Kinetic Theory of Gases Detailed notes for the prep of JEE/NEET. This note is the best for your competitive exam preparation like JEE.NEET.

# KINETIC THEORY OF GASES Detailed Notes for JEE/NEET

### BEHAVIOUR OF GASES

#### IDEAL GAS

In an ideal gas, we assume that molecules are point masses and there is no mutual attraction between them. The ideal gas obeys following laws :**BOYLE’S LAW**According to Boyle’s law for a given mass of ideal gas, the pressure of a ideal gas is inversely proportional to the volume at constant temperaturei.e., _{}**CHARLE’S LAW**For a given mass, the volume of a ideal gas is proportional to temperature at a constant pressure i.e., _{}**GAY-LUSSAC’S LAW**For a given mass of ideal gas, the pressure is proportional to temperature at constant volume i.e., _{}**AVOGADRO’S LAW**According to Avogadro’s law, the number of molecules of all gases are same at same temperature, pressure and volume i.e., _{} for same P, V and T.The value of Avogadro number is 6.02 × 10^{23} molecules.**GRAHAM’S LAW**

- At constant temperature and pressure, the rms speed of diffusion of two gases is inversely proportional to the square root of the relative density

i.e., v_{rms}_{} ⇒_{}

- According to Graham’s law, the rate of diffusion of a gas is inversely proportional to the square root of its density, provided pressure and temperature are constant

_{}**DALTON’S LAW**The pressure exerted by a gaseous mixture is equal to sum of partial pressure of each component gases present in the mixture,i.e., P = P_{1} + P_{2 }+ P_{3}+……………… P_{n}A relation connecting macroscopic properties P, V and T of a gas describing the state of the system is called **equation of state**.The equation of state for an ideal gas of n mole is

_{}where R is universal gas constant whose value is

R = 8.31 J/mol K and R = N_{A}k, where k is Boltzmann’s constant (N_{A} is Avogadro number). n is the number of moles of a gas and_{}, N_{A} is Avogadro’s number where m is the mass of a gas, N is the number of molecules and M is the molecular weight of a gas.

#### EQUATION OF REAL GAS

The real gas follows Vander Wall’s law. According to this: ;here a and b are Vander Waal’s constant

_{}

#### CRITICAL TEMPERATURE, VOLUME AND PRESSURE

- The temperature at or below which a gas can be liquefied by applying pressure alone is called
**critical temperature**T_{C}. It is given by_{} - The volume of gas at a critical temperature T
_{C }is called**critical volume**V_{C}, where V_{C}= 3b - The pressure of gas at a critical temperature T
_{C }is called**critical pressure**P_{C}, where_{}

#### GAS EQUATION

- The gases found in nature are real gases.
- The real gas do not obey ideal gas equation but they obey Vander Waal’s gas equation

_{}

- a’ depends upon the intermolecular force and the nature of gas.
- b’ depends upon the size of the gas molecules and represents the volume occupied by the molecules of the gas.
- The molecules of real gas have potential energy as well as kinetic energy.
- The real gas can be liquefied and solidified.
- The real gases like CO
_{2}, NH_{3}, SO_{2}etc. obey Vander Wall’s equ^{n}at high pressure and low temperature.

### KINETIC THEORY OF AN IDEAL GAS

The basic assumptions of kinetic theory are :

- A gas consist of particles called molecules which move randomly in all directions.
- The volume of molecule is very small in comparison to the volume occupied by gas i.e., the size of molecule is infinitesimally small.
- The collision between two molecules or between a molecule and wall are perfectly elastic and collision time (duration of collision) is very small.
- The molecules exert no force on each other or on the walls of containers except during collision.
- The total number of molecules are large and they obey Newtonian mechanics.

_{} ….(i)where _{} is called mean square velocity and _{} is called root mean square velocityi.e, _{} ….(ii)and _{} ….(iii)where m = mass of one molecule and n = number of molecules_{} ….(iv)or _{}_{}or _{} ….(v)where E is translational kinetic energy per unit volume of the gas. It is clear that pressure of ideal gas is equal to 2/3rd of translational kinetic energy per unit volume.**Kinetic interpretation of temperature** : From eq^{n}. (iv), we get

_{}For 1 mole of a gas at temperature T :PV = RT so _{}_{} (_{}is Boltzmann constant)or _{} ….(vi)or _{}or _{} ….(vii)or _{}It is clear from eq.(vi) that at a given temperature, the average translational kinetic energy of any gas molecules are equal i.e., it depends only on temperature.From eq

^{n}. (vii) It is clear that

_{}_{}, where M is molecular mass of the gas.

### DEGREE OF FREEDOM

*The degree of freedom of a particle is the number of independent modes of exchanging energy or the number of independent motion, which the particle can undergo.*For **monatomic gas** such as helium, argon, neon etc. the molecules can have three independent motion i.e., it has

3 degree of freedom, all translational.

For a **diatomic gas** molecules such as H_{2}, O_{2}, N_{2},_{ }etc. it has two independent rotational motion besides of three independent translational motion, so it has 5 degree of freedom.

In **polyatomic gas** molecules such as CO_{2}, it can rotate about any of three coordinate axes. It has six degree (three translational + three rotational) of freedom. At high temperature the molecule can vibrate also and degree of freedom due to vibration also arises, but we neglect it.

