FINALS Flashcards
the ability to do work or transfer heat
energy
the study of energy and its transformation
thermodynamics
the study of chemical reactions and the energy changes that involve heat
thermochemistry
seen between oppositely charged ions
electrostatic attraction
chemical bonds are formed
energy is released
when chemical bonds are broken
energy is consumed
can be converted from one form to another, but it is neither created nor destroyed
energy
portion of the universe that we single out study
system
are everything else
surroundings
TYPES OF SYSTEM
Open, Closed, Isolated
can exchange heat and mass with its surroundings
open system
can only exchange heat with its surroundings
closed system
can not exchange heat or mass with its surroundings
isolated system
system is the sum of all kinetic and potential energies of all components
internal energy
system absorbed energy from the surroundings.
ΔE > 0, Efinal > Einitial
the system released energy to the surroundings.
ΔE < 0, Efinal < Einitial
What is the value of ΔE if Efinal equals Einitial?
zero
three parts of thermodynamic quantities
number, unit, sign
the system gains energy from the surroundings.
A positive ΔE
the system loses energy to the surroundings.
negative ΔE
change of internal energy is:
ΔE = q + w
heat is absorbed by the system from the surroundings
endothermic
heat is released by the system into the surroundings
exothermic
internal energy is a
state function