Confused in Choosing between Electric and Regular Bed? Here’s all you need to know As an outcome, we have seen that with the durability of the time things are getting advanced and coming up with more and more features so as now same with beds nowadays electric beds are fetching very popular in people, as a result, many of the manufacturers and companies are adding electric beds in their stock as it has been seen that an electric bed is more comfortable and reliable than an ordinary bed but here is not the end. The question is what to choose between them which bed will bounce your satisfaction as well as which bed is value for money and is it worth to buy hospital beds/electric beds lets discuss in below topics and see. Adjustable bed vs Ordinary bed – A brief comparison As we have seen there are 2 sides of every coin so do everything had its advantages and disadvantages so let us see what are the benefits and disadvantages of having an electric/hospital bed Benefits of Elec
CHAPTER - 13
KINETIC ENERGY
- BOYLE's LAW:- It states that at a constant temperature, volume of given mass of gas is inversely proportional to its pressure.
v ~ 1\p
or PV= constant
- CHARLES LAW:- It states that at constant pressure, the volume of a given mass of gas is directly proportional to its absolute temperature.
V~T
or V\T = constant
- GAY LUSAC"S LAW:- It states that at constant volume, the pressure of a given mass of gas is directly proportional to its absolute temperature.
P~T
or, P\T = constant
For 1 degree Celsius rise in a temperature,
P(t) = P(b) (1 + t/273.15)
- IDEAL GAS EQUATION:- For 'n' mole of gas,
PV = nRT
for 1 mole, PV= RT
UNI.VERSAL GAS CONSTANT,
R = 8.31 J 1/mol 1/K
BOLTZMANN CONSTANT,
Kb = R/Na
Na -> AVAGADRO'S NO.
- IDEAL GAS:- A gas that obeys gas law strictly is an ideal or perfect gas. The molecules of such gas are of point size and there is no force of attraction between them.
- ASSUMPTION OF KINETIC THEORY OF GASES:-
- all gases consist of molecules that are rigid, elastic spheres identical in all respect for a given gas.
- the size of a molecule is negligible as compared with the average distance between two molecules.
- diving the random motion, the molecules collide with each other and with the wall of a vessel. The collisions are almost instantaneous
- the molecular density remains uniform throughout the gas
- the collisions are perfectly elastic in nature and there are no forces of attraction or repulsion between them.
- LAW OF EQUIPARTITION OF ENERGY
For any thermodynamical system in thermal equilibrium, the energy of the system is equally divided into its various degree of freedom, and the energy associated with each degree of freedom corresponding to each molecule is 1/2KbT, where Kb is the BOLTZMANN'S CONSTANT and T is the absolute temperature.
The law of equipartition of energy holds a good for all degrees of freedom whether translational, rotational, or vibrational.
A monoatomic gas molecule has only translational kinetic energy.Ex + Er = 1/2mv(x)*2 + 1/2mv(y)*2 + 1/2mv(z)*2 + 3/2.2KbT
So, a monoatomic gas molecule has only three degrees of freedom.
In addition to a translational kinetic energy, a diatomic molecule has two rotational kinetic energies.
E(t) + E(r) = 1/2mv(x)*2 + 1/2mv(y)*2 + 1/2mv(z)*2 + 3/2.2KBT
◯一◯
Here the line joining the two atoms has been taken x-axis about where there is no rotation, So, the degree of freedom of a diatomic molecule is 5, it does not vibrate.At a very high temperature, vibration is also activated due to which two extra degrees of freedom emerge from vibrational energy. Hence, at very high temperature degree of freedom of diatomic molecule is seven.
- PRESSURE EXERTED BY AN IDEAL GAS
P = 1/3e⊽*2
or, P = 1/3 nM⊽*2
where P = Pressure n = number density (no. of molecules/volume) M = mass of one molecule ⊽^2 = square mean speed also called kinetic gas eqn.
- MEAN K.E PER MOLECULE OF GAS
E = 1/2m⊽^2or, E = 3/2 KbT
- DALTON'S LAW OF PARTIAL PRESSURE
It states that total pressure of a mixer of non-reacting ideal gas is the sum of partial pressure exerted by individual gases in the mixture.
P = p1+p2+p3+....................+pn
- GRAHAMIC LAW OF DIFFUSION
It states that the rate of diffusion of a gas to inversely proportional to the square root of its density.
r~1/r√⍴
Graham's Law = r1/r2 = √⍴2/√⍴1
- SPEEDS OF THE GASES
Average Speed
- LAW OF EQUIPARTITION OF ENERGY
For any thermodynamical system in thermal equilibrium, the energy of the system is equally divided into its various degree of freedom, and the energy associated with each degree of freedom corresponding to each molecule is 1/2KbT, where Kb is the BOLTZMANN'S CONSTANT and T is the absolute temperature.
