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15 Cards in this Set

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isolated
cannot exchange energy OR matter with the surroundings
closed
can exchange energy BUT NOT matter with the surroundings
open
can exchange BOTH matter and energy with the surroundings
isothermal
temperature of the system reamins constant
adiabatic
no heat exchange occurs
isobaric
pressure of the system remains constant
heat (q)
q = mc(deltaT)

m = mass
c = specific heat
deltaT = change in temperature
endothermic
reactions that absorb energy
exothermic
reactions that release energy
enthalpy (H)
total H =
H of products - H of reactants
Entropy (S)
delta S =
S final - S initial
or
q in reversible process / T
spontaneous / nonspontaneous
spon = deltaG is negative
nonspon = deltaG is positive
Gibbs Free Energy (G)
deltaG =
deltaH - T(deltaS)
Bond Dissociation Energy
deltaH of reaction =
deltaH of bonds broken - deltaH of bonds formed
or
total energy input - total energy released
Hess's Law
enthalpies of reactions are additive