thermochemistry. do now – check and edit prelabs objective – thermochemistry exothermic,...
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Thermochemistry
• Do Now – Check and edit prelabs
• Objective – Thermochemistry • Exothermic, endothermic, calorie, joule, heat
capacity, and specific heat
• Homework – Pg 510 # 9-11
Energy Transformations
Energy is the capacity to do work or supply heat
Energy has no mass or volume
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
Exothermic and Endothermic Processes
System and Surroundings
Law of conservation of energy
Exothermic and Endothermic Processes
System and Surroundings
Law of conservation of energy
Exothermic and Endothermic Processes
Endothermic Reactions – System absorbs energy from surroundings
Exothermic Reactions- System gives off energy to the surroundings
Units of Measuring Heat Flow
calorie = amount of heat it takes to raise the temp of 1 g of water 1 °C
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
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
Heat Capacity and Specific Heat (C)
Heat Capacity = amount of heat needed to increase the temp of an object 1 °C
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
Heat Capacity and Specific Heat (C)
C = q = heat (Joules or calories)__ m x ∆T mass(g) x change in temp (°C )
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?
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?
Enthalpy
EnthalpyHeat content of a system at constant pressure
Enthalpy
qsys
= ∆H = -qsurr
= -m x C X ∆T
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
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.