Lab_3

other, when one of these variables is changed, it affects at least one of the other two variables. The second law of thermodynamics states that there is a tendency in nature to move towards a state of greater molecular disorder. Entropy is a measure of disorder, solid crystals, the most structured form of matter, have very low entropy values. The more highly disorganized gases have high entropy values. The potential energy of isolated energy systems that is available to do work decreases with increasing entropy. The second law of thermodynamics states that heat can never be transferred, by its own effort, from a zone of lower temperature to another of higher temperature. Macrostates describe the behavior of an entropy system Introduction The following report will talk about the laboratory carried out on the gas laws and the importance of their respective identification. It will be analyzed, its changes and transformations, how temperature, pressure, and volume can affect the system according to the law that governs it. Various experiments indicating their changes will be discussed together with the help of high and low-temperature water containers. In addition, the probability will be studied and how entropy is present in daily life Material and Methods  Styrofoam cup  Stopwatch  Thermometer  10 ml sealable syringe and graph paper (Found in the Ideal Gas Law baggie).  Dice (Found in Second Law of Thermodynamics baggie).  Crushed ice  Pencil  Water Lab 15 Experiment 1: Charles’ Law Results/Observations Enter your data in the following table and record your observations: JWH 3 Physics II

% =|(-273+4.92) / (-273)| x 100 % = 98% In order to reduce the large percentage of the error, it is necessary to have more suitable equipment to be able to reach absolute zero. They are needed from syringes, to cooling equipment to be able to obtain a more reasonable error 7. Would it be possible to cool a real gas down to zero volume? Why or why not? What do you think would happen before that volume was reached? It would not be possible, since for very low temperatures, it is very likely that the gas will condense first into a liquid Lab 18 Experiment 2: Probability of States Results/Observations Enter your data in the following tables: Note : k is the Boltzmann constant, 1.38 x 10 -23 J/K. Prelab Question 2 - Microstate Data for 2 Dice Macrostate Possible Microstates (Dice Combinations) Number of Microstates (  ) Entropy S = k  ln(  ) 2 1 1 0 3 2 2 9.57 x 10 -24 4 3 3 1.52 x 10 -23 5 4 4 1.91 x 10 -23 6 5 5 2.22 x 10 -23 7 6 6 2.47 x 10 -23 8 5 5 2.22 x 10 -23 9 4 4 1.91 x 10 -23 10 3 3 1.52 x 10 -23 JWH 6 Physics II

JWH 9 Physics II

the type of probabilistic behavior illustrated by this example. The spontaneous change of a system goes from less possibility to greater probability, to achieve it generates greater entropy. The disorder is much more likely than in order. There is a tendency to go from low entropy to high entropy. Conclusions In this experiment I was able to come up with several conclusions, such as when the pressure increases and decreases, a kind of cycle is formed in which energy is not lost at any time and everything returns to its normal state, therefore obeying the first law of thermodynamics where it tells us about conservation of energy. Also, this experiment makes reference to the ideal gas laws in this case it refers specifically to Boyle's law in which it tells us that “the pressure exerted by a physical force is inversely proportional to the volume of a gaseous mass, as long as its temperature remains constant”, and that exactly is fulfilled in the development of the experiment. The experiment gives us a rather curious data and also important to analyze in which a small but no less important variation in temperature is noted due to the sudden decompensation that occurs when the pressure increases and decreases, it returns to room temperature due to the heat flow from the environment into the syringe. JWH 12 Physics II