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It is a cost effective approach that involves minimum chemical USAGE, minimum WASTE GENERATION
It involves not to produce green house gases like `CH_4,CO_2`
It works for not producing wasteful by products in the PROCESS
All

Frenkel defect in usually favoured by a very small difference in the sizes of cation and anion.
Frenkel efect is a disocation defect.
TRAPPING of an electron in the lattice leads to the formation of F - center
Schottky defects have no effect on the physical properties of solids.

`(i) and (III)
(i), (II) and (iii)
(i) and (IV)
(ii), (iii) and (iv)

`BeCI_(2)` is a covalent COMPOUND
`BeCI_(2)` can FORM diner
`BeCI_(2)` is an electron deficient molecule
The HYBRID state of Be in `BeCI_(2)` is `sp^(2)`

<P>(M and O) and (N and P) are two pairs of enantiomers
Bromination PROCEEDS through trans-addition in both the reactions
O and P are identical MOLECULES
(M and O) and (N and P) are two pairs of diastereomers

it behaves as a weak acid in water due to self ionization
acidity of its aqueous solution increases upon addition of ethylene GLYCOL
it has a three-dimensional structure due to hydrogen bonding
it isa weak electrolyte in water

The number of neighbours of an atom PRESENT in the topmost layer is 12.
The EFFICIENCY of the atom packing is 74 %
The number of octahedraland tetrahedral voids per atom are 1 and 2 respectively.
The unit cell edge length is `2sqrt2` times the radius of the atom.

The isotopes of chlorine with mass NUMBER 35 and 37 EXIST in ratio `3:21` if its average atomic mass is 35.5
The mass of one amu is APPROXIMATELY `1.6xx10^(-24)g`
The number of molecules in 1 ml of a gas at STP is called Loschmidt number
If `6.023xx10^(21)` molecules of a solute are present in 100 ml SOLUTION molarity of solution is 0.1M

All d-orbitals except `d_(Z^(2))` have two ANGULAR NODES.
`d_(x^(2)y^(2)), d_(z^(2))` lie on the axes.
The degeneracy of p-orbitals remains UNAFFECTED in the presence of external MAGNETIC field.
d-orbitals have 3-fold degeneracy.

first IONIZATION POTENTIAL of Al is less than the first ionization potential of MG
second ionization potential of Mg is greater than the second ionization potential of Na
first ionization potential of Na is less than the first ionization potential of Mg
THIRD ionization potential of Mg is greater than the third ionization potential of Al

(I) and (II) only .
(I) and (III) only
(II) and (III) only
(I), (II) and (III) only

It is recognized by its PUNGENT ORDER and production of white fumes, on blowing across the mouth of the test tube.
It is recognised by increase in intensity of white fumes when a glass rod moistened with ammonia solution is held near the mouth of the test tube.
It is recognised by its TURNING litmus PAPER blue.
X' gas is `CI_(2)` with GREENISH yellow fumes.

`CH_(3)COONA` may be the salt solution 'X'
Y' may be `[Fe(H_(2)O)_(5)(SCN)]^(2+)` ion
Z' may be the basic ACETATE of IRON (III)
Oxidation state of iron in 'Y' and 'Z' remains constant

ADDING an excess of hyposolution to the brown solution, 'D' is reduced to colourless solution and WHITE precipitate BECOMES visible.
F is `Cu_(3)[Fe(CN)_(6)]_(2)`
The reduction of hyposolution YIELDS tetrathionate ions
The co-ordination number of iron in the chocolate brown ppt. (F) is different from that of `K_(4)[Fe(CN)_(6)]`

both`H_(2) ^(+) and H_(2)^(-)` do not EXIST
`H_(2)^(-) ` is more stable than ` H_(2)^(+)`
`H_(2)^(+)`is more stable than ` H_(2)^(-)`
both ` H_(2)^(+) and H_(2)^(-)` are equally stable

Frenkel defect is usually favoured by a very small difference in the sizes of cation and anion
Frenkel defect is a dislocation defect
Trapping of an electron in the LATTICE leads to the FORMATION of F-center
Schottky defects have no EFFECT on the physical PROPERTIES of solids

O-O bond length are EQUAL
Thermal decomposition of `O_(3)`is endothermic
`O_(3)`is diamgentic in nature
`O_(3)` has a bent STRUCTURE

increasing TEMPERATURE increases the fraction of molecules having `U_(mps)`
Increasing temperature increases `U_(mps)`
In a SAMPLE of gas at a given temperature, molecules with extremely low and high speeds are less 
At the same temperature lighter gaseous having narrow DISTRIBUTION of molecular speeds than heavier gaseous 

