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15 Cards in this Set
- Front
- Back
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isolated
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cannot exchange energy OR matter with the surroundings
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closed
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can exchange energy BUT NOT matter with the surroundings
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open
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can exchange BOTH matter and energy with the surroundings
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isothermal
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temperature of the system reamins constant
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adiabatic
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no heat exchange occurs
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isobaric
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pressure of the system remains constant
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heat (q)
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q = mc(deltaT)
m = mass c = specific heat deltaT = change in temperature |
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endothermic
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reactions that absorb energy
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exothermic
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reactions that release energy
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enthalpy (H)
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total H =
H of products - H of reactants |
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Entropy (S)
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delta S =
S final - S initial or q in reversible process / T |
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spontaneous / nonspontaneous
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spon = deltaG is negative
nonspon = deltaG is positive |
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Gibbs Free Energy (G)
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deltaG =
deltaH - T(deltaS) |
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Bond Dissociation Energy
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deltaH of reaction =
deltaH of bonds broken - deltaH of bonds formed or total energy input - total energy released |
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Hess's Law
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enthalpies of reactions are additive
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