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# Calculating the temperature of a Blue Bunsen Burner Flame

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Introduction

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.

Middle

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.

Conclusion

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.

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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

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