The eclipsed CONFORMATION of ethane is more STABLE than STAGGERED conformation, because eclipsed conformation has no TORSIONAL strain
The eclipsed conformation of ethane is more stable than staggered conformation even though the eclipsed conformation has torsional strain
The staggered conformation of ethane is more stable than eclipsed conformation, because staggered conformation has no torsinal strain
The staggered conformation of ethane is less stable than eclipsed conformation, because staggered conformation has torsional strain

The eclipsed conformation of ETHANE is more stable than STAGGERED conformation, because eclipsed conformation has no torsional strain.
The eclipsed conformation of ethane is more stane THA staggered conformation EVEN though the eclipsed conformation has torsional strain.
The staggered conformation of ethane is more stane than eclipsed conformation, because staggered conformation has no tosional strain.
The staggered conformation of ethane is less stable than eclipsed conformation because staggered conformation has torional strain.

the eclipsed CONFORMATION of ETHANE is more stable than staggered conformation EVEN though staggered conformation has torsional strain.
the staggered conformation of ethane is more stable than eclipsed conformation, because staggered conformation has no torsional strain.
the staggered conformation of ethane is less stable than eclipsed conformation, because staggered conformation has torsional strain.
the staggered conformation of ethane is less stable than eclipsed conformation, because staggered conformation has no torsional strain.

the eclipsed conformation of ETHANEIS more stable than staggered conformation EVEN though the eclipsed conformation has torsional strain
the staggered conformation of theane is more stable than eclipsed conformation becasuse staggered conformationhas no torsional strain
the staggered conformatin of ETHANE is less stable than eclipsed conformation because staggered conformation has torsional strain
the staggered conformation of THANE is less stable than eclipsed conformation becausestaggered conformation has torsional strain

A and B
B and C
A and C
A, B and C

ICE has a HIGHLY ordered three dimensional hydrogen bonded structure.
Each oxygen atom in ice is surrounded tetrahedrally by four other oxygen atoms at a distance of 276 pm.
Hydrogen bonding GIVES ice a rather open structure with wide holed. These HOLES can hold some other MOLECULES of approapriate size interstitially.
All are correct

Graphite is not a CONDUCTOR because, it does not contain free ELECTRONS 
Graphite is a THREE dimensional conductor because, the p-electrons are delocalised three dimensionally 
Graphite is a two dimensional conductor because p-electrons are delocalised two dimensionally 
In graphite all the carbon atoms UNDERGO `sp^(3)` hybridization 

GRAPHITE is not a conductor because, it does not contain free electrons 
Graphite is a three dimensional conductor because, the p-electrons are delocalised three DIMENSIONALLY 
Graphite is a TWO dimensional conductor because p-electrons are delocalised two dimensionally 
In graphite all the carbon atoms undergo SP hybridization 

Rotation around carbon-carbon bond in ethane MOLECULE is not POSSIBLE, because ethane molecule contains a pi `(pi)` bond between the carbon and carbon and ethane has very low melting point
Rotation around carbon-carbon bond in ethane molecule is not possible, because ethane molecule contains both SIGMA `(sigma)` bond and pi `(pi)` bond between the carbon and carbon.
Rotation around carbon-carbon bond in ethane molecule is possible because of CYLINDRICAL symmetry of sigma `(sigma)` bond between carbon-carbon atoms
Rotation around carbon-carbon bond in ethane molecule is not possible, because ethane molecule contains both sigma `(sigma)` bond and pi `(pi)` bond between the carbon and carbon and ethane has very high BOILING point

at absolute zero temperature, entropy of a PERFECTLY CRYSTALLINE SOLID is zero
at absolute zero temperature, the entropy of a perfectly crystalline substance is + ve
at absolute zero temperature, the entropy of all crystalline substance is zero
at `0^(@)C`the entropy of a PERFECT crystalline solid is zero.

ELECTROPHILE is a NEGATIVELY charged SPECIES and canform a bond by accepting a pair of electrons from another electrophite
electrophiles are GENERALLY neutral species and can form a bond by accepting a pair of electrons from a NUCLEOPHILE
electrophile can be either neutral or positively charged species and can form a bond by accepting a pair of electrons from a nucleophile
electrophile is a negatively charged species and can form a bond by accepting a pair of electrons from a nucleophile.

