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Chemistry Hobbs - Coggle Diagram

- - - - Solute
        
        minority component
      - Solvent
        
        majority component
  - - - Molarity (M)
        
        No. of Moles of Solute
        
        L of Solution
      - Molality (m)
        
        No. of Moles of Solute
        
        Mass (Kg) of Solvent
      - Molar Fraction
        
        No. of moles of solute
        
        No. of moles of solvent and solute
  - - - A solvent normally has higher entropy than the pure solute and solvent
        
        Solvents are usually entropically favoured
    - - The salt needs to be split into positive and negative ions to calculate enthalpy
- - - - Raoult's Law
        
        Pa=Vapor Pressure of Solvent
        
        Xa=Mole Fraction of A
        
        P*a=Vapour Pressure of Pure Solvent A
- - - - Gas
        
        Under given conditions of pressure and temperature a material will be found in one of these states depending on...
        
        Intermolecular forces
        
        These are attractive forces within the molecules which fight agents kinetic energy
        
        Kinetic Energy
        
        Kinetic energy is directly proportional to temperature
      - Liquid
      - Solid
      - A phase is a form of matter that is uniform throughout in chemical composition and physical state
        
        A phase transition is the spontaneous conversion of one phase to another phase. Occurs at a characteristic temperature for a given pressure
    - - X-axis
        
        Energy
        
        The slope of the line = The inverse specific heat capacity for that phase
      - Y-axis
        
        Temperature
    - - the pressure exerted by the vapour at equilibrium with its condensed phase at a given temperature
        
        Intermolecular Forces rise
        
        Lowers
        
        Temperature rise
        
        Rises
    - - When kinetic energy and the pressure is high enough sublimation occurs
        
        This converts the solid straight to a gas
    - - Critical Point
        
        This is where the gaseous and liquid phase merge together under a great deal of temperature and pressure
    - - R=Gas Constant
        
        H=Enthalpy of Vaporisation
        
        T=Temperature (Kelvin)
        
        p=Pressure
- - - - E.g.
        
        Vapaur Pressure Lowering
        
        Boiling Point Elevation
        
        Change in Bp/Fp = (Kb/Kf)(mb)
        
        Freezing Point Elevation
        
        Osmosis
        
        Osmatic Pressure is the hydrostatic pressure due to h
- - - - Q<K
        
        increase product formation until eq. is increased
        
        Q>K
        
        Increase reactant to reach eq.
        
        Q=K
        
        @ Equilibrium
    - - Reaction shifting
        
        Towards Products
        
        Q increases
        
        Towards Reactants
        
        Q Decreases
    - - G<0
        
        Spontanious
      - G=0
        
        Equilibrium
      - G>0
        
        Not Sponatnious