CHAPTER
5 States of Matter
Gaseous Laws: Ideal gas equation PV = nRT
R = 0.0821 L atm mol–1 K–1
Boyle’s law: R = 8.314 J K–1 mol–1
1 R = 2 cal K–1 mol–1, R = 8.314 × 107 erg K–1 mol–1
V ∝ (n, T = const) ⇒ P1V1 = P2 V2
P
Graham’s Diffusion Law
Charle’s law:
It is applicable for non reacting gases
V T2
V ∝ T(n, P= const) ⇒ 2= 1 1 1
V1 T1 r∝ ;r∝ ;r∝ (P,T =
constant)
d VD Mw
Gay lussac’s law:
Rate of diffusion
P2 T2
P ∝ T(n, V
= const) ⇒ = ldiffused gas Vdiffused gas n diffused gas
P1 T1 =r = ;r = ;r
t time taken t time taken t time taken
Avogadro’s law:
V ∝ moles ∝ number of molecules (P,T = const) (When, l = distance travelled by diffused gas)
Kinetic Gas Equation : PV = (1/3) mN V2rms
Dalton’s Law of Partial Pressure Average Kinetic Energy (KEav)
Pmixture= P1 + P2 + P3.....(T & V const.) 3
K.Eav = nRT (n moles)
2
Partial pressure 3
K.Eav = RT (1 mol or NA molecules)
Pmoist gas= Pdry gas + Pwater vapour 2
3
It is applicable for non reacting gases. K.Eav = KBT (1 molecule)
2
From ideal gas equation KB = 1.38 × 10–23 JK–1 molecule–1 = Boltzmann constant
PAV = nA RT & PBV = nB RT v12 + v 22 + v32 + ... + v 2n
u rms =
(PA & PB are partial pressure) N
v1 + v 2 + v3 + ... + v n
In the form of mole fraction. u av =
N
nA
PA = XAPT = P; 3RT 8 RT 2RT
nT T =u rms = ; u av = ; u mp
Mw π Mw Mw
nB
PB = XBPT = P urms: uav: ump = 3 :
8
:
nT T 2 =1 : 0.92 : 0.82
π
[XA + XB = 1] 8
ump: uav: urms = 2 : : 3 =1 : 1.128 : 1.224
PT = sum of partial pressure of all gases π
5 States of Matter
Gaseous Laws: Ideal gas equation PV = nRT
R = 0.0821 L atm mol–1 K–1
Boyle’s law: R = 8.314 J K–1 mol–1
1 R = 2 cal K–1 mol–1, R = 8.314 × 107 erg K–1 mol–1
V ∝ (n, T = const) ⇒ P1V1 = P2 V2
P
Graham’s Diffusion Law
Charle’s law:
It is applicable for non reacting gases
V T2
V ∝ T(n, P= const) ⇒ 2= 1 1 1
V1 T1 r∝ ;r∝ ;r∝ (P,T =
constant)
d VD Mw
Gay lussac’s law:
Rate of diffusion
P2 T2
P ∝ T(n, V
= const) ⇒ = ldiffused gas Vdiffused gas n diffused gas
P1 T1 =r = ;r = ;r
t time taken t time taken t time taken
Avogadro’s law:
V ∝ moles ∝ number of molecules (P,T = const) (When, l = distance travelled by diffused gas)
Kinetic Gas Equation : PV = (1/3) mN V2rms
Dalton’s Law of Partial Pressure Average Kinetic Energy (KEav)
Pmixture= P1 + P2 + P3.....(T & V const.) 3
K.Eav = nRT (n moles)
2
Partial pressure 3
K.Eav = RT (1 mol or NA molecules)
Pmoist gas= Pdry gas + Pwater vapour 2
3
It is applicable for non reacting gases. K.Eav = KBT (1 molecule)
2
From ideal gas equation KB = 1.38 × 10–23 JK–1 molecule–1 = Boltzmann constant
PAV = nA RT & PBV = nB RT v12 + v 22 + v32 + ... + v 2n
u rms =
(PA & PB are partial pressure) N
v1 + v 2 + v3 + ... + v n
In the form of mole fraction. u av =
N
nA
PA = XAPT = P; 3RT 8 RT 2RT
nT T =u rms = ; u av = ; u mp
Mw π Mw Mw
nB
PB = XBPT = P urms: uav: ump = 3 :
8
:
nT T 2 =1 : 0.92 : 0.82
π
[XA + XB = 1] 8
ump: uav: urms = 2 : : 3 =1 : 1.128 : 1.224
PT = sum of partial pressure of all gases π
