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Thermochemistry - Thermochemistry Group Participants Jason...

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Thermochemistry Group Participants: Jason Christian , Connor Dennis, Josh Istas Section Number: 416 Meeting Time: 7:30-10:20 September 28, 2006 TA: Amanda Reeves Introduction When reactions occur, energy either remains constant, is given off, or is absorbed. A reaction that gives off energy is called an exothermic reaction. A reaction that absorbs energy is an endothermic reaction. In this experiment, energy is transferred as heat and measured in a calorimeter. If mass, specific heat – heat gained or lost when one gram of substance changes 1°C– and change in temperature, heat energy gained or released can be measured. In this experiment, specific heat of water is used, 4.184 J/(g°C), since the solutions used are made up mostly of water. Liter moles Molarity M H H H e Temperatur in Change t Heat Specific s mass m t ms H Absorbed Heat or leased Heat H q Absorbed Heat or leased Heat q Dissolving tion neutraliza Celsius C g J grams = = + = = = = = = = = ° × _ _ _ _ _ _ Re _ _ _ _ Re _ )) /( ( Experimental Experiment Part 1 First, the calorimeter is set up with a stand, two Styrofoam cups, a clamp, and a temperature probe. Next, 35.0 mL of 1.0 M HCL is placed in the calorimeter. The temperature of the solution in the calorimeter is measured. Then, 25.0 mL of 1.0 M NaOH is added. While swirling the solution gently, the temperature change is measured with Logger Pro. The amount of moles of each solution is recorded to find the ratio of NaOH to HCL. Next, heat is calculated. The data found is written on the board with data from other groups.
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Experiment Part 2A First, 25.0 mL of 1.0 M HCl is added to the calorimeter and the temperature is being recorded with Logger Pro. Next, 25.0 mL of 1.0 M NaOH and 10.0 mL of distilled water are added to the calorimeter. When the temperature stops changing, the maximum and minimum temperatures are recorded. The change in heat is calculated.
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