Enthalpy of a Reaction

Enthalpy of a Reaction - we had exothermic energy given...

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Enthalpy of a Reaction Shawn Whitcraft Group Member: Marc Whetstone
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Statement of Purpose: The purpose of this experiment is to use a calorimeter to measure the amount of energy given off by the reaction of predetermined chemicals. We determine the enthalpy change of the reaction of HCl and NaOH solutions. After measuring the enthalpy change in the first reaction, then we measure the effect of doubling the amount of each chemical in the reaction and record the results. Data Section: Sample Calculations: 1. 2.1g X 50ml (1g/1ml) X 4.18 X 2.8 = 1228.92 4.04g X 50ml (1g/1ml) X 4.18 X 4.4= 3715.184 2. 80 + .2016 X 695 X 2.8 = -156072.3136 3. Q = 100 X 4.18 X 6.8 Q= 2842.4 4. Q=200 X 4.18 X 6.6 Q=5517.6 Results and Discussion: After completing the experiment and completing the calculations, the results showed that when you combine water and ammonium nitrate you will have endothermic energy that can be measured by the decrease in the temperature of the solution. When combining HCl and NaOH,
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Unformatted text preview: we had exothermic energy given off. This is measured in the rise in the temperature of the solution. When we doubled the amount of ammonium nitrate used in the measurement we had almost had a double in the amount of endothermic energy given off. We noticed a similar result Enthalpy of Reaction Data Chemical One Amount Chemical Two Amount Beginning Temp C End Temp C Change C Test 1 water 50 ml NH 4 NO 3 2.1g 22.8 20-2.8 Test 2 water 50 ml NH 4 NO 3 4.04g 22.8 18.4-4.4 Test 3 HCl 50 ml NaOH 50 ml 22.8 29.6 6.8 Test 4 HCl 50 ml NaOH 100 ml 22.8 26.6 3.8 Test 5 HCl 100 ml NaOH 100 ml 22.8 29.4 6.6 when we doubled the volume of the base and didnt change the amount of acid. When we doubled the volumes of both the acid and the base, we had similar measurements in exothermic energy as we did before we doubled the two measured amounts of chemicals....
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Enthalpy of a Reaction - we had exothermic energy given...

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