Calorimeter Temperature Reaction

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Introduction The purpose of this experiment was to investigate the relationship between thermal energy and chemical reactions. A calorimeter is a metal container that is insulated for the purpose of conservation during a chemical process. In the calorimeter, a stirring rod and a thermometer place to keep track of the heat changes occurring during the experiment. Calorimetry was used in the experiments to measure the absorbed heat in a chemical process. This method of calorimetric measurement is good for conserving heat due to the energy transference from the liquid placed in the calorimeter to the calorimeter itself. The law of conservation of energy states that the amount of heat lost equals the amount of heat gained in a well insulated environment. …show more content…

The temperature the calorimeter actually went down when the KCl began to dissolve. The calculated specific heat of solution for the KCl solution was 4.19j/gc, the heat of the calorimeter was .8 degrees celsius, and the total heat was 524.84j. After finding the moles of salt in the KCl solution, calculations showed that the molar heat of the solution was -5301.42j/mol. There are many factors that indicate that this reaction is endothermic. The first indicator of this reaction being endothermic was the fact that the final temperature did not stray from the initial temperature. A low constant from the calorimeter can indicate an endothermic reaction as mentioned in the introduction because the calorimeter absorbs heat. There was more heat lost in this experiment than there was cold …show more content…

The calorimeter constant is the base of all math used within this experiment. The constant is needed to calculate temperature change which is needed for the heat change formula. If the calorimeter constant is missing or incorrect, it would throw the entire experiment off. The temperature change is also a very important factor in the experiment because it is need to calculate the heat change. The temperature change can also be an indication of an endothermic or exothermic

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