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46 Cards in this Set
- Front
- Back
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Ek=
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Ek = (1/2)mv2
energy of motion |
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kinetic energy
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energy of motion
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energy
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capacity to supply heat or do work
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Potential energy
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Ep - energy based on position
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thermodynamics
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the study of energy and its transformation
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thermochemistry
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(a subset of thermodynamics - the study of heat flow in chemical reactions
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potential energy
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stored energy; energy due to position
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Joule
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1 J = (1kg*m2)/s2
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1 cal
also how many J in a cal |
1cal = 4.184 J exactly
amount of heat required to raise the temperature of 1.0 g of water by 1 degree C |
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dietary calorie
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C, 1000c so it's the amount of energy to raise 1000 g of water 1 degree C
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heat
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flow of energy from a body at higher temperature to one at a lower temperature when the 2 bodies are in thermal contact
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temperature
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a measure of thermal energy, measure of the kinetic energy of molecular motion
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heat vs temperature
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Ex 1g H2O (l) 100 degree C
vs 1 g H2O (g) 100 degree C gas has way more heat |
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work
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force applied over a distance or
W= F*d |
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work of expanding gases
and what is it sometimes called |
w = -PΔv ...
sometimes called PV work |
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w
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w = F*d
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P
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P = F/A
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F
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F = P*A
where P = pressure |
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w defined as what when substitutions done
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w = P*A*d
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under constant P, w =
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w = -PΔv
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internal energy
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E, sum total of all potential kinetic energies of all the particles in the system
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system
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that part of the universe that we single out to study
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surroundings
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everything else besides the system in the universe... mainly the stuff around like table, air in room, etc.
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First Law of Thermodynamics
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1. energy can be converted from one form to another but it cannot be created or destroyed
2. law of cons of energy 3. energy lost by the system must equal the energy gained by surrounds 4. total energy of an isolated system is constant (law of conservation of mass-energy from e = mc2 from Einstein) |
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ΔE is equal to what
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ΔE = q+w
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ΔE conceptually
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change in internal energy of the system
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ΔE described in before/after
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Δ = Efinal - Einitial
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q
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heat
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w
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work
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Delta means
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final minus initial
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The sign is determined from the point of view of the ____
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system
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if q is positive then
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q --> [system] heat flows into the system from surroundings
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if q is negative then
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[system] --> q heat from the system into the surroundings
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if w is positive, then
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w --> [system] the surroundings are doing work on the system
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if w is negative, then
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[system] --> w the system does work on surroundings
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state function
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a function or property whose value depends only on the present state or condition of the system not on the path used to arrive at that state
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qsubv indicates what
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heat transfer occurring at a constant volume
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ΔH is called what and equals what?
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enthalpy of a system
ΔH = ΔE + PΔV |
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enthalpy of fusion
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the amount of heat necessary to melt a substance without changing its temperature
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the amount of heat necessary to melt a substance without changing its temperature is called what?
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enthalpy of fusion
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enthalpy of vaporization
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amount of heat required to vaporize a substance without changing its temperature
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amount of heat required to vaporize a substance without changing its temperature is what?
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enthalpy of vaporization
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sublimation
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straight from solid to gas; such as dry ice solid CO2
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heat capacity
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C = q/ΔT
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Hess's law
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The overall enthalpy change for a reaction is equal to the sum of the enthalpy changes for the individual steps in the reactions
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standard heat of formation
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the enthalpy change ΔH°f for the formation of 1 mol of a substance in its standard state from its constituent elements in their standard states
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