Physics : Calorimeter Lab Report

3335 Words Apr 21st, 2015 14 Pages
Konstantina Stavroulaki
Chemistry 3 Section 12
Partners: Kiley Anselmo, Meghan Freeman
Calorimeter Lab Report
Introduction
According to the first law of thermodynamics, energy can be neither destroyed nor created. Thus, the total amount of energy in the universe stays constant, and the expression of the total amount of energy is the following: ΔUtotal = 0 Eq.1
However, since it is not quite achievable to keep track of changes of energy in the universe, a possible way to make it doable is tracking the energy changes in a small portion of the universe that represents the “system”, with everything that belongs outside of it called the “surroundings”. Therefore, the total energy of the system can be expressed as the sum of energy changes in the system and the surroundings. Given that the total energy never changes, one can end up with the following equation: ΔUsystem + ΔUtsurroundings = ΔUtotal = 0 Eq.2
There are two main ways of changing the energy of a system that include either the transfer of heat (q) or the the ability to do “work”. The last one is about work being done on the system by the surroundings or the system doing work on its surroundings. There are many types of work such as chemical work, expansive work, electrostatic work, gravitational work etc. In this experiment, the change of energy because of work is negligible.…

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