Q26Single correctOrganic Chemistry — Some Basic Principles and Techniques
Consider the following reactions:
Which of these reactions are possible?

SolutionAnswer: Option 2B and D Approach:
Assess each reaction for the feasibility of a Friedel-Crafts type substitution under anhydrous Lewis-acid conditions, considering the stability of the intermediate carbocation.
Step 1:Aryl halides such as chlorobenzene do not form the aryl cation, because the C-Cl bond has partial double-bond character; reaction A fails.
Step 2:Chlorination of benzene with excess chlorine over a Lewis acid in the dark proceeds; reaction B is possible.
Step 3:Vinyl halides do not undergo Friedel-Crafts because the vinyl cation intermediate is unstable; reaction C fails.
Step 4:Allyl halide generates a resonance-stabilized allyl cation, so the Friedel-Crafts alkylation proceeds; reaction D is possible.
Final answer: B and D
Q27Single correctOrganic Chemistry — Some Basic Principles and Techniques
In the following reaction sequence,
The major product B is:

Approach:
Identify the more strongly activating, ortho/para-directing group on the trisubstituted benzene and place the incoming bromine accordingly.
Step 1:Acetylation of the amine gives the acetanilide derivative A, bearing an NHCOCH3 group.
Step 2:The acetanilido group is more electron-donating (+M) than the methyl group, so it directs the electrophile.
Step 3:Bromination occurs ortho to the acetanilido group, giving product B.
Final answer: Option a (Br ortho to NHCOCH3, methyl para)
Q28Single correctOrganic Chemistry — Some Basic Principles and Techniques
SolutionAnswer: Option 3μA>μB and ke(B)>ke(A) Approach:
Compare the steric bulk of ethoxide (A) and tert-butoxide (B) to decide which favours elimination over substitution.
Step 1:Ethoxide is small and favours substitution, giving a large ratio of substitution to elimination.
Step 2:tert-Butoxide is bulky and favours elimination, lowering its substitution-to-elimination ratio.
Step 3:The bulky base B promotes elimination, so its elimination rate constant exceeds that of A.
μA>μB, ke(B)>ke(A)
Final answer: μA>μB and ke(B)>ke(A)
Q29Single correctBiomolecules
Which of the following statements is correct?
SolutionAnswer: Option 4Gluconic acid is a partial oxidation product of glucose Approach:
Recall the oxidation chemistry of glucose and the structure of gluconic acid to evaluate each statement.
Step 1:Mild oxidation of the aldehyde group of glucose with bromine water gives gluconic acid, a monocarboxylic acid.
Step 2:Strong oxidation with HNO3 gives the dicarboxylic glucaric (saccharic) acid, not gluconic