Chapter 06 - Thermochemistry Handout II

Chapter 06 - Thermochemistry Handout II - Chapter 6...

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Chapter 6 Chapter 6 Thermochemistry: Energy Flow and Thermochemistry: Energy Flow and Chemical Change II Chemical Change II
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Experimental Determination of Energy Change in Reactions Experimental Determination of Energy Change in Reactions Calorimetry the measurement of heat energy changes in a chemical reaction. Calorimeter device which measures heat changes in calories change in temperature is used to measure the heat loss or gain. 3
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Specific heat capacity the number of calories of heat needed to raise the temperature of 1 g of the substance 1 o C. Specific heat, c s , for water is 1.0 cal/g o C it takes 1 calory of energy to heat 1 gram of water 1 o C To determine heat released or absorbed in a reaction, you need: specific heat, c s total number of grams or moles of solution, m s temperature change (increase or decrease), T s Calorimetry Calorimetry Q s = m s x T s x c s
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Calorimetry: Measuring Energy Content Calorimetry: Measuring Energy Content Specific Heat Capacity Example: specific and molar heat capacity of water specific heat capacity c H2O = 1 cal/g. o C = 4.184 J/g.K molar heat capacity C H2O = (4.184 J/g.K) x (18.02 g/mol) = 75.40 J/mol.K Specific Molar Substance Heat Capacity Water, H 2 O 4.184 (J/g.K) 75.40 (J/mol.K) Ethanol, C 2 H 5 OH 2.46 113.16 Carbon tetrachloride, CCl 4 0.862 44.39 Aluminum, Al 0.900 24.28 Graphite, C 0.711 8.53 Iron, Fe 0.450 25.13
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High specific heat capacity of water More energy required to heat water than rock (4.2 J/g.K vs. ~ 0.7 J/g.K) Energy absorbed during the day is released during the night Keeps temperatures moderate
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Question 1 . If 0.10 mol of HCl is mixed with 0.10 mol of KOH in a “coffee cup” calorimeter, the temperature of 1.50 x 10 2 g of the solution increases from 25.0 o C to 29.4 o C. If the specific heat of the solution is 1.00 cal/g o C, calculate the quantity of energy evolved in the reaction. Question 2.
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Chapter 06 - Thermochemistry Handout II - Chapter 6...

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