University:
The University Of Western Ontario
Course:
2223B | Organic Chemistry of Biological Molecules
Academic year:

2023
Views:

76

Pages:

1
Author:

Cole M.

Kinetic Molecular Theory of Gases Boltzmann’s Constant: For something to have a high temperature, then the average kinetic energy of the molecules are high as well PV = NkBT (N is simply the number of molecules/atoms of that substance and kB is Boltzmann’s constant) kB = R/NA = 1.38x10-23 J/K - Heat Capacity at Constant Volume & Pressure: For a monatomic ideal gas (only the noble gases), the internal energy is simply: KEtot = Uint = (3/2) PV = (3/2)NkT = (3/2)nRT In order to increase internal energy, heat up the system or increase the pressure on the system (do work) Change in internal energy is: ΔU = Q + W (Q is heat and W is work) and is actually the first law of thermodynamics which states there are only two ways in order to add energy to a system (If the gas expands then energy is decreased → -W and if - gas is compressed then energy is increased → +W) W = PΔV and only works if pressure remains constant (basically you need to heat up the system in order to keep pressure the same) Heat capacity is when heat is added, how much does the temperature increase? (C = Q/ΔT) You can do this for constant volume (CV) or constant pressure (CP) CV is constant for any monatomic ideal gas (CV = (3/2)NkB = (3/2)nR) CP is constant for any monatomic ideal gas (CP = (5/2)nR Therefore, CP - CV = nR Kinetic Molecular Theory of Gases: Macroscopic components of a substance such as pressure, volume, temperature have to do with the microscopic components, such as positions and speed Force is also: F = ΔP/Δv (where P is momentum) KEavg = (3/2)kBT Also, remember that V = Ah (Area times height)