Thermodynamics

There are many definitions of thermal comfort, which depends on the aims and expectations of those who defined it (Chappells, and Shove, 2004). Jiao (2010) stated that, the rate at which human body gain and lose energy, and also the state of comfort is satisfactory once all heat flow in and out of the body are in equilibrium. Also, (ASHRAE 2004), described it as “the state of mind that expresses satisfaction with the surrounding environment.” This definition highlights subjective and…

Lattice Dynamics 2.1 Introduction The discussion has been done in chapter1 about the nature crystal structure of Silicon Carbide and its properties was under the equilibrium condition, which means the location of each atom is restricted at its lattice site. The vibration of atoms about their equilibrium sites will be considered in this chapter. The fundamental reason of this vibration is thermal and the lowest achievable energy (i.e. zero-point energy). The forces acting on atoms tend to always…

The theoretical concepts that underlie the Hot Ice experiment involve a supercooled, supersaturated aqueous solution becoming a solid. When a liquid is cooled beyond its freezing point but remains liquid is known as supercooling or undercooling, and being supersaturated occurs when the solutes in a solution exceed the saturation point. The sodium acetate in a supercooled state will rapidly change into a solid with the addition of physical energy or a nucleation site. During the transformation of…

In order to understand this experiment we will investigate key components of it. First, we will explore the history of a basketball. By knowing its history, we will have an exceptional grasp on, of how basketball has evolved over time. Afterwards we will learn about different types of basketballs and their exterior and interior materials. By being familiar with this we can predict what is propelling to happen in the experiment. Third, we will investigate Charles Law. This will aid us to…

The purpose of this experiment has been met and all heat changes in each part of the experiment were measured. In Part I we had to calculate the specific heat (SH) and the atomic mass of a metal. In this case, Copper was examined and the specific heat of Copper was calculated to be 0.262 J/g℃, even though the actual specific heat is 0.387 J/g℃. The percent error of that calculation is 32.299%. A considerable reason for this error is inaccurately reading the thermometer to the tenth degree digit…

Part 1: Test of Melting Point Generally, ionic solids have very high melting point temperatures. Covalent molecules have a lower melting point. Polar covalent molecules have a higher melting point than non-polar covalent molecules. 1. Mold an aluminum foil boat that will serve as a tray for the table salt, sugar, wax. 2. At different corners of the boat place a very small amount of each substance. a. Table Salt b. Sugar c. Wax 3. Set the hot plate on high. 4. Observe and record the order…

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1. Fill a mason jar half-full with tepid water. Put it on the hotplate and raise the temperature to 98 degrees. Make sure you can keep it at this temperature for several hours. 2. Wash your hands. Cover the surfaces adjacent to your kitchen stove with paper towels. Place the test tube racks close to the stove on the paper towels. 3. Fill the pot with water and bring to a boil. Uncap your test tubes. Using your kitchen tongs, carefully drop your graduated cylinder, test tubes and their caps in…

Brandon Thai 5/17/17 Freezing Point Depression Abstract The freezing temperature of pure Cyclohexane and a solution of Biphenyl and Cyclohexane was determined. This was done by examining the temperature curves for each solution. The freezing temperature for pure cyclohexane was determined to be 7.3 degrees celsius and the mixture of Biphenyl and Cyclohexane was 2.07 degrees celsius. Introduction The purpose of this experiment is to determine the freezing point for pure cyclohexane and a…

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…