Frenkel DEFECT is a dislocation defect
Frenkel defect is found in HALIDS of alkaline metals
SCHOTTKY defects have no effect on the density of crystalline solids
Frenkel defects decrease the density of crystalline solids

Frenkel defects are USUALLY favoured by a very small differences in the sizes of the cation and anion
Frenkel DEFECT is a dislocation defect
Trapping of an ELECTRON in the lattice leads to the formation of F-centre
Schottky defects have no effect on the physical properties of solids

a carbonyl compound with a HYDROGEN atom on its alpha-carbon RAPIDLY equilibrates with its corresponding enol and this process is known as carbonylation
the carbonyl compound with a hydrogen atom on its alpha-carbon rapidly equilibrates with its corresponding enol and this process is known as keto-enol tautomerism
a carbonyl compound withhydrogen atom on its alpha-carbon never equilibrates with its corresponding enol
a carbonyl compound with a hydrogen atom on its alpha-carbon rapidly equilibrates with its corresponding enol and this process is known as aldehyde-ketone equilibrium

`BeCI_(2)` is a covalent COMPOUND
`BeCI_(2)` is an ELECTRON deficient molecule
`BeCI_(2)` can from dimer
the HYBRID state of Be in `BeCI_(2)` is `sp^(2)`

`BI_(3)` is the weakestLewis acid AMONG the BORON halides
there is minimum `ppi- ppi`back bonding in `BF_(3)`
`BF_(3)` is the STRONGEST LEWISACID among the otherboronhalides
there ismaximum `ppi-ppi`back bonding in `BF_(3)`.

Hydroxide of aluminimum is more acidic than the hydroxide of boron
Hydroxide of boron is basic while the hydroxide of aluminium is amphoteric.
Hydroxide of aluminium is amphoteric since `Al-O` and `O-H` BONDS have NEARLY same ionic charcter
Hydroxide of boron is acidic since it ionizes in WATER to `BO_(3)^(3-)` land `H^(+)` ions.

It contains `CS^(3+)` and `I^(-)` ions.
It contains `Cs^(+), I^(-)` and lattice `I_(2)` MOLECULE.
It is COVALENT molecule.
It contaisn `Cs^(+)` and `I_(3)^(-)` ions.

It forms CYCLIC compounds
It forms CARBENE or SUBSTITUTED carbene
Two atoms are removed from `ALPHA " and " beta ` positions
In ` CHCl_(3) alpha ` - eliminationis not possible

For every gas there exists a characteristic TEMPERATURE above which it cannot be liquefied no matter however high is the pressure applied called CRITICAL temperature of the gas. 
For every gas there exists a characteristic temperature at which its compressibility factor is equal to unity for some range of pressure. 
Amongst `He, N_2, O_2 and CO_2,CO_2` has the lowest value of "a" and He has the lowest value "b" where a and BARE VANDER walls constants of the gas. 
The extent of departure of Z (compressibility factor) from unity is the measure of the extent of deviation from ideal behavior. 

The number of neighbours of an atom present in the TOPMOST layer is 12
The efficiency of the atom packing is 74%
The number of octahedral and tetrahedral voids per atom are 1 and 2 respectively
The unit cell edge length is `2sqrt2` times the radius of the atom

i only correct
ii only correct
iii only correct
all are correct

The density of `H_2O_2` is greater than `H_2O`
`H_2O_2` is a better IONIZING solvent thant `H_2O` because of more hydrogen in `H_2O` due to its high DIPOLE MOMENT
BOILING point of `H_2O_2` is more than `H_2O` because of more hydrogen BONDING in `H_2O_2`
On cooling water freezes earlier than `H_2O2`

In `H_2` and `D_2`the RATIO of bond length is 1:2
`""_1H^1` ' can be used as a tracer
`""_1H^3`emits LOW ENERGETIC B radiation and no g radiations
all the above

a and B are identical
a and b are diastereomers
a and C are enantiomers
a and b are enantiomers

Red precipitate is formed due to formation LEAD sulphochloride.
Red precipitate is formed due to DISPROPORTIONATION of `Hg_(2)CI_(2)`
Red precipitate [C] on dilution with water DECOMPOSE into `PbS` and `PbCI_(2)`
Red precipitate [C] on dilution with `H_(2)O`, it decomposes into Hg and `HgCI_(2)`.

the chemisorption of `H_(2)` as `H` atoms on the surface of glass is endothermic
Physical adsorption does not require ACTIVATION energy
Chemisorption is always unimolecular
In adsorption, only solute from the SOLUTION is adsorbed on the surface surface of the solid adsorbent

cltaltb
C=blta
clta=b
a=b=c

`(I)GT(II)gt(IV)gt(III)`
`(I)gt(III)gt(II)gt(IV)`
`(II)gt(I)gt(III)gt(IV)`
`(III)gt(I)gt(IV)gt(II)`

`(I) gt (II) gt (IV) gt (III)`
`(I) gt (III) gt (II) gt (IV)`
`(II) gt (I) gt (III) gt (IV)`
`(III) gt (I) gt (IV) gt (II)`