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Heat of Combustion Lab

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Introduction

Determining the heat of combustion 11IB chemistry HL Raw Data -Wax Initial mass of wax �0.01g 12.53g Final mass of wax �0.01g 11.86g Initial temperature of water �0.1�C 10.8�C Final temperature of water �0.1�C 35.5�C Volume of cold water �0.5ml 200ml -Ethanol Initial mass of Ethanol �0.01g 161.15g Final mass of Ethanol �0.01g 160.28g Initial temperature of water �0.1�C 10.1�C Final temperature of water �0.1�C 35.1�C Volume of cold water �0.5ml 200ml -Butanol Initial mass of Butanol �0.01g 227.49g Final mass of Butanol �0.01g 226.62g Initial temperature of water �0.1�C 10.4�C Final temperature of water �0.1�C 36.9�C Volume of cold water �0.5ml 200ml Data processing -Wax (C25H52) Change in temperature (?T) �0.2�C(�0.1�0.1) �0.81%(�0.2/24.7*100) Tf-Ti 35.5�C -10.8�C = 24.7�C Total mass of wax was burned �0.02g(�0.01�0.01) �2.99%(�0.02/0.67*100) 12.53g-11.86g = 0.67g Changing energy �0.21(�0.2�0.01) �0.10%(�0.21/20.6*100) Q=cm?T =200g*4.18J/g�C*24.7�C =20.6KJ ?H comb �0.10%�2.99% =�3.09% 0.0309*10827.9 =�334.6 ?H comb =Q/mass of burned wax*molar mass =20.6KJ/0.67g =30.7KJ/g 30.7KJ/g*352.7g/mol =10827.9KJ/mol -Ethanol (C2H6O) ...read more.

Middle

If we just heated it in normal temperature such as 20�C, we couldn't see the changes of temperature well, and it could take more time to heat it. We also measure the changes of mass of material to see how much we burned. We put some ice in the water to make the initial temperature of water as lower than 10�C. When the temperature decreased up to 10�C, we took out ice from the water. After we took out the ice and fill the cylinder up to 200ml of water, the temperature was higher than 10�C because the temperature of the water changed very quickly. We measured the temperature of water and then we hang the tin can on the hanger, so the temperature might increased again during we set up all the experiment systems. So we should measure the temperature of water when we set up all the things. For example we should measure it after we turn the light on the candle wax and hang the tin can on the hanger. ...read more.

Conclusion

So they are burned and evaporated more after we measure the temperature. Another fact that we should consider is that not only the water was being heated, but also the thermometer, stirring rod and the tin can were also being heated. We should consider that they were also heated, so we should measure how much heat were used to heat them. Also some other heat would have been lost round the sides of the tin can, and from the water to the atmosphere. Due to our room temperature are different from the temperature of water. The good thing that we did in our experiment is that we made some space when we set up the large metal can to surround the candle. As we make some space under the large can by putting some flat cylinder under the can, the candle burned more quickly and well. If we didn't make the space for it, air might stuck in there so it would take more time to reaches up to 35�C. ?? ?? ?? ?? ...read more.

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