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Chem 162 Exam 2
Thermochemistry
The study of the changes in energy that accompany chemical reactions
Thermodynamics
Study of the relationship between heat, work, and energy
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Chemical energy
Potential energy that depends on the way atoms are bonded together
Breaking chemical bonds
Energy gets absorbed
Forming chemical bonds
Energy gets released
Internal energy (E)
the sum of the kinetic and potential energies of all particles in the system. Units in
Joules or calories
calorie vs Calories
calorie is the science equivalent and Calorie is the nutrition equivalent
Heat (q)
The transfer of energy between system and surroundings. transferred from "hot" to
"cold"
Endothermic
Reaction that absorbs heat from the surroundings (q = +)
Exothermic
Reaction that gives off heat to the surroundings (q = -)
Work (w , J)
The energy transferred when an object is moved by a force
w = -P * deltaV
When volume increases (Work question)
w=-
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When volume decreases (Work question)
w=+
The first law of thermodynamics
Energy can be transferred and transformed, but it cannot be created or destroyed.
Change in energy formula
Heat + Work (q + w)
q after endothermic rxn
q=+
q after exothermic rxn
q=-
Enthalpy
The heat content of a system at constant pressure
Melting
solid to liquid
Evaporation
Liquid to gas
Freezing
liquid to solid
Condensation
Gas to liquid
Sublimation
solid to gas
Deposition
gas to solid
Temperature (T , C or K)
The measure of the average kinetic energy of the molecules.
heat capacity (Cp)
the energy required to raise the temperature of an object by 1 degree C at constant
pressure
Specific heat capacity
The amount of energy required to raise the temperature of 1 gram of a substance by 1
degree celcius
Molar heat capacity
the energy required to raise the temperature of one mole of a substance by one degree
Celsius
kinetic energy
energy of motion
potential energy
stored energy
calorie to Joule
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Chem 162 Exam 2
Thermochemistry
The study of the changes in energy that accompany chemical reactions
Thermodynamics
Study of the relationship between heat, work, and energy
Previous
Play
Next
Rewind 10 seconds
Move forward 10 seconds
Unmute
0:02
/
0:15
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Brainpower
Read More
Chemical energy
Potential energy that depends on the way atoms are bonded together
Breaking chemical bonds
Energy gets absorbed
Forming chemical bonds
Energy gets released
Internal energy (E)
the sum of the kinetic and potential energies of all particles in the system. Units in
Joules or calories
calorie vs Calories
calorie is the science equivalent and Calorie is the nutrition equivalent
Heat (q)
The transfer of energy between system and surroundings. transferred from "hot" to
"cold"
Endothermic
Reaction that absorbs heat from the surroundings (q = +)
Exothermic
Reaction that gives off heat to the surroundings (q = -)
Work (w , J)
The energy transferred when an object is moved by a force
w = -P * deltaV
When volume increases (Work question)
w=-
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Chem 162 Test 1.pdf~~~)@(&(*&#)))))))))))))))))))))))))))))))))#&*(*&(#*^@!!!!!#~@~##
When volume decreases (Work question)
w=+
The first law of thermodynamics
Energy can be transferred and transformed, but it cannot be created or destroyed.
Change in energy formula
Heat + Work (q + w)
q after endothermic rxn
q=+
q after exothermic rxn
q=-
Enthalpy
The heat content of a system at constant pressure
Melting
solid to liquid
Evaporation
Liquid to gas
Freezing
liquid to solid
Condensation
Gas to liquid
Sublimation
solid to gas
Deposition
gas to solid
Temperature (T , C or K)
The measure of the average kinetic energy of the molecules.
heat capacity (Cp)
the energy required to raise the temperature of an object by 1 degree C at constant
pressure
Specific heat capacity
The amount of energy required to raise the temperature of 1 gram of a substance by 1
degree celcius
Molar heat capacity
the energy required to raise the temperature of one mole of a substance by one degree
Celsius
kinetic energy
energy of motion
potential energy
stored energy
calorie to Joule
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