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Thermochemistry
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• Do Now – Check and edit prelabs
• Objective – Thermochemistry • Exothermic, endothermic, calorie, joule, heat
capacity, and specific heat
• Homework – Pg 510 # 9-11
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Energy Transformations
Energy is the capacity to do work or supply heat
Energy has no mass or volume
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Energy Transformations
Energy is the capacity to do work or supply heat
Energy has no mass or volume
Thermochemistry = study of energy changes that occur during chemical reactions
Heat (q) always flow from warmer to cooler
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Exothermic and Endothermic Processes
System and Surroundings
Law of conservation of energy
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Exothermic and Endothermic Processes
System and Surroundings
Law of conservation of energy
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Exothermic and Endothermic Processes
Endothermic Reactions – System absorbs energy from surroundings
Exothermic Reactions- System gives off energy to the surroundings
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Units of Measuring Heat Flow
calorie = amount of heat it takes to raise the temp of 1 g of water 1 °C
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Units of Measuring Heat Flow
calorie = amount of heat it takes to raise the temp of 1 g of water 1 °C
1 Calorie = 1 Kilocalorie = 1000 calories
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Units of Measuring Heat Flow
calorie = amount of heat it takes to raise the temp of 1 g of water 1 °C
1 Calorie = 1 Kilocalorie = 1000 calories
Joule (J) is the SI unit for measuring energy1 J = 0.2390 cal 4.184 J = 1 cal
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Heat Capacity and Specific Heat (C)
Heat Capacity = amount of heat needed to increase the temp of an object 1 °C
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Heat Capacity and Specific Heat (C)
Heat Capacity = amount of heat needed to increase the temp of an object 1 °C
Specific Heat = amount of heat needed to increase the temp of 1 gram of a material 1 °C
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Heat Capacity and Specific Heat (C)
C = q = heat (Joules or calories)__ m x ∆T mass(g) x change in temp (°C )
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Calculating the Specific Heat of a Metal
C = q = heat (Joules or calories)__ m x ∆T mass(g) x change in temp (°C ) Sample Problem 17.1 pg 510
The temperature of a 95.4 gram piece of copper increases from 25.0 °C to 48.0 °C when the copper absorbs 849 J of heat. What is the specific heat of copper?
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Calculating the Specific Heat of a Metal
C = q = heat (Joules or calories)__ m x ∆T mass(g) x change in temp (°C ) Sample Problem 17.1 pg 510
The temperature of a 95.4 gram piece of copper increases from 25.0 °C to 48.0 °C when the copper absorbs 849 J of heat. What is the specific heat of copper?
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Enthalpy
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EnthalpyHeat content of a system at constant pressure
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Enthalpy
qsys
= ∆H = -qsurr
= -m x C X ∆T
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17.1
9. 1.76 x 103 cal 1.76 kcal 7.36 x 103 J 7.36 kJ
10. 2.36 x 10-1 J/(g*°C)
11. 2.8 x 102 kJ
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17.2
18. 2Mg(s) + O2(g) → 2MgO(s) + 1204 kJ or
2Mg(s) + O2(g) → 2MgO(s) ∆H= -1204 kJ
19. 3.72 x 102 kJ
20. Heat of combustion is the heat of reaction for the complete burning of one mole of a substance.