Stage 3

• Photosynthesis

  Cellular respiration breathing
• Properties of Gases

  • Don't have own volume
  • Don't have own shape
  • Expand and contract
  • Fluency
  • High diffusion
  • Solubility
• Gas Variables

  • Pressure (P)
  • Volume (V)
  • Temperature (T)
  • Quantity of gas (expressed in moles)
• Moles= grams / Molas Mass
• Temperature Scales

  • Farenheit
  • Celsius
  • Kelvin
• Boyle's Law (pressure-volume relationship)

  The volume of a fixed amount of gas is inversely proportional to its pressure, when the temperature is constant.
• Boyle's Law

  If pressure increases, volume decreases

  If pressure decreases, volume increases
• Charles Law (volume-temperature relationship)

  At a constant pressure, the volume of a gas is directly proportional to the absolute temperature.
• Charles Law

  If temperature increases, volume increases

  If temperature decreases, volume decreases
• Gay-Lussac's Law (Pressure-Temperature)

  The pressure of a gas is directly proportional to its absolute temperature, when the volume is fixed.
• Gay-Lussac's Law

  If temperature increases, pressure increases

  If temperature decreases, pressure decreases
• Ideal Gas Law 


  If the gas is at a low pressure and a high temperature the density of the gas is going to be very low, so it can be considered that there are no interactions between the gas molecules and the volume of the molecules is zero.
• Combined Gas Law


  This law establishes the relationship between the pressure, volume, and absolute temperature of a fixed amount of gas
• Law of Partials Pressures

  The total pressure of a mixture of gases is the sum of the partial pressure exerted by each of the gases that make up the mixture.
• Thermodynamics: 


  This is the part of physics that studies the heat and work exchanges that accompany physicochemical processes.
• Chemical Thermodynamics


  The relationship between chemical reactions and the energy changes that involve the heat associated with said chemical changes.
• Chemical Kinetics: 


  Studies the speed at which a chemical process occurs and the factors that affect it.
• Energy


  The ability to do work or transfer heat
• Work (W)


  s the energy used to achieve the displacement of a body a certain distance (d) against a certain force (F)
• Heat (Q): 


  Is defined as the form of energy that is transferred due to a temperature difference
• Exothermic Reaction


  Release of energy
• Endothermic Reaction


  Absorption of energy
• Thermodynamic System


  Is the portion of the universe that is taken for study, and the environment is the rest of the universe that is outside the system and that can act on it or not.
• System + Natural environment = Universe
• Thermodynamics system classification

  • Open system
  • Closed system
  • Isolated system
• Open Systems:


  They can exchange energy and matter with their environment
• Closed systems: 


  They can exchange energy, but their mass remains constant, they cannot leave or enter.
• Isolated Systems: 


  Cannot exchange energy or matter with their environment
• State of aggregation of the components:

  • Homogeneous
  • Heterogeneous
• Homogeneous


  It's made up of a single phase
• Heterogeneous


  It consists of more than one phase.
• Thermodynamic Variables

  • Extensive
  • Intensive
• Extensive Variables


  The extensive variables depend on the mass of the system.
• Intensive Variables


  Intensive variables are independent of the mass of the system
• Entropy (s)


  magnitude that indicates the energy that cannot do useful work in a thermodynamic process.
• Entalphy (H)


  Meassure of the termal energy of a chemical system
• Free Energy (G)


  It is a measure of the amount of energy available to carry out a job in the system.
• Internal Energy


  The total energy (kinetic and potential) that a system has due to the particles that make it up.
• Heat Capacity


  The amount of heat absorbed or given, required to change the temperature of said substance by 1 C.
• Heat of Reaction


  It is the heat absorbed or released in a process or chemical reaction.