The law of equipartition of energy holds a good for all degrees of freedom whether translational, rotational, or vibrational.
A monoatomic gas molecule has only translational kinetic energy.
Ex + Er = 1/2mv(x)*2 + 1/2mv(y)*2 + 1/2mv(z)*2 + 3/2.2KbT
So, a monoatomic gas molecule has only three degrees of freedom.
In addition to a translational kinetic energy, a diatomic molecule has two rotational kinetic energies.
E(t) + E(r) = 1/2mv(x)*2 + 1/2mv(y)*2 + 1/2mv(z)*2 + 3/2.2KBT
◯一◯
Here the line joining the two atoms has been taken x-axis about where there is no rotation, So, the degree of freedom of a diatomic molecule is 5, it does not vibrate.
At a very high temperature, vibration is also activated due to which two extra degrees of freedom emerge from vibrational energy. Hence, at very high temperature degree of freedom of diatomic molecule is seven.
- PRESSURE EXERTED BY AN IDEAL GAS
P = 1/3e⊽*2
or, P = 1/3 nM⊽*2
where P = Pressure
n = number density (no. of molecules/volume)
M = mass of one molecule
⊽^2 = square mean speed
also called kinetic gas eqn.
- MEAN K.E PER MOLECULE OF GAS
E = 1/2m⊽^2or, E = 3/2 KbT
- DALTON'S LAW OF PARTIAL PRESSURE
It states that total pressure of a mixer of non-reacting ideal gas is the sum of partial pressure exerted by individual gases in the mixture.
P = p1+p2+p3+....................+pn
- GRAHAMIC LAW OF DIFFUSION
It states that the rate of diffusion of a gas to inversely proportional to the square root of its density.
r~1/r√⍴
Graham's Law = r1/r2 = √⍴2/√⍴1
- SPEEDS OF THE GASES
Average Speed
- DALTON'S LAW OF PARTIAL PRESSURE
It states that total pressure of a mixer of non-reacting ideal gas is the sum of partial pressure exerted by individual gases in the mixture.
P = p1+p2+p3+....................+pn
- GRAHAMIC LAW OF DIFFUSION
It states that the rate of diffusion of a gas to inversely proportional to the square root of its density.
r~1/r√⍴
Graham's Law = r1/r2 = √⍴2/√⍴1
- SPEEDS OF THE GASES
Average Speed
v= √8RT/πMor, v = √8PV/πMor, v = √8KbT/πM m/s
Root Mean Square Speed
Ⅴrms= √3RT/M
or, Vrms = √3RV/M m/s
or, Vrms = √3KbT/M
MOST PROBABLE SPEED
Vmp =√2RT/M
or, Vmp = √2PV/m
or, Vmp = √2KbT/M
DEGREES OF FREEDOM
The total number of co-ordinates of independent quantities required to describe completely position and configuration of a dynamical system is known as number of degrees of freedom of the system.
f= 3N-K
N = no. of molecules
K = no. of co-ordinates of the particle
For monoatomic, f=3
diatomic, f=5
triatomic (linear motion), =7
triatomic (non-linear motion), =6
MEAN FREE PATH
It is the average distance travelled by a molecule between two successive collisions. It is denoted by λ.
λ= 1/mπd*2
d= diameter of each molecule
m= no. of molecules per unit volume
λ= KbT/√2πd*2P
SPECIFIL HEAT CAPACITY
Average energy of a molecule at temp. T = 3/2KbT
total internal energy of a mole of such a gas is,
U= 3/2KbT
Na=3/2RT
molar specific heat at constant volume Cv(monoatomic gas)=
dv/dt = 3/2RT
For an ideal gas,
Cp - Cv = R
Cp = 5/2R
Ratio of specific heats,
Cp/Cv = 5/3
DIATOMIC GASES
A diatomic molecule has 5 degree of freedom : 3 transitional and 2 rotational,
U = 5/2KbT, Na = 5/2RT
Cv (rigid diatomic) = 5/2R
Cp = 7/2R
rigid diatomic = 7/5
POLYATOMIC GASES
Polyatomic molecule has 3 translational, 3 rotational and a certain number (f) of vibrational modes.
V = (3/2KbT + 3/2KbT + fKbT)Na
Cv = (3+f)R, Cp = (4+f)R
Note :- Cp -Cv = R is true for any ideal gas.
BROWNIAN MOTION
It is a zig-zag motion of the particle of microscopic size suspended in water, air, or some other fluid. This motion can be explained on the basis of K.T.
It depends upon :-
- size of suspended particle
- 'f' of fluid
- temperature of medium
- viscosity of the medium
LINK TO THIS CHAPTER'S YOUTUBE VIDEO:- https://youtu.be/voNdPhHOfVI
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