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Specific Heat of Copper Lab

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Introduction

J. Ryan Specific Heat of a Metal Pre ? Lab: 1. (mass of water)(specific heat water)(temperature of water final - temperature of water initial)=(mass of metal)(unknown)(temperature of metal final - temperature of metal initial) 2. percentage error = (measure-actual/actual) x 100 Procedure: 1. Measure the initial temperature of the water and the and the metal and also measure the mass of both 2. Measure the mass of the beaker then fill a large beaker which is about half full of water. Place the beaker of water on the hot plate then start heating the water until it reaches boiling point 3) Record the mass of the calorimeter 4) ...read more.

Middle

Immediately pour the metal into the calorimeter cup so that the metal is covered by the water. Cover the calorimeter with its cover 9) Insert the thermometer through the small hole in the cover. Stir very slowly with a stirring rod, and record the highest temperature reached by the water. Material Mass Temperature Metal in boiling water 57.39 g ± 0.05 100.8°C± 0.05 Calorimeter 297.86g± 0.05 N/A Calorimeter + water 450.05g± 0.05 17.35°C± 0.05 Water in beaker 152.19± 0.05 100.8°C± 0.05 Water in Calorimeter after hot metal added. 507.44g± 0.05 20.2°C± 0.05 Beaker 177.23g ± 0.05 Follow-Up : X = unknown specific heat of metal (152.19 ± 0.05)(4.186)(20.2 ± 0.05 - 17.35 ± 0.05 ) ...read more.

Conclusion

Another limitation that I think was present was that when we are transferring the metal into the calorimeter the temperature of the metal might have changed a little even thought we tried to move it as quickly as possible and that could be a limitation. There are also some errors that we are not able to prevent from happening. For example, the electrical thermometer could have a different temperature and it will also change the temperature of the water because it will take some time for the temperature to stay at constant. Even though we try as hard to not have any errors human error will always be present. ...read more.

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