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used to develop criteria for predicting the direction of a chemical reaction
is the reaction spontaneous? occuring on it's own without added work? and Time?
Thermodynamics and Kinetics
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Study of heat and work
Thermochemistry
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energy that is transferred by system-surrounding until thermal equilibrium is established. (not state functions)
heat (q)
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energy transfer between system and surrounding but results in (w=fxd) movement.
(not state functions)
Work (w)
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the universe
surroundings
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specific part of the universe that is of interest
system
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3 types of system
open, closed and isolated
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matter and energy transfer can occur between system and surroundings
open
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only energy transfer can occur. Ex: earth
Closed
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no matter or energy transfer can occur ex. thermos bottle
q+w
isolated
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depends of the present state of the system not how it got there. (final + initial condition)
state functions
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measures the energy absorbed or released as heat in a chemical or physical change
Calorimeter
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absorbs energy
endothermic
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releases energy, system releases energy to the surrounding
exothermic
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measure of avg kinetic energy of the particles in a sample. higher the temp, molecules move faster
KE = 1/2 mv^2
Temperature
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amount of heat reqd to change temp. (intensive) always constant, the mass/ change in temp is a ratio.
heat=mass x change in temp x specific heat capactiy
(J) (g) (deg C) (J/g deg C)
specific heat capactiy (cp)
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measure of systems capactiy to take up heat (extensive property)
C=q/change in temp
Heat capacity (C)
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Law of conversion of energy. energy cannot be created nor destroyed.
qsyst + qsurr= 0
qsyst = -qsurr
First law of thermodynamics
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Energy = q+w
q>0 toward the system (endo) heat absorbed w>0= work done on the system by the surr.
q<0 away from the system (exo) heat released w<0= work done by the system on the surr
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H(heat of rxn)=u + pv
-measured using a calorimeter
enthalpy
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energy available to do work
gibbs free energy (delta G)
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delta H= Hfinal - H initial
delta H>0 endothermic
delta H<0 exothermic
directly proportional to the amount of reactions/products involved
enthalpy of reaction (delta H)
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allow chemists to find "H" (enthalpy) for reactions that cant be perfomed directly
Hess's Law
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in any spontaneous process, the entropy (s) "disorder" of the universe is increasing. and remains unchanged in an equilibrium process.
1. s<l<g
2. increase in s, increase in T, particles moving faster
3. delta S = Sprod - Sreact
2nd law of thermodynamics
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products are favored
free energy
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delta H<0, delta S>0
Spontaneous free energy
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delta G
if (-) spontaneous
if (+) non spontaneous
if (=0) equal
delta G=delta H-TdeltaS
(for S to be negative, temp needs to be low)
Gibbs free energy
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delta H <0, delta H>0
delta S <0, delta S>0 all depends on temperature
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Factors that can change a non spontaneous rxn to spontaneous rxn:
- Temp
- couple a ns rxn with one that is spont
- pressure
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every substance has a finite(f) entropy, but at zero Kelvin, the entropy may become zero as in the case of a perfect crystal
3rd law of thermodynamics
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speed of any change over a period of time
amount of mol (react)/ time
rate
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atoms, ions and molecules react to form products when they collide provided particles have enough kinetic energy.
collision theory
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factors affecting reaction rates
- Temp-energy move faster
- catalyst
- concentration-the more qty the more reaction
- particle size-the more you have---> rxn faster
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if stress is applied to a system in dynamic equlibrium, the system changes to relieve the stress
Le Chateliers principle
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3 types of stresses
- change in R/P
- change in temp
- change in P/ change in V (gases)
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