N₂(g) + 3H₂(g) ⇌ 2NH₃(g)
In the above equilibrium, if the pressure is increased, the volume will decreases. The system responds to this effect by reducing the number of gas molecules. i.e., it favours the formation of ammonia.
If the pressure is reduced, the volume will increases. It favours the decomposition of ammonia.

(i) Methyl bromide to acetone (ii) Benzyl alcohol to 2-phenylacetic acid.
\(CH_{ 3 }Br+Mg\overset { dry\quad ether }{ \longrightarrow } { CG }_{ 3 }MgBr\overset { { CH }_{ 3 }CHO }{ \longrightarrow } \overset { \underset { | }{ OMgBr } }{ \underset { \overset { | }{ { CH }_{ 3 } } }{ CH } } -{ CH }_{ 3 }\overset { { H }_{ 2 }O }{ \longrightarrow } { CH }_{ 3 }\underset { \overset { | }{ { CH }_{ 3 } } }{ C } HHOH\overset { Cu }{ \underset { { NH }_{ 3 } }{ \longrightarrow } } \left( { CH }_{ 3 } \right) _{ 2 }CO\) 
(ii) C₆H₅CH₂OH + SOCl₂ \(\longrightarrow\) C₆H₅CH₂CI + KCN \(\longrightarrow\) C₆H₅CH₂CN \(\overset { { H }_{ 3 }O^{ + } }{ \longrightarrow } \) C₆H_sCH₂COOH

Ozone adds to carbon-carbon triple bond of alkynes to form ozonides. The ozonides are hydrolysed by water to form carbonyl compounds. The hydrogen peroxide formed in the reaction may oxidise the carbonyl compound to carboxylic acid.
(a) Acetylene

(b) Propyne:

(i) The principle involved is different compounds are adsorbed on an adsorbent to different degree.
(ii) Silica gel and alumina are the commonly used adsorbent. The components of the mixture move by varying distances over the stationary phase.

(i) Carbon compounds containing more than one halogen atom are called polyhalogen compounds.
(ii) They are classified as
(i) gem dihalides
(ii) Vicinal dihalides.
(a) Gem dihalide: In this compound, two halogen atoms are attached to one carbon atom
e.g, CH₃CHCl₂ ethylidene chloride.
(b) Vicinal dihalide: In this compound, two halogen atoms are attached to two adjacent carbon atoms.
\(\underset { \overset { | }{ Cl } }{ { CH }_{ 2 }- } \underset { \overset { | }{ Cl } }{ { CH }_{ 2 } } \) 1, 2-dichloro ethane

Depletion of ozone layer creates some sort of holes in the blanket of ozone which surrounds us in the atmosphere and this is known as ozone hole
(i) With the depletion of the ozone layer, UV radiations filters into the troposphere which leads to ageing of skin, cataract, sunburn, skin cancer etc.
(ii) By killing many of the phytoplanktons, it can damage the fish productivity.
(iii) Evaporation rate increases through the surface and stomata ofleaves which can decrease the moisture content of the soil.

1.In the case of gaseous solute in liquid solvent, the solubility decreases with increase in temperature.
2. When a gaseous solute dissolves in a liquid solvent, its molecules interact with solvent molecules with weak inter molecular forces when the temperature increases, the average kinetic energy of the molecules present in the solution also increases.
3. The increase in kinetic energy breaks the weak inter molecular forces between the gaseous solute and liquid solvent with results in the release of the dissolved gas molecules to gaseous state,
4. The dissolution of most of the gases in liquid solvents is an endothermic process, the increase in temperature decreases the dissolution of gaseous molecules

(ii) Bond order \(\alpha\) Stability
Greater the bond order, more stable the molecule is
Eg: N₂(B.O = 3) is much stable than O₂(B.O = 2)
Bond order \(\alpha {1\over Bond \ length}\)
Greater the bond order shorter is the bond length.
Eg: Nitrogen: B.O. = 3; Bond length =110pm Oxygen: B.O. = 2; Bond length = 121pm.

P_solute  = K_H X_{solute in solution}
At pressure 1.5 atm,
p₁ = K_H x_{1       ------}(1)
At pressure 6.0 atm,
p₂ = K_H x₂        -----(2)
Dividing equation (1) by (2)
From equation p₁/p₂ = x₁/x₂
1.5/6.0 = 0.24/x₂
Therefore x₂ = 0.24 x 6.0/1.5 = 0.96 g/L.

\(K_c={[AB]^2\over [A_2][B_2]}\)
A - green
B - blue

Given that 'V' is constant (closed system)
At equilibrium
\(K_c={({4\over V})^2\over ({2\over V})({2\over V})}={16\over 4}=4\)
K_P = K_C (RT)^Δn
K_P = 4(RT)^o = 4
At Stage 'x'
\(Q={({6\over V})^2\over ({2\over V})({1\over V})}={36\over 2}=18\)
Q > K_C ie., reverse reaction is favoured
At Stage 'y'
\(Q={({3\over V})^2\over ({3\over V})({3\over V})}={9\over 3\times 3}=1\)
K_C > Q ie., forward reaction is favoured.

