Linetic
theory
collection of molecules that in random directions.
Gases are a more
rapidly
Gases
Ideal Gas Real Gas
↳ The intermolecular ↳
force (IMF) bu The intermolecular force (IMF) bw
molecules is zero .
IMF = 0 molecules is not zero . IMF #0
↳ ↳
Energy of ideal gas molecules Energy of real
gas molecules
-0
E =
K E . . + P E
.
.
E =
K E . . + P E . .
E = K E .
Behaviour of Gases : -
the intermolecular force (IMF) between molecules
1 is
negligible .
2 At
high temperature low pressure ,
and all gases follow the following simple
relation, which is called the equation.
gas
PV = nRT where p =
Pressure V = volume
g
n =
Number of moles; T =
Temperature
R //mol-K gas constant
= $ 314
.
universal .
R
Ideal gas ↳ Number of moles
I Mass Im Num of Particles (N
Mo
.
TT2> Tz n = =
number (Nn)
Molar Avogadro's
-
mass
T3
↳
O
PVenRT = RT
platm)
P =
/ART P =
↳
pr = RT Here , Kn == 1 3841523 T/
.
-
PV =
NKsT
Boltzmann constant
, Boyle's law : -
PV curve : -
Px P
From the
gas equation
PV nRT
,
= X
if n and I are constant, then
PV constant
= >
-
VCI G
&
P, Vi =
PeVe
O > V
O -
This is an isothermal process and
the P-V graph will be hyperbolic .
Slope of the curve - :
PV = constant
on
differentiating
Pdr + vdp = 0
pdV = - VdP
=> slope-m =
d=
Charles's law From the
gas equation
: -
PV nRT
=
,
if n and p are constant, then
VIT ↳ This is an isobaric process .
or
=
P-v graph P-T graph V-T
graph
Do Po Vo
·
v ·
T
L
- T
Slope m = 0
slope m = o
slope m
=
theory
collection of molecules that in random directions.
Gases are a more
rapidly
Gases
Ideal Gas Real Gas
↳ The intermolecular ↳
force (IMF) bu The intermolecular force (IMF) bw
molecules is zero .
IMF = 0 molecules is not zero . IMF #0
↳ ↳
Energy of ideal gas molecules Energy of real
gas molecules
-0
E =
K E . . + P E
.
.
E =
K E . . + P E . .
E = K E .
Behaviour of Gases : -
the intermolecular force (IMF) between molecules
1 is
negligible .
2 At
high temperature low pressure ,
and all gases follow the following simple
relation, which is called the equation.
gas
PV = nRT where p =
Pressure V = volume
g
n =
Number of moles; T =
Temperature
R //mol-K gas constant
= $ 314
.
universal .
R
Ideal gas ↳ Number of moles
I Mass Im Num of Particles (N
Mo
.
TT2> Tz n = =
number (Nn)
Molar Avogadro's
-
mass
T3
↳
O
PVenRT = RT
platm)
P =
/ART P =
↳
pr = RT Here , Kn == 1 3841523 T/
.
-
PV =
NKsT
Boltzmann constant
, Boyle's law : -
PV curve : -
Px P
From the
gas equation
PV nRT
,
= X
if n and I are constant, then
PV constant
= >
-
VCI G
&
P, Vi =
PeVe
O > V
O -
This is an isothermal process and
the P-V graph will be hyperbolic .
Slope of the curve - :
PV = constant
on
differentiating
Pdr + vdp = 0
pdV = - VdP
=> slope-m =
d=
Charles's law From the
gas equation
: -
PV nRT
=
,
if n and p are constant, then
VIT ↳ This is an isobaric process .
or
=
P-v graph P-T graph V-T
graph
Do Po Vo
·
v ·
T
L
- T
Slope m = 0
slope m = o
slope m
=
