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5 Thermochemistry - Coggle Diagram

- - - - ΔH = ΔE + PΔV = q
    - - the enthalpy change when one mole of a compound is formed from its elements under standard conditions
    - - the enthalpy change when the amounts of reactants shown in the equation react to give products under standard conditions
  - - - endothermic
    - - exothermic
  - - - the amount of energy required to raise the temperature of 1 g of a substance by 1 K
      - specific heat
        
        s = q/(m*ΔT)
    - - q - msΔT
    - - the heat absorbed by the water is a very good approximation of the enthalpy change for the reaction
      - because the volume in the bomb calorimeter is constant, what is measured is really the change in internal energy ΔE
- - - - work
        
        energy used to cause an object that has mass to move
        
        F*d
      - heat
        
        energy used to cause the temperature of an object to rise
        
        flows from warmer objects to cooler objects
    - - potential energy
        
        energy an object possesses by virtue
      - kinetic energy
        
        energy an object possesses by virtue of its motion
    - - joule
        
        J
      - calorie
        
        cal
    - - energy can be converted from one type to another
    - - energy is neither created nor destroyed
    - - the sum of all kinetic and potential energies of all components of the system
      - ΔE= E(final) - E(initial)
        
        ΔE>0
        
        absorb energy from the surroundings
        
        endergonic
        
        ΔE>0
        
        release energy to the surroundings
        
        exergonic
      - ΔE= q + w
        
        energy is exchanged between the system and the system and the surroundings
      - state function
        
        ΔE depends only on E(initial) and E(final), but q and w do not
    - - energy in foods
        
        carbohydrates and fats
      - energy in fuels
        
        fossil fuels
  - - - the molecules we want to study
    - - everything else
    - - heat is absorbed by the system from the surroundings
        
        endothermic
      - heat is released by the system into the surroundings
        
        exothermic