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40 Terms
chemical energy
potential energy stored in chemical bonds
internal energy (E)
the sum of all the kinetic and potential energies of all the components of a system
thermochemistry
the study of energy and its transformations
first law of thermodynamics
energy cannot be created or destroyed, though it can change from one form to another
universe =
system + surroundings
heat
energy used to cause the temperature of an object to increase
work
energy used to cause an object that has mass to move
state entity
a property of an entity based soley on its chemical or physical state or both nut not on how it achieved that state. only concerned with the difference between initial and final value
thermal energy
the portion of the total internal energy of a system that is proportional to its absolute temperature
kinetic energy
the energy of an object in motion
kinetic energy formula
KE= ½ mu2
potential energy
the energy that an object has because of its position
exothermic process
energy in the form of heat flow from a system into surroundings
hear is released
endothermic process
energy in the form of heat flows from the surroundings into the system.
heat is absorbed
heat transfer from system to surroundings
q<0
heat transferred to the system
q>0
work done by the system
w<0
work done on the system
w>0
pressure-volume (P-V) work
the work associated with the expansion or compression of a gas
enthalpy (H):
a measure of the total energy of a system; the sum of the internal energy and the pressure-volume product of a system
enthalpy (H) equation
H= E + PV
enthalpy change (△H)
the energy absorbed by an endothermic process or given off by an exothermic process that takes place at constant pressure
enthalpy change (△E) equation
△H = △E + △(PV)
enthalpy of fusion (△Hfus)
the energy required to convert one mole of a solid substance at its melting point into the liquid state; also called the heat of fusion
enthalpy of vaporization (△Hvap)
the energy required to convert one mole of a liquid substance as its boiling point into the vapor state; also called the heat of vaporization
system
includes the molecules we want to study; the chemical equation
surroundings
everything else
heat capacity (Cp)
the energy required to raise the temperature of an object by 1oC at constant pressure
formula to calculate how much thermal energy (q) must be transferred to an object to raise its temperature by an amount △T
q = Cp(△T)
specific heat (Cs)
the energy required to raise the temperature of 1g of a substance by 1oC at constant pressure
specific heat equation
Cp (J / oC) = m(g) x Cs [s/g x oC)]
equation; relates energy flow to the change in temperature of a mass (m) of a pure substance
q= mcs △T
molar heat capacity (Cp)
the energy required to raise the temperature of one mole of a substance by 1oC at constant pressure
molar heat capacity (Cp) equation
q= ncp△T
calorimetry
the experimental determination of the quantity of energy transferred during a phase or chemical process
calorimeter
a device used to measure the absorption or release of energy by a phase change or chemical process
enthalpy of reaction (△Hrxn)
the enthalpy change that accompanies a chemical reaction; also called the heat of reaction
thermochemical equation
the chemical equation of a reaction that includes the change in enthalpy that accompanies the reaction
bomb calorimeter
a constant-volume device used to measure the energy released during a combustion reaction
calorimeter constant (C calorimeter):
the heat capacity of a calorimeter