1. For part 1, is the theoretical final temperature the same as the measured temperature? Explain any difference.
No, in part 1, the theoretical final temperature is not the same as the measured temperature. This is caused by the base assumption of the ‘Principle of Heat Exchange’, which is that the principle only holds true if heat is not lost to its surroundings. Although, the loss of heat to its environment (ex. Desk, air, cup, etc.) was attempted to be minimized by quick transfer of the water and object, and the use of a calorimeter, the data proves that there was a loss of heat as the theoretical temperature was higher than the resulting temperature.
2. For part two, compare your specific heat capacity value of the test object to other …show more content…
Name two good applications of an object with high heat capacity. Name two good applications of an object with low heat capacity.
An object with a high specific heat capacity would be a very useful material for oven gloves as a high amount of heat will only cause a small change in temperature increase, which will keep your hand burn free and the ability to touch objects in the stove without a huge increase in temperature. Another application of using an object with a high specific heat capacity would be a swimming pool, since water has a high specific heat capacity, people can enjoy being outside in the sun and remaining cool in the water as the warm radiation waves only increase the temperature of the water slightly.
An object with a low specific heat capacity would be a very useful component of a cooking instrument, such as a frying pan, as they can be quickly heated without much heat being supplied. This will then cook the food on the frying pan quickly. Another application of a low specific heat capacity object would be a thermometer, this way it will be able to detect and show change of temperature rapidly and accurately.
6. Why did you choose a certain procedure, how were you able to remain accurate and show
No, in part 1, the theoretical final temperature is not the same as the measured temperature. This is caused by the base assumption of the ‘Principle of Heat Exchange’, which is that the principle only holds true if heat is not lost to its surroundings. Although, the loss of heat to its environment (ex. Desk, air, cup, etc.) was attempted to be minimized by quick transfer of the water and object, and the use of a calorimeter, the data proves that there was a loss of heat as the theoretical temperature was higher than the resulting temperature.
2. For part two, compare your specific heat capacity value of the test object to other …show more content…
Name two good applications of an object with high heat capacity. Name two good applications of an object with low heat capacity.
An object with a high specific heat capacity would be a very useful material for oven gloves as a high amount of heat will only cause a small change in temperature increase, which will keep your hand burn free and the ability to touch objects in the stove without a huge increase in temperature. Another application of using an object with a high specific heat capacity would be a swimming pool, since water has a high specific heat capacity, people can enjoy being outside in the sun and remaining cool in the water as the warm radiation waves only increase the temperature of the water slightly.
An object with a low specific heat capacity would be a very useful component of a cooking instrument, such as a frying pan, as they can be quickly heated without much heat being supplied. This will then cook the food on the frying pan quickly. Another application of a low specific heat capacity object would be a thermometer, this way it will be able to detect and show change of temperature rapidly and accurately.
6. Why did you choose a certain procedure, how were you able to remain accurate and show