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Unformatted text preview: Thermochemistry Jabiz Behzadpour, Davin Anaya, and Michael Dean Lab Section 414 7:30 AM Thursday Mekala Pansalawatta 10/4/2007 Introduction: All of the chemical reactions that exist involve the exchange of energy. That exchange will either cause heat to be absorbed or released. When heat is released the reaction is referred to be exergonic, while when the heat is absorbed the reaction is endergonic. This experiment will involve calculating the amount of heat absorbed or released by using values obtained through experimentation. The equation utilized for this is q=ms t where q stands for the amount of heat that is absorbed or released, m stands for the mass of the sample, s is the specific heat of the sample, and the change in temperature is represented by t. When a base is neutralized by an acid, it releases energy which may be measured by that equation. It is important to calculate the heat given off during reactions because that information tells the researcher the potential energy of the two compounds, which is used in the pharmacy industry when creating new medications by combining various compounds. Experiment: Required Equipment 1.0 M NaOH 1.0 M HCl Autopipetter 1.0 M HC 2 H 3 O 2 Distilled water Calorimeter Split up into five different teams, and each team will examine a different combination of NaOH, HCl, and H 2 O when reacted. Team 1: 25 mL NaOH, 15 mL HCl, 20 mL H 2 O; Team 2: 25 mL NaOH, 20 mL HCl, 15 mL H 2 O; Team 3: 25 mL NaOH, 25 mL HCl, 10 mL H 2 O; Team 4: 25 mL NaOH, 30 mL HCl, 5 mL H 2 O; Team 5: 25 mL NaOH, 35 mL HCl, 0 mL H 2 O. Compute the following results for each team: moles of NaOH, moles of HCl, ratio of NaOH:HCl, change in temperature, q rxn , and the result of the pH indicator. You may do this by adding the ingredients together. At the end, add a drop of indicator to the beaker and gently swirl the reaction to observe if it changes color or not. The pH indicator will remain colorless in acidic solutions but turn bright pink in basic solutions....
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