Chemistry in English Hóa học bằng tiếng anh

Volume 25
Managing Editor
Mahabir Singh
Editor
Anil Ahlawat
(BE, MBA)

No. 9

September 2016

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CONTENTS

Class 11
NEET | JEE Essentials

8

Examiner’s Mind

21

Ace Your Way CBSE

32

MPP-3

41

Concept Map

46

Class 12
Concept Map

47

NEET | JEE Essentials

48

Examiner’s Mind

62

Ace Your Way CBSE

69

MPP-3

75

Competition Edge
Chemistry Musing Problem Set 38

78

NEET Phase II Solved Paper 2016

79

Chemistry Musing Solution Set 37

84

Crossword

85

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CHEMISTRY TODAY | SEPTEMBER ‘16

7


STATES OF MATTER : GASES AND LIQUIDS

EXISTENCE OF DIFFERENT STATES OF MATTER
ª A substance may exist as solid, liquid or gas under

GASEOUS STATE

ª Gaseous state exists in two different forms : vapour
form (exists below critical temperature) and gas
form (exists above critical temperature).

appropriate conditions of temperature and pressure.

ª A substance may also exist simultaneously in all
the three states under certain specific conditions
of temperature and pressure. For example, water
exists as ice, water and water vapour at 0.01°C and
4.58 mm of Hg pressure. Such temperature of a
substance is said to be its triple point.

ª Measurable properties of gases :
z
z
z
z

Mass (S.I. unit – kg)
Volume (S.I. unit – m3)
Temperature (S.I. unit – K)
Pressure (S.I. unit – Pa)


Mysterious new state of matter in a real material !
Researchers have just discovered the evidence of the new state known as
‘quantum spin liquid’ and it causes electrons to break down into smaller
quasiparticles. The electrons aren’t actually splitting down into smaller
physical particles but the new state of matter is breaking electrons down
into quasiparticles. Quasiparticles are not actually real particles, but are
concepts used by physicists to explain and calculate the strange behaviour
of particles. The matter itself also isn’t a liquid in the traditional sense
of word, but it instead refers to the fact that the quantum spins of the

electrons in the material suddenly start interacting to create a disordered
state, creating all kinds of strange behaviours.
8

CHEMISTRY TODAY | SEPTEMBER ‘16


CHEMISTRY TODAY | SEPTEMBER ‘16

9


GAS LAWS
Boyle’s Law
At constant T,
1
V ∝ or P1V1 = P2V2
P

Gay-Lussac’s Law
At constant V,
P1 P2
=
P ∝ T or
T1 T2

Charles’ Law
At constant P,
V V
t (°C)

Vt = V0 +
V0 or V ∝ T or 1 = 2
T1 T2
273.15

Gas Laws
Dalton’s Law of Partial Pressures
Ptotal = p1 + p2 + p3 + ... pn
RT
= (n1 + n2 + n3 + ...)
V

Graham’s Law of Diffusion

Avogadro’s Law
At a given
T and P,
V∝n

r1
d
M2
= 2 =
r2
d1
M1

Graphical
representations
Boyles’ Law


 



 



(at const. P)




 


Charles’ Law



 







–273.15°C 0 °C
 



 

 

 









 




0 = 22.4 L mol–1





 

ª Ideal gas equation : PV = nRT, where the constant R represents work done per degree per mole.
0.0821 L atm K–1 mol–1

0.083 L bar K–1 mol–1

8.314 J K–1 mol–1

1.99 cal K–1 mol–1






82.05 cm3 atm K–1 mol–1

8.31 × 107 erg K–1 mol–1

8.314 dm3 kPa K–1 mol–1

5.189 × 1019 eV K–1 mol–1

KINETIC THEORY OF GASES

Relation between different speeds : ump : uav : urms =
1 : 1.128 : 1.224

ª Average

kinetic energy
3 RT 3
K .E. =
= kT
2 NA 2

per

molecule

MOLECULAR SPEEDS
Most probable
speed (ump)
2RT
M
10

Average
speed (uav)

Root mean square
speed (urms)

8RT
πM

CHEMISTRY TODAY | SEPTEMBER ‘16

3RT
M

:

MAXWELL’S DISTRIBUTION OF SPEEDS









1
3

ª Kinetic gas equation : PV = mNu2

      


















































BEHAVIOUR OF REAL OR NON-IDEAL GASES











 







 












!