### MEAN FREE PATH

The distance covered by the molecules between two successive collisions is called the **free path**.The average distance covered by the molecules between two successive collisions is called the **mean free path.**i.e., _{}_{}where, n = number of molecules per unit volume d = diameter of each molecule K_{B} = Boltzmann’s constant T = temperatureP = pressureMean free path depends on the diameter of molecule (d) and the number of molecules per unit volume n. At N.T.P., λ for air molecules is 0.01 µm.

### LAW OF EQUIPARTITION OF ENERGY

*If we dealing with a large number of particles in thermal equilibrium to which we can apply Newtonian mechanics, the energy associated with each degree of freedom has the same average value (i.e., ), and this average value depends on temperature.*From the kinetic theory of monatomic ideal gas, we have….(i)orEnergy of molecule = (number of degree of freedom) × ….(ii)So it is clear from equation (i) and (ii) that monatomic gas has three degree of freedom and energy associated per degree of freedom is (where k is **Boltzmann’s constant**)Since we know that internal energy of an ideal gas depends only on temperature and it is purely kinetic energy. Let us consider an 1 mole ideal gas, which has N molecules and f degree of freedom, then total internal energyU = (total number of molecules) × (degree of freedom of one molecule)× (energy associated with each degree of freedom) =(N) (f) × ()U = Nf ….(iii)Differentiating eq.(iii) w.r.t T, at constant volume, we get, ….(iv)Now molar, specific heat at constant volume is defined as ….(v)so ….(vi)where R is universal gas constant.Now by

**Mayer’s formula**, …. (vii)So ratio of specific heat is …(viii)where f is degree of freedom of one molecule. (a) For

**monatomic gas**, f = 3, , so (b) For

**diatomic gas**, f = 5, ,

_{}(c) For **polyatomic gas**, f = 6, _{} , _{}

_{}**KEEP IN MEMORY**

- Real gases behave like perfect gas at high temperature and low pressure.

In real gas, we assume that the molecules have finite size and intermolecular attraction acts between them.

- Real gases deviate most from the perfect gas at high pressure and low temperature.
- Gaseous state of matter below critical temperature is called vapours. Below critical temperature gas is vapour and above critical temperature vapour is gas.
- Random motion of the constituents of the system involving exchange of energy due to mutual collisions is called thermal motion.
- Total kinetic energy or internal energy or total energy does not depend on the direction of flow of heat. It is determined by the temperature alone.
- The internal energy of a perfect gas consists only of kinetic energy of the molecules. But in case of the real gas it consists of both the kinetic energy and potential energy of inter molecular configuration.

### DISTRIBUTION OF MOLECULAR SPEEDS

The speed of all molecules in a gas is not same but speeds of individual molecules vary over a wide range of magnitude.Maxwell derived the molecular distribution law (by which we can find distribution of molecules in different speeds) for sample of a gas containing N molecules, which is _{} …(1)where N(v)dv is the number of molecules in the gas sample having speeds between v and v + dv.where T = absolute temperature of the gasm = mass of moleculek = Boltzmann’s constantThe total number of molecules N in the gas can be find out by integrating equation (1) from 0 to ∞ i.e., _{} ….(2)

Figure shows Maxwell distribution law for molecules at two different temperature T_{1} and T_{2}(T_{2 }> T_{1}). The number of molecules between v_{1 }and v_{2} equals the area under the curve between the vertical lines at v_{1} and v_{2} and the total number of molecules as given by equation (2) is equal to area under the distribution curve.

The distribution curve is not symmetrical about most probable speed, v_{P},(v_{P} is the speed, which is possessed in a gas by a large number of molecules) because the lowest speed must be zero, whereas there is no limit to the upper speed a molecule can attain. It is clear from fig.1 that v_{rms}(root mean square) > (average speed of molecules) > (most probable speed) v_{P}

### AVERAGE, ROOT MEAN SQUARE AND MOST PROBABLE SPEED

#### AVERAGE SPEED

To find the average speed _{}, we multiply the number of particles in each speed interval by speed v characteristic of that interval. We sum these products over all speed intervals and divide by total number of particlesi.e., _{} (where summation is replaced by integration because N is large) _{} ….(1)

#### ROOT MEAN SQUARE SPEED

In this case we multiply the number of particles in each speed interval by v^{2} characteristic of that interval; sum of these products over all speed interval and divide by Ni.e., _{} ….(2)Root mean square speed is defined as

_{}

#### MOST PROBABLE SPEED

It is the speed at which N(v) has its maximum value (or possessed by large number of molecules), so_{} ….(3)It is clear from eq^{n}. (1), (2) and (3)

_{}The root mean square velocity of a particle in thermal system is given by

_{}where R – universal gas constantT – temperature of gasm – mass of the gasM – molecular weight of gas or mass of one mole of a gas.The average speed of the gas molecules is given by

_{}where M is the mass of one mole and m is the mass of one particle.Most probable speed is that with which the maximum number of molecules move. It is given by

_{}The most probable speed, the average speed as well as root mean square speed increases with temperature.**KEEP IN MEMORY**

- Brownian motion, provides a direct evidence for the existence of molecules and their motion. The zig-zag motion of gas molecules is Brownian motion.
- Average speed

_{}

- Root mean square speed,

_{}

- Most probable speed

_{}

- V
_{rms}:_{}: V_{mp}= 1.73 : 1.60 : 1.41

V_{rms} > _{} > V_{mp.}