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16 Cards in this Set

  • Front
  • Back
the study of the transfers of energy as heat that accompany chemical reactions and physical changes.
measures the energy absorbed or released as heat in a chemical or physical change.
a measure of the average kinetic energyof the particles in a sample or matter.
measurement of heat.
the SI unit of heat as well as all other forms of energy.
- direction of energy
- transfer of heat
- high --> low
- you never get cold, you only lose heat
specific heat
the amount of energy required to raise the temperature of one gram of substance by one celcius degree or by one kelvin.
- conductors and insulators
- conductors = low specific heat ex. gold, lead
- insulators = high specific heat (holds onto energy) ex. water, glass
Cp= q/(m * delta T)
specific heat (J/g*K) = energy lost or gained (J)/ mass(g) * change in temp
heat of reaction
the quantity of energy released or absorbed as heat during a chemical reaction. (kJ/mol)
thermochemical reaction
an equation the includes the quantity of energy released or absorbed as heat during the reaction as written.
enthalpy change
the amount of energy absorbed or lost by a system as heat during the process at constant pressure
exothermic reaction
- energy is released
- the q is negative
endothermic reaction
- energy is absorbed
- the q is positive
- tend to be more unstable
molar heat of formation
the energy released or absorbed as heat when one mole of a compound is formed by combination of its element.
enthalpy change/ delta H of elements in their standerd state
heat of combustion
the energy released as heat by the complete combustion of one mole of a substance.
hess's law
the overall enthalpy change in a reaction is equal to the sum of enthalpy changes for the individual steps in the process.