not exact. Instead, we should next time calculate them in the same way we found the specific heat capacity of steel. * We did not measure the initial temperature of copper and assumed it is at room temperature. Next time, we should calculate the exact temp. Of the copper. * We did not heat the copper coin for the same period of time. This means that the copper coin reached a different temperature each time. Next experiment, we should heat the copper coin for a same given time. ...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

Here's what a teacher thought of this essay

4 star(s)

A well described experiment with clearly set out calculations. In places a little more attention to detail would have been helpful.

Marked by teacher Adam Roberts 14/10/2013

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. A Colorimetric Determination of Manganese In Steel

    0.2g of the paper clip was weighed out and then transferred to a 250cm3 glass beaker. About 40cm3 of 2mol/l nitric acid was added to the beaker before the beaker was covered with a clock glass and gently heated in a fume cupboard.

  2. Determining the iron content in a sample of steel wool.

    Sources of error in the procedure could either be systematic or random. For example, there might be errors on the burette, graduated pipette and the volumetric flask scales. The error is one half of the smallest unit on the scale, which is cm3.

  1. Investigate how the solubility of Potassium Nitrate is affected by Temperature.

    is as I have written before, the reaction needs Activation energy and this energy is taken away from the warm water particles as heat energy and then, when the particles collide with KNO3 ions this is

  2. Indirect determination of enthalpy change of decomposition of sodium hydrogen carbonate by thermochemical measurement ...

    These temperatures cannot be measured directly, but they can be inferred by extrapolating the baselines to obtain the temperatures on the initial and final baselines at the time the reaction was initiated. In this way, we obtain ?T for both reactions.

  1. The aim of this experiment is to answer the following question: What is the ...

    Therefore when I am transferring the chemical from the sealed jar to the burette, I will ensure that safety goggles are on; so that any spillage will not come into contact with the eyes. I will also ensure that I am using a funnel on the burette.

  2. Analysing the ethanoic acid concentration in different types of vinegars.

    Cider Vinegar: Titration No. 1 2 3 Start position 28.8 35.6 42.6 Final position 35.6 42.6 49.8 NaOH used 6.8 7.0 7.2 Average NaOH used = (6.8 + 7.0 + 7.2) = 7.0cm3 [Ethanoic acid] in vinegar sample = 0.7 mol/dm3 pH metering I took 3 readings for the pHs of the distillates and took an average.

  1. Investigation to find out the factors affecting heat of neutralisation, and then choosing one ...

    - (60 * 4.2 * 5.6 /1000 / 0.03) 2. - (60 * 4.2 * 5.5 / 1000/ 0.03) 3. - (60 * 4.2 * 5.5 / 1000/ 0.03) =1. -47.0 KJmol-1 2. -46.2 KJmol-1 3. -46.2 KJmol-1 To find an average of these figures: - (47.0 + 46.2 + 46.2)

  2. AIM: To study the effect of solid impurities on boiling point of water and ...

    Prepare a NaCl solution by mixing 5.5g of NaCl in 50 ml water in a beaker. 1. When the NaCl gets dissolved in water heat the above solution on a Bunsen burner with a wire mesh and thermometer inserted in it till the solution starts boiling observing the temperature every 10 seconds 1.

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