Pressure
1 atm= 76 cm of Hg= 760 mm of Hg= 760 torr
1 atm= 1.0110⁵ Nm²
1 atm= 1.0110⁵ Pa
1 bar= 0.9862 atm≈ 1 atm
mL= milli-litre
cm= centimeter
m= meter
dm= decimeter
atm= atmosphere
N= Newton
Pa= Pascals
Boyle's Law
According to Boyle's law,
V ∝ P⁻¹
or, PV = constant @particular temperature.
or, P₁V₁=P₂V₂
Charles' Law
According to Charles' Law,
V ∝ T @constant Pressure
therefore, V₁/T₁ = V₂/T₂
or, V₁T₂ = V₂T₁
Gay-Lussac's Law
According to Lussac's law,
P ∝ T
or, PT⁻¹ = constant @constant volume
P₁T₂ = P₂T₁
Ideal Gas Equation
PV=nRT
or, PVT⁻¹ = constant = nR
R= Universal Gas Constant
Universal Gas Constant
[R] = Lit atm K⁻¹ mol⁻¹ = work done per Kelvin per mole
R= 0.0821 Lit atm K⁻¹ mol⁻¹
R= 8.314 J K⁻¹ mol⁻¹ = 8.314 Pa cm³ K⁻¹ mol⁻¹
R= 1.987 cal K⁻¹ mol⁻¹
R= 5.189* 1019 eV K⁻¹ mol⁻¹
Dalton's Law of Partial Pressure
According to Dalton's Law of Partial Pressure,
P = P₁+P₂+P₃+.....+Pₙ = ΣPₙ
Where P is the total pressure and P₁, P₂, P₃... are the partial pressures of gases 1, 2, 3 and so on.
P₁= P*x₁
where x₁ is the mole fraction of gas 1.
Graham's Law of Diffusion
r= rate of diffusion
M= molar mass of given gas
d= density of given gas
n= number of moles of given gas
Velocity of Gas Particles
α:v:u = 1 : 1.128 : 1.224
Kinetic Energy
k = Boltzmann Constant = 1.380649 × 10−23 joule per kelvin
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