CH_4(g) + 2O₂ \(\rightarrow\) CO₂ + 2H₂O
16g                          (2x18)g
As per stoichiometric equation,
16 g of methane produces 36 g of H₂O
\(\therefore\) 32 g of methane will produce = \(\frac { 36 }{ 16 } \times 32=72\) g of water.

(i) Water exists in space in the interstellar clouds, in proto-planetary disks, in the comets and icy satellites of the solar system, and on the Earth.
(ii) In particular, the ortho-to-para ratio (OPR) of water in space has recently received attention. Like hydrogen, water can also be classified into ortho-H₂O and para-H₂O), in which the directions are antiParallel.

(iii) At the temperature conditions of the Earth (300 K), the OPR of H₂O is 3.
(iv) At low temperatures below (<50 K) the amount of para-H₂O) increases. It is known that the OPR of water in interstellar clouds and comets has more para-H₂O) (OPR = 2.5) than on Earth.

Efficiency = work performed / heat absorbed
\(\eta =\frac { |{ q }_{ h }|-|{ q }_{ c }| }{ |{ q }_{ h }| } \)
q_h  - heat absorbed from the hot reservoir
q_c  - heat transferred to cold reservoir
\(\eta =1-\frac { |{ q }_{ c }| }{ |{ q }_{ h }| } \) ....(1)
For a reversible cyclic process
\(\Delta\)S(universe) = \(\Delta\)S(system)+\(\Delta\)S(surroundings) = 0
\(\Delta\)S(system) = -\(\Delta\)S(surroundings)
\(\frac { qh }{ { T }_{ h } } =\frac { -{ q }_{ c } }{ { T }_{ c } } \)
\(\frac { -{ T }_{ c } }{ { T }_{ h } } =\frac { { q }_{ c } }{ { q }_{ h } } \)
\(\frac { { T }_{ c } }{ { T }_{ h } } =\frac { |{ q }_{ c }| }{ |{ q }_{ h }| } \)  .....(2)
Substituting (2) in (1)
\(\Rightarrow \eta =1-\frac { { T }_{ c } }{ { T }_{ h } }...(3)\)
T_h >> T_c
Hence, \(\eta \) < 1

The volume of a gas increases with temperature at constant pressure. Each line (isobar) represents the variation of volume with temperature at certain pressure. The pressure increases from PI to P. i.e. P₁ < P₂ < P₃ < P₄ < P₅ When these lines are extrapolated or extended to zero volume, they' intersect at a temperature of - 273.15°C. All the gases are becoming liquids if they are cooled to sufficiently low temperatures. In other words, all gases occupy zero volume at absolute zero

It is due to weak metallic bonds and large atomic size.

V₁ = 8.5 dm³ V₂ = 6.37 dm³
T₁ = ? T₂ = 0^o C = 273 K
\(\frac { { V }_{ 1 } }{ { T }_{ 1 } } =\frac { { V }_{ 2 } }{ { T }_{ 2 } } \)
\({ V }_{ 1 }\times \left( \frac { { T }_{ 2 } }{ { V }_{ 2 } } \right) ={ T }_{ 1 }\)

T₁ = 364.28 K

Circumference of the orbit - 2\(\pi\)r         .... ...(1)
Circumference of the orbit of H - atom (n = 1) - n\(\lambda\),  .........(2)
(1) = (2) \(2 \pi r=\lambda \text { (or) } 2 \pi r=\frac{\mathrm{h}}{\mathrm{mv}}\)

The largest use of plaster of paris is in the building industry as well as plasters. It is used for immobilising the affected part of organ where there is a bone fracture or sprain. It is also employed in dentistry, in ornamental work and for making casts of statues and busts.

Metal Hydride (Hydrogen Sponge):
The best studied binary hydrides are the palladium - hydrogen system. Hydrogen interacts with palladium in a unique way, and forms a limiting monohydride, PdH. Upon heating, H atoms diffuse through the metal to the surface and recombine to form molecular hydrogen. Since no other gas behaves this way with palladium, this process has been used to separate hydrogen gas from other gases.

\(2 \mathrm{Pd}(\mathrm{s})+\mathrm{H}_{2}(\mathrm{~g}) \rightarrow 2 \mathrm{PdH}(\mathrm{s})\)
The hydrogen molecule readily adsorbs on the palladium surface, where it dissociates into atomic hydrogen. The dissociated atoms dissolve into the interstices or voids (octahedral/tetrahedral) of the crystal lattice.
Technically, the formation of metal hydride is by chemical reaction but it behaves like a physical storage method, i.e., it is absorbed and released like a water sponge. Such a reversible uptake of hydrogen in metals and alloys is also attractive for hydrogen storage and for rechargeable metal hydride battery applications.

The carbon monoxide of the water gas can be converted to carbon dioxide by mixing the gas mixture with more steam at 400^oC and passed over a shift converter containing iron/copper catalyst. This reaction is called as water-gas shift reaction.
CO + H₂O ➝ CO₂ + H₂