Gaseous State Formulas

The Gaseous State concept is one of the important topics in chemistry. The study of gaseous state formulas is very crucial to do calculations easily. If you are stuck with difficult Gaseous state concept related problems then provided Gaseous state formulas list helps you a lot. So, try to memorize all the formulas of the Gaseous state concept and apply them whenever needed. However, the Gaseous state formula sheet aid you to learn the formulas daily and enhances your knowledge of the Gaseous State concept.

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Important List of Gaseous State Formulas

In this section, students will discover the list of all Gaseous State formulas with examples for some concepts. Also, you can get some help from the formula sheet of the Gaseous State. This Gaseous State Formulae list is very effective to revise all the important points quickly before the exams or during homework for students. Hence, check out the important Gaseous State Formulas Table & Sheet from here.

1. Gas Laws:
(i) Boyle’s Law:
It is states that at constant temperature, the volume of a given mass of a gas is inversely proportional to the pressure.
V ∝ \(\frac{1}{\mathrm{p}}\)

(ii) Charle’s law:
This law states that at constant pressure, the volume of a given mass of a gas is directly proportional to its absolute temperature.
V ∝ T & Vt = V0\(\frac{273.15+t}{273.15}\)

(iii) Gay-Lussac’s Law or Amonton’s Law:
At constant volume, the pressure of a given mass of a gas is directly proportional to its absolute temperature.
P ∝ T & Pt = P0\(\left(1+\frac{t}{273.15}\right)\)

2. Ideal gas equation:
PV = nRT

  • R = 0.0821 litre atm. deg.-1 mole-1
  • R =62.4 litres mm. deg.-1 mole-1
  • R = 8.314 × 107 ergs deg.-1 mole-1
  • R = 82.05 C.C.atm. deg.-1 mole-1
  • R = 2 cals, deg.-1 mole-1
  • R = 8.314 JK-1 mole-1

3. Graham’s Law of Diffusion Or Effusion:
\(\sqrt{\frac{M_{2}}{M_{1}}}=\frac{r_{1}}{r_{2}}=\frac{P_{1}}{P_{2}} \sqrt{\frac{d_{2}}{d_{1}}}\) r1 & r2 rate of diffusion
Rate of diffusion = \(\frac{\text { Volume of gas diffused }}{\text { Time taken for diffusion }}\)

4. PV = \(\frac{1}{3} \mathrm{mn} \overline{\mathrm{v}}^{2}\)

5. Velocities related to gaseous state:
RMS velocity C = \(\sqrt{\frac{3 \mathrm{PV}}{\mathrm{M}}}=\sqrt{\frac{3 \mathrm{RT}}{\mathrm{M}}}=\sqrt{\frac{3 \mathrm{P}}{\mathrm{d}}}\)
& Average speed = \(\sqrt{\frac{8 \mathrm{RT}}{\pi \mathrm{m}}}\)
& Most probable speed = \(\sqrt{\frac{2 R T}{M}}\)
Average speed = 0.9213 × RMS speed
& RMS speed= 1.085 × Average speed
MPS = .816 × RMS; RMS = 1.224 MPS
& MPS : A.V. speed : RMS = 1 : 1.128 : 1.224

6. Mean free Path (λ):
The distance travelled by the gaseous molecule b/w the two successive collision is known as mean free path.
λ = \(\frac{1}{\sqrt{2} \pi \sigma^{2}} \cdot \frac{\mathrm{RT}}{\mathrm{PV}}\)

7. Collision frequency:
Z = \(\frac{1}{2}\) σ π2N2v
& Z = \(\frac{1}{2}\) × no. of collision × total no. of molecules

8. Specific heat of gases:
Cv = Cv × M & CP = CP × M
γ = \(\frac{C_{p}}{C_{V}}\)

9. Difference between real gas & ideal gas:

Ideal gas Real gas
1. Obeys gas law under all conditions P and T. Obeys only at low of P and T.
2. Obeys ideal gas equation Does not obeys ideal gas equation
3. Intermolecular interaction between gaseous molecules are negligible. Intermolecular interaction between gaseous molecules not negligible.
4. Volume of a particle is negligible as compared to total volume of the gas. Volume of a particle is not negligible as compared to total volume of the gas.
5. Exists only at high temperature and low pressure Exists only at low temperature and high pressure

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