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Midterm #1 - Thermochemistry
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49 Terms
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thermodynamics
the general study of energy and its interconversions
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energy (E)
the capacity to do work
* 1 J = 1 kgm^2/s^2
* 1 cal = 4.184 J
* 1000 cal = 1 kcal = 1 Cal
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work (w)
a force acting over a distance
w = force (distance)
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heat (q)
the flow of energy caused by a difference in temperature
* exchange of therma energy
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kinetic energy
the energy of motion
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thermal energy
a form of kinetic energy
* energy associated with temperature
* temperature is a measure of the thermal energy
* temperature is proportional to the heat transferred
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potential energy
energy that is stored in an object or energy associated with the composition and position of the object
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chemical energy
a form of potential energy
* energy stored in the structure of a compound
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system
defined area of investigation (the subject)
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surroundings
everything that the system can exchane energy with (everything else other than the system)
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state function
depends only on the current state and not the path taken
* ex - temp, pressure, concentration, physical state, enthalpy
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path function
depends on route taken to get between two states; “journey”
* ex - work and heat
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extensive property
based on the amount of a substance
* ex - mass, volume, and length
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intensive property
not based on the amount of a substance (inherent)
* ex - temperature, color, melting point, molecular weight
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internal energy
kinetic energy + potential energy
* state function
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first law of thermodynamics - law of conservation of energy
the total energy of the universe is constant
* energy can neither be created nor destroyed, only transferred
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change in energy equation
delta E = q + w
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\-q
system loses thermal energy
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\+q
system gains thermal energy
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\-w
work is done by the system
* using work and requires more energy
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\+w
work is done on the system
* gaining energy
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how much work is done during the combustion?
delta E = q + w
* use wording to access if it is - or +
* find w in kJ
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heat exchange
occurs when there is a difference in temp
* flows from high to low temp
* continues until thermal equilibrium is reached
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heat capacity
the amount of thermal energy a system must absorb through a heat transfer in order to undergo a specified change in temp
* like threshold
* q = C (delta T)
* q = J/ celcius
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specific heat capacity
heat capacity per gram
* q = mass C (delta T)
* mass = g
* q = J/ g celcius
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molar heat capacity
heat capacity per mol
* q = mol C (delta T)
* q = J/(mol Celcius)
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heat capacity and thermal energy relationship
higher heat capacity = more thermal enregy needed to raise the temp
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thermal energy transfer
(mC delta T) of system = - (mC delta T) of surroundings
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pressure-volume work
when force is changing the volume against an exerted pressure
w = -pressure (delta V)
* p = L atm
* energy = J
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pressure equation
pressure = force/area
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pressure to energy converstion
1 L(atm) = 101.3 J
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bomb calorimetery
constant volume
q rxn = -q cal = -C delta T
* C = kj/mol
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solving bomb calorimetery
1. find heat capacity (c) of bomb calorimeter
2. use heat capacity to find E rxn
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enthalpy
a measurement of energy in a thermodynamic system
* delta H = delta E + P(delta V)
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enthalpy at a constant pressure
delta H = q
* usually for atmospheric pressure (coffee cup)
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constant pressure calorimetry (coffee cup)
ΔHrxn = qrxn = -q of solution/ water
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ΔH vs ΔE
they are almost the same
* will be similar if small change in volume
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bond energy/ enthalpy
energy needed to break one mole of a bond in a compound
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using bond enthalpy to find ΔHrxn
1. ΔHrxn = bonds broken - bonds formed
2. ΔHrxn = energy of all bonds in the products vs. all bonds in the reactants
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solving for bond energy
ΔHrxn = broken (+ value) + formed (- value)
ΔHrxn (kJ/mol) = ΔH of product - ΔH of reactant
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standard enthalpy change
the change in enthalpy for a process when all reactants and products are in their standard states (ΔH°rxn)
* ΔH°rxn = ΔH°f of product - ΔH°f of reactant
* catabolic = -
* anabolic = +
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hess’s law
the change in enthalpy for a stepqise process is the sum of the enthalpy changes of the steps
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multiplying equation for hess’s law
multiply everything including ΔH
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reversing the equation in hess’s law
make the ΔH the opposite sign
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lattice energy
energy of formation of a crystalline solid from gaseous ions; the two ions attract
* always - since energy is being released
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ionization energy
remove an electron
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bond energy
breaking bond
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lattice energy trends
ion charge increases = magniture increases
ion size increases = magnitude decreases
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ionic radii trend
down and to the left it increases
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