Calorimeter
A team was sent to the chemical manufacturing division of a small chemical company to help the technicians with experiments. Since the notes written by the technicians were inaccurate and unfinished, all of the experiments they had preformed needed to redone and documented correctly. The head of the company gave the new team the task of trying to figure out why some chemical reactions caused the reaction vessel to get cold and others caused the vessel to get hot. The group constructed an apparatus to measure the quantity of thermal energy gained or lost during the chemical reactions± (Bellama, 193). This device was called a calorimeter. A series of different reactions were conducted using two different calorimeters. First, hot and cold water tests were preformed. Based on these results the scientists calculated the heat capacities of the calorimeter. The density and specific heat of pure water were used for these calculations. The other tests that were redone and rec!alculated were: salts in water, precipitation reactions, and acid base reactions. Then the question of whether the solution absorbed or gave off heat can be answered. Also, whether or not the concentration of an acid base reaction made a diff
Ten milliliters of sodium sulfate were measured into a graduated cylinder and added into the calorimeter. Therefore, the general trend of the results indicate that these two precipitation reactions released heat into their surroundings. 0 kJ/mol, more than the three and six molar solutions. The balanced equations of the two reactions can be seen below. The experiment itself further reinforced our interpretation of the results as both calorimeters became warmer as the reactions progressed. Therefore, according to our results, the concentration did affect the amount of heat given off by the reaction in this experiment. Equations in the lab manual were used to calculate the ∆H for each experiment. Results The results for the heat capacities of the calorimeters were determined using the hot and cold water tests. The solution was monitored, and the temperature was recorded every ten seconds until it began to decrease. As seen in Tables 4 and 5, all of the results gleaned from the weak and strong acid base experiments were negative. For our experiments, our team chose to use acetic acid and ammonium hydroxide for our weak acid and base.
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