Thermodynamics

    Cards (13)

    • Thermodynamics
      The study of the relations between heat, work, temperature, and energy
    • Laws of Thermodynamics
      • Describe how the energy in a system change and whether the system can perform useful work on its surroundings
    • 0th Law

      1. If two objects are in equilibrium with another object, therefore, they are also in equilibrium with each other
      2. Thermal Equilibrium = No heat transfer
      3. Heat moves from hot to cold surface
    • 1st Law

      Law of Conservation of Energy. Energy can't be created nor destroyed. It can, however, be transferred and transform into another form
    • 2nd Law

      • The entropy of the universe is always increasing
      • Entropy (∆S) is the tendency of a matter to become disorganized
      • Everything is doomed for chaos and destruction
      • Your room will have a chance of becoming disorganized as time goes by, but never a chance of it becoming more organized on its own
    • 3rd Law

      • The entropy of a crystalline solid at a temperature of zero Kelvin (absolute zero) is equal to zero
      • Solid has lesser entropy than liquid and gas since its particles are more organized
    • System
      The collection of bodies, matter, or mass that is being studied
    • Surrounding
      What's left in the universe, except the system
    • Enthalpy (∆H)

      The total internal energy (∆U) of a system
    • Types of Systems
      • Isovolumetric: ∆U = Q, Any change in energy is the result of heat transfer, Constant volume, W = 0
      • Isothermal: Q = W, Heat transferred us completely used for work, Constant temperature, ∆U = 0
      • Adiabatic: ∆U = - W, Internal energy is used exclusively for work, No heat transfer, Q = 0
      • Isolated System: ∆U = 0, No change in internal energy, Q = 0, W = 0
    • Gibbs Free Energy (∆G)
      ∆G = ∆H - T∆S, Tells us about the spontaneity of a process
    • Gibbs Free Energy Relationships
      • Spontaneous: ∆G = -, Thermodynamically favorable, Always spontaneous, Never nonspontaneous
      • Nonspontaneous: ∆G = +, Thermodynamically unfavorable, Always nonspontaneous, Never spontaneous
      • ∆G = -, ∆H = -, ∆S = +, Energetically favorable, Entropically favorable, Spontaneous
      • ∆G = +, ∆H = +, ∆S = -, Energetically unfavorable, Entropically unfavorable, Nonspontaneous
      • ∆G = +/-, ∆H = +, ∆S = +, Energetically unfavorable, Entropically favorable, Spontaneous at high temperature
      • ∆G = +/-, ∆H = -, ∆S = -, Energetically favorable, Entropically unfavorable, Spontaneous at low temperature
    • Thermodynamic systems can be classified as open (exchange matter with surroundings), closed (no exchange of matter but exchange heat/energy), or isolated (neither exchanges matter nor energy).
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