1- Chapter 13 - Gasses Flashcards
1
Q
Boyles Law? (Fixed Temp)
A
p1V1=p2V2
2
Q
Charles Law? (Constant pressure)
A
V1/T1=V2/T2
3
Q
Universal Gas Law?
A
PV/T=constant
pV=nRT for n moles, where R is molar gas constant.
(pV=nNAkT)
(pV=NkT)
4
Q
Assumptions in working out kinetic theory of gasses?
A
- Gas Consisits of sperate molecule sin random motion
- Intermolcular forces can be negleted due to large distance
- The Objects make inelastic collisons
- Ignore gravity and relativity
- Neglect volume of molecules
5
Q
3 Steps for working out kinetic theory of gasses?
A
- Momentum Change at colision calculation
- Average over all speed
- Average over all directions
6
Q
Kinetic theory of gas equation
A
7
Q
What is c2?
A
Its the mean squared speed
8
Q
Crms=
A
9
Q
ΔU=
A
W + Q
change in internal energy=Work done + themal transfer
10
Q
Q(thermal transfer)=
A
mcpΔT(=mcpΔθ)
11
Q
Likly displacement from start of a gas molecule? =
A
λ N0.5
Where λ is the mean free path = average travel without collision.
12
Q
R (molar gas constant) =
A
NAK (avogadros number x boltzman constant)
13
Q
Total kinetic energy of gas molecules=
A
3/2 NkT
(or 3/2 nRT)
(as one molecule =3/2kT)
14
Q
Rough energy of any particle?
A
kT
15
Q
A
