Thermodynamics Of Borax LAB REPORT

The credentials are Mr. Kent’s Chemistry Page: Endothermic and Exothermic Process and Bozeman Science: Endothermic and Exothermic Reactions. The Bozeman Science: Endothermic and Exothermic Reaction was created in 25 September 2013, however, the other source doesn’t have a written date on the website. This source is reliable, because the author is a teacher has studied for many years and she had evidence to back up.

The mixture was heated at 120°C using an aluminum block and was stirred gently. After all of the solid dissolved, it was heated for 20 additional minutes to ensure the reaction was complete.

Is this reaction endothermic or exothermic? What does that mean and how do you know? (~3 sentences)

11. The experiment was repeated three more times using different water temperatures (room temp water, cold temp water, hot temp water).

Once 5 trials have been completed, continue and repeat steps 1-6 for the other temperatures (15oC, 25oC, 35oC & 45oC).

Substance A and B were weighed; Substance A weighed 0.502 g and substance B weighed 0.503 g. Both substances were put into two different test tube with approximately 8 ml of DI water into the test tub. Substance A and B were stirred and B dissolved while A did not. This shows that B is soluble in water compared to A. Thus, shows that B is soluble in water than A. The reason why B is soluble in water is because it has a higher dipole moment than A. With a higher dipole moment, it shows that it is soluble in water since it is polar and the bonds were easily broken.

AP Chemistry Background The solubility product constant, Ksp, is a particular type of equilibrium constant. The equilibrium is formed when an ionic solid dissolves in water to form a saturated solution. The equilibrium exists between the aqueous ions and the undissolved solid. A saturated solution contains the maximum concentration of ions of the substance that can dissolve at the solutions temperature. A knowledge of the Ksp of a salt is useful, since it allows us to determine the concentration of ions of the compound in a saturated solution. This allows us to control a solution so that precipitation of a compound will not occur, or to find the concentration needed to cause a precipitate to form. The solubility product which will be

In this unit we have conducted research and experiments on our chosen reactions to create the highest exothermic reaction for the The Heat-and-Eat meal pack will use a chemical reaction that involves two reactants. Reactant 1 is a solid and Reactant 2 is a liquid.

It’s predicted that when adding the chemical substance into the water, energy will be released or absorbed, this will be observed by a temperature change, therefore, there would be an exothermic or endothermic reaction.

The solid water was the control variable in the experiment and the investigators compared values that resulted from irradiation of the solid water with each bolus’ average Dmax. Table 1 recorded the ratios that resulted from these values. ANOVA calculations from the values shown in Table 1 resulted in an F value of 762.65 and a P value of less than 0.0001. The investigator compared the results between each individual group with a Tukey HSD test. When compared to one another, each sample resulted in a P value less than 0.01.

The purpose of the experiment was to determine the thermodynamic properties of changes in entropy, enthalpy and free energy, and to calculate the solubility product (Ksp) of borax. The hypothesis of this experiment was accepted, due to the titration of borax and HCl yielding the equation, y = -2932.9x + 3.1221 from the graph of ln Ksp vs. 1/ T. Furthermore, the values for ΔS˚, ΔH˚ and ΔG˚ were calculated to be -24.4 J/mol ∙K, 25.96 kJ/mol, and -32.12 J, respectively. The properties of thermodynamics (entropy, enthalpy and free energy) can be seen in terms of spontaneity. Entropy, ΔS˚, is the tendency for the universe to move towards more disorder. If entropy is negative, then the amount of disorder within a system would decrease and reactions

The styrofoam cups were used to store the acid (cup was labeled A) and base (cup was labeled B) prepare for them to be mixed. A lid was put on cup A and then the temperature probe was inserted to begin to measure the temperature

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

Empty and clean the test tubes and repeat steps 2-10 again for a second dataset.

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.