chapter 6

  • breaking bonds requires energy while forming bonds releases energy

  • PE = mgh

  • KE = m(v)²/2

    • mass, velocity

  • si unit of energy is joules = kg(m²)/s²

  • 1 cal = 4.184 j

  • E total = KE + PE +internal energy

    • internal energy is extensive

  • work is positive (energy added) when done ON the thermodynamic system, and negative (energy subtracted) when it’s done BY the system

    • work (JOULES = L.atm) = -PΔV

  • q = heat

    • positive if absorbed by / added to the system

    • negative is evolved / released by the system

  • open system is open to atmosphere

  • closed isn't open to atmosphere but energy can cross that boundary

  • isolated system isn’t open to atmosphere and nothing can cross the boundary

  • state function:

    • property of a system that depends only on present state (final and initial) and not the path

    • p, v, energy, t

  • change in internal energy = heat + work

    • CHECK UNITS

  • heat of reaction

    • exo -

    • endo +

  • enthalpy = u +pv

  • q = ΔH

    • change in enthalpy

  • ΔU = q + w = ΔH - PΔV

  • q = CΔt

    • molar heat capacity

  • q= mcΔt

    • c = specific heat

  • ΔH° = Eᴘ - Eʀ


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