Research Paper On Thermodynamics

In this experiment you will observe some physical and some chemical changes. You will observe that energy must be used to start some chemical reactions, and that it is produced in others.

Objective : To demonstrate the differences between physical and chemical changes while observing the laws of conservation of matter and energy.

The law of thermodynamics in can predict the direction of chemical reactions and changes in substances

In part I, the ΔH of each individual reaction was obtained by performing each reaction inside a calorimeter. Temperature probes were inserted in the calorimeter and ΔT was measured. By using the equation q = Msol’n x Cp x ΔT + Ccal x ΔT, the heat absorbed by the surroundings, q, was obtained for each reaction. The negatives of these values, or heat released by the

The study of Entropy is the study of the amounts of this energy being dispersed in a given process at a certain temperature. Although this is a founding law of nature, life does not rise from nature through entropy but through the blocking of entropy. While each particle carrying a potential amount of energy will unload that energy and spread it to as many other less energetic particles as possible, systems work to use the energy by creating boundaries and walls, both physical and chemical. (10)

The most challenging concept that I’ve learned in Chemistry is thermochemistry. This is a branch of thermodynamics

Chang, R. (2010). Chemistry. 10th ed. 1221 Avenue of the Americans, New York: McGraw- Hill Companies, Inc.

This report discusses how varying the mole ratio of the reactants affects the amount of the product that is produced and the amount of the reactants that remain at the end of the chemical reaction. We know that you can’t simply add another atom of nitrogen and take an atom of hydrogen away from ammonia because it would change to another substance. We also know that in a chemical reaction atoms cannot be created or destroyed but can make a new substance. A guiding question was made so they can figure out how to solve/find out what is going on. The atomic theory is connected to this lab because that the atoms in the lab cannot be created of destroyed during a chemical reaction. Meaning that each side the of the equation must include the same number of each type of atom. The relationship between the amounts of any two compounds, in moles, that are involved in a chemical reaction. In this lab we are showing how different ratios of moles of sodium bicarbonate and acetic acid and how the different moles leave and percentage out of the product but still remains in the lab. How this lab works we will combine sodium bicarbonate and acetic acid and we are see the amount of CO2 leftover after the reaction happens. Knowing this.

The theoretical molar enthalpy was calculated by using Hess’ Law of Summation. The theoretical values of the standard molar enthalpy of formation, also known as delta H not of formation, were taken from the product side of the net ionic equation and added up; the delta H not of formation values for the reactants were also added up. Following Hess’s Law of Summation, the change in enthalpy per mole of reaction, delta H not of reaction, is equal to that of the total delta H not of formation reactants subtracted from the total delta H not of formation of the products, to calculate the theoretical molar enthalpy of reaction.

As told at the beginning of this lab report, our aim of this experiment was to test the validity of Hess’s law which suggests that the enthalpy change of a reaction must be equal to the sum of the enthalpy changes of the other reactions that relate to the original reaction. Our result achieved from this experiment is the simple proof of Hess’s Law’s validity.

Introduction: The theory behind this experiment is the heat of a reaction (∆E) plus the work (W) done by a reaction is equal to

Purpose: To measure the heats of reaction for three related exothermic reactions and to verify Hess’s Law of Heat Summation.

The Hypothesis was proven partially correct by the experiment. As the hypothesis stated, when the temperature was increased, the efficiency of the catalysed reaction decreased. This was due to the denaturing of the active site of the protein. However,

Purpose: This lab taught procedures for determining heat of capacity of a calorimeter and measuring enthalpy of change for three reactions. It also enforced methods of analyzing data obtained through experimentation and calculating enthalpy. These procedures are used in the branch of thermodynamics known as thermochemistry which is the study of energy changes that accompany chemical reactions. Concepts from this lab can be used to determine the potential energy of a chemical reaction. Much of the energy people depend on comes from chemical reactions. For example, energy can be obtained by burning fuel, metabolizing of food or discharging a batter.

Introduction: Every chemical change is accompanied by a change in energy usually in the form of heat. If heat is evolved, the reaction is exothermic, and if heat is absorbed, the reaction is endothermic. The energy change of a reaction that occurs at constant pressure is called the heat of reaction or the enthalpy of reaction (ΔHr). This quantity of heat is measured experimentally by allowing the reaction to occur in a calorimeter. In this experiment you will determine the heat of neutralization when an acid and a base react to form 1 mole of water. In a perfect calorimeter, heat is exchanged only between the reaction and the calorimeters water. Technically, some heat may may be absorbed the calorimeter. All calorimeters exchange some heat with its environment. This amount of heat is called the calorimeters heat capacity (the amount of of heat required to raise its temperature 1∘Celsius). We are going to “pretend” that our calorimeter is the perfect calorimeter.