Equations of State

Question 1

Pressure equation

Answer 1

P = F/A 
(F = force; A = area)

Question 2

Energy Classification

Answer 2

The total internal energy, E, of a particle (or a system) is the sum of the potential energy and kinetic energy of all the particles present in the system

Question 3

Internal energy of a chemical system depends on

Answer 3

• # of partcles
• type of particles
• temperature

Question 4

Coulomb potential energy

Answer 4

V (r) = (Q1 * Q2) / 4(pi)(epsilon)r

Question 5

Quantization definition

Answer 5

particle (atom, molecule, subatomic, etc.) in a confined region of space

restricted to certain discrete values of energy

Question 6

Boltzmann Distribution

Answer 6

(N2/N1) = e^(Ei/Ej)/kT

Question 7

Trends of the Boltzmann Distribution

Answer 7

• The bigger the energy of the state, the lower its population
• The bigger the temperature, the more likely it is that a higher energy state is populated

Question 8

What is the Boltzmann distribution used for

Answer 8

formula for calculating relative populations at different states

Question 9

Equipartition Theorem

Answer 9

Used to calculate avg. kinetic energy of translational and rotational modes of motion in molecules

Equation: 3/2kT

Question 10

Kinetic Molecular Theory of Gases assumptions

Answer 10

• gases consist of molecules (or atoms) in constant, random motion
• Pressure, P, arises from collisions with container walls
• No attractive or repulsive forces between molecules. Collisions elastic (total kinetic energy = same)
• volume of molecules= negligible (compared to total volume of sample)