NOTE: k = Boltzmann constant = 1.38E-23
NOTE: R = the gas constant = 8.314
NOTE: remember to use Celcius and Kelvin when appropriate

1.1: Molecular Speeds
a) (.004 kg)/(1 mol) * (1 mol)/(6.022e23 atoms)
b) "The total kinetic energy of the collection of X atoms is KE."
   <KE>Ar = KE/X
   <KE>He = KE/X
c) m = (atomic weight)/(6.022e23 atoms)
   <KE> = (1/2)*m*v2
d) KE = (3/2)kT
   T = [<KE>*(3/2)]/k

1.2: Mass On Spring
a) <PE> = 1/2*k*T  (k = 1.38*10^-23)
b) <v> = 0
c) PE + KE = kT
   <PE> + (1/2)mv2 = kT
   <v2> = [2*(kT-<PE>)]/m
d) 1

1.3: Equipartition of Energy
a) N = pV / kT        **NOTE: convert liters to m3
   U = (5/2)*N*k*T
b) find weight of N2: (.028kg)/(1mol) * (1mol)/(6.022e23 atoms)
   (3/2)kT = (1/2)mv2
c) n = (weight) * (1mol)/(63g)
   U = 3nRT
d) U = mgh  ::  h = U/(mg)
   U = (1/2)mv2  ::  vcm = sqrt[2U/m]

1.4: Gas Laws
a) N/V = p/(k*T)
b) Temperature remains the same
c) p1V1 = p2V2
d) N = N/V * Vi
   W=NkT*ln(Vf/Vi)
    

1.5: First Law of Thermodynamics
a) V1/T1 = V2/T2
b) N = pV / kT
   delta.U = (5/2)*N*k*(Tf - Ti)
c) Wby = p(Vf - Vi)
d) delta.U = Q - Wby
    Q = delta.U + Wby