Thermochemistry and Thermodynamics. Energy Ability to do work or produce heat.
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Transcript of Thermochemistry and Thermodynamics. Energy Ability to do work or produce heat.
Energy
Kinetic Energy • Energy in motion
Potential Energy • Due to the composition or
position of an object
Law of Conservation of Energy
• Energy cannot be created or destroyed, only converted from one form to another
Let’s talk terminology.
• System: part of a system that a chemist chooses to study
• Surroundings: the rest of the universe
Ice and water = System
Beaker, air, and everything else= surroundings
A system can interact with its surroundings.
Let’s talk terminology.
• Energy transfers involve transfers of heat and/or work.
• Internal Energy (E): total energy within a system
Thermal energy: energy associated with random molecular motions
Chemical Energy: energy associated with the bonds and intermoleuclar attractions
Let’s talk terminology.
• Since energy and work are so closely related, we use the same unit to measure both.
• Joule (J)
• Calorie (cal): 1 cal = 4.186 J
Heat
• The energy transferred between a system and its surroundings as a result of temperature difference
• Symbol: q
Heat Capacity
• The amount of heat needed to increase the temperature of n object exactly 1°C
• Depends on mass and chemical composition
Specific Heat
• Amount of heat required to raise the temperature of 1 g of that substance by 1°C
Page 559
Calorimetry Problems
q = cp m ΔTcq = amount of heat/energy transferred (Joules)
m = mass of the substance (grams)ΔTc = temperature change of the substance
Tfinal – Tinitial
cp= specific heat of the substance
• How much heat is needed to raise the temperature of 20.0 grams of liquid water from 5 °C to 20 °C?
• How much heat is released by 200.0 grams of a solid aluminum as it cools from 200.0 °C to 150.0 °C?