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The specific heat capacity of lead.

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Eirik Hjerten�s 04.02.04 The specific heat capacity of lead Introduction: Our aim in this experiment was to determine the heat capacity of lead. We would use the know heat capacity of water and lower a hot ball of lead into a calorimeter with water and measure all the needed temperatures and masses and put them into the equation: Q=C x M x ?t And the principle Heat lost= heat gained (for an isolated system) We know that the literature value is 130 J kg-1�C-1 so if the experiment is carried out properly, I think we will get a value in the proximity of that. However, experiments like this are know to have great uncertainties due to heat loss or gain from the surroundings. Equipment: * Electric cooker * Lead ball * Casserole * Calorimeter * Thermometer * Balance Procedure: First we put a casserole with water on the electric cooker. ...read more.


However, since we will convert the mass to kg in the calculations the uncertainty will be immensely small so we will not consider it. Weights Calorimeter 39 g Calorimeter w/water 132 g Water in calorimeter 132 g - 39 g = 93 g Lead ball 199 g Temperatures Boiling Water 99�C +/- 1�C Lead ball before heating (same as room temperature) 20�C +/- 1�C Lead ball after heating (same as water) 99�C +/- 1�C ?T in lead ball during heating ?Tmin= 98�C - 21�C= 77�C ?Tmax= 100�C - 19�C= 81�C ?T = 99�C - 20�C= 79�C +/- 2�C Water in calorimeter Before placing the lead ball in it 14�C +/- 1�C When thermal equilibrium achieved 20�C +/- 1�C ?T in the closed system ?Tmin= 19�C - 15�C= 4�C ?Tmaz= 21�C - 13�C= 8�C ?T = 20�C - 14�C = 6�C +/- 2�C Calculations: The heat required to increase the temperature in the calorimeter: H = mw x cw x ?T + mal x cal x ?T Hmin = 0.093 ...read more.


The only way to escape this source of error with our available equipment would be to isolate the closed system better. If we had available resources it might have been possible to create a close room where we could place the calorimeter. We could have a digital thermometer in the calorimeter that was connected to a very powerful fan that automatically increased of decreased the temperature in the room to the same as in the calorimeter. This is only an idea and I doubt it would be possible to do this at school. Another thing about this experiment is that we get a too high uncertainty in the temperature. This played an especially large part in the change in temperature in the calorimeter. The percentage uncertainty was as high as 33 %. If this had been smaller, we could have had a drastically smaller uncertainty in the answer. It would be possible to do this by simply using an electronic thermometer. ...read more.

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