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CHAPTER 5
STATES OF MATTER
1
...
Measurable properties of gases : P,V, T, n, Viscosity,
specific heat are some measurable properties
...
Gas Laws : The quantitative relationship b/w any two of
the variables (V, n, P,T) when other two are constant
...
Boyle’s Law : The pressure of fixed msss of gas varies
inversely with the volume at constant T
...
)
P1V1 = P2 V2
5
...
VαT
6
...
PαT
7
...
8
...
V α n ( P, T constant)
9
...
(T, V, constant)
10
...
12
...
Gases consist of large number of identical particles
(atoms or molecules) that are so small that the actual
volume of the molecules is negligible in comparison to
the empty space between them
...
There is no force of attraction between the particles of a
gas at ordinary temperature and pressure
c
...
Pressure is exerted by the gas as a result of collision of
the particles with the walls of the container
e
...
At any particular time, different particles in the gas have
different speeds and hence different kinetic energies
g
...
Compressibility factor (Z) : It determine extent of devation
of real gases from Ideal gas behavior : Z =
PV
for ideal
n
...
T
...
Vander waal’s Equation : P
14
...
gas cannot be liquefied whatever high pressure may be
15
...
16
...
17
...
74
18
...
E
...
19
...
At higher altitude : The b
...
of water decreases b/c the
atmospheric pressure is less than one atmosphere
...
Surface Tension (V) : It is force acting per unit length
perpendicular to the line drawn on the surface : (Nm-1) : It
decreases with increases in T, it increases with increase in
external pressure, b/c of it falling drops of liquid are
spherical, liquid in capillary tube rises
...
Viscosity (η) : It is resistance offered to the flow of liquid
due to friction b/w layer of fluids
...
A
...
dv
dn
Effect of T & P on viscosity : It decreases with increase in
T, and increases with increase in P
...
Low M
...
& B
...
of molecular liquids is due to low
magnitude of molecular interaction energy
...
At what condition surface tension vanishes ?
2
...
At what temperature below which a gas does not obey ideal
gas law?
4
...
What is the molar volume at 0oC and 1 bar pressure?
75
6
...
7
...
How is the partial pressure of a gas in a mixture is related to
the total pressure of the gaseous mixture?
9
...
10
...
Ans 2
...
Ans 3
...
Ans 4
...
Ans 5
...
Ans 6
...
Both decreases with increase in temperature
Ans 8
...
At hill station the atmospheric pressure is less and so
boiling point decreases
...
For ideal gas Z=1
...
1
How do you convert pressure in atmosphere in to SI unit
...
2
What type graph will you get when PV is plotted against P
at constant temperature
...
3
What would have happened to the gas if the molecular
collisions were not elastic?
Q
...
5
Why liquids diffuse slowly as compared to gases?
Q
...
7
In terms of Charle’s law explain why -273o C is the lowest
P
...
T 2
?
n
temperature?
Q
...
9
What correction is applied to obtain pressure of dry gas
with the total pressure & aqueous tension?
Q
...
Answers to two marks questions
Ans 1
...
Ans 2
...
Ans 3
...
Ans 4
...
77
Ans 5
...
i
...
P
...
T 2
n
Ans 6
...
m
2
(m 3 ) 2 ( K ) 2
mal
N
...
e
...
Vander waal’s equation
Ans 8
...
R
...
P (dryygas) = P (Total) – Aqueous tension
Ans 9
...
Surface tension can explain (i) capillary action
...
Three Marks Questions
Q
...
0 moles of gas occupying 5dm3
volume at 3
...
(R= 0
...
2
PV
nR
3
...
0mol x 0
...
Ans
34
...
0625g at 543 o C
and 1 bar pressure what is molar mass of phosphorous?
Ans
...
05
at 0 o C
(54 b 273 ) 273
Or V2 = 11
...
35 ml of vapours at 0 oC and 1 bar pressure weight
0
...
0625
x 22700
11
...
3
A mixture of dihydrogen and dinitrogen at 1 bar pressure
contains 20% by weight of H2
...
Ans The mixture of H2 and O2 contain 20% H2 means 20 gm H2
& 80gm O2
n2 (H2) =
P(H2) =
Q
...
5contest
...
5
0
...
P1 = 1bar
...
constant 30oC
So by Boyle’s low P1V1 = P2 V2
1 x 500 = P2 x 200
Q
...
5 bar
Calcutate the total pressure in mixture of 4g of O 2 and 2gm
...
(R =
0
...
Mol-1
Ans
P
no2
=
Q
...
0821 x 273
2
x
2
1
1
8
1 22
...
2 atm
...
Ans
(i) At higher altitudes atmospheric pressure decreases, but
inside the balloon gas exerts pressure and size becomes larger
...
8
What do you mean by ideal gas and real gas? Why do real
gases deviate from ideal behaviors?
Ans
...
Real gas deviate from ideal behaviour due to force of attraction
and because of volume of molecules of gases are not
negligible
...
9
Using the equation of state PV=nRT Show that at given T,
density of gas proportional to gas pressure P
...
RT
v
m 1
m RT
, , R
...
...
(Where P
M
PxP
RT
M
m
)
v
const
...
10 Critical temperature of CO2 and CH4 gases are 31
...
90C respectively
...
b/c
of greater polarity and high molecular wt
...
(a)Why aerated water bottles kept under water during summer?
(b) Which property of liquid is responsible for spherical
shape of drop?
(c) Why is moist air lighter than dry air?
(d) Define aqueous tension?
(e) What is units of a and b which are vander waal’s
constant?
Ans (a) To reduce temperature so to reduce pressure, other wise
bottle may burst
...
(c) Moist air has water vapours which lowers vapour density,
so it is lighter
...
(e)Unit of a in atm
...
Q
...
b/c of surface tension
...
3 Arrange following in order of increasing density:
Q
...
RT
d
PM
P
, R, M are constant, so d depends upon
so at 250C,
RT
T
P
T
1
P 1
o
Hence increasing order of
, At 273 C, 1atm
298
T 546
density will be: O2 at 2730 C, 1atm < O2 at 250 C, 2atm
...
4
An O2 cylinder has 10L O2 at 200 atm
...
50ml
of O2 at 1 atm in one breath at 370C
...
5 x 10 3 L
81