Chapter 8 Flashcards
Thermodynamics
-thermochemistry
The study of energy and temperature changes
- energy changes in chemical reactions
Energy is:
the ability to do work
Forms of energy:
- Potential energy:
- Kinetic energy
- stored energy
- energy of motion
Types of energy changes:
- Heat:
- Work:
- the transfer of kinetic energy
- the transfer of energy from one form to another
1000 calories=
1 kcal = 1 Calorie
1 calorie (c) =
4.184 J
Change in energy:
ΔE = q+w (Total energy released = sum of heat (q) and work (w)
Exothermic change
releases energy (sometimes depicted as +energy on the R side of a chemical equation) releases heat energy: -q system does work on surroundings: -w
Endothermic change
Absorbs change (sometimes depicted as +energy on the L side of a chemical equation) absorbs heat energy: +q surroundings does work on system: +w
In thermochemistry:
- The System:
- the surroundings:
- is the part of the universe being studied
- the rest of the universe
The law of conservation of energy
Energy cannot be created or destroyed
ΔE system = -ΔE surroundings
Heat energy and temperature
Heat: the t o t a l kinetic energy transferred from one object to another
Temperature: the a v e r a g e kinetic energy of the particles in a substance
Specific heat
the relationship between heat mass and temp
the amount of heat required to raise the temperature of one gram of material by 1*C
Equation for specific heat
specific heat = (heat)/ ((mass)x(change in temperature))
s=q/mΔT
q=msΔT
Heat capacity, C
the amount of heat required to raise a substance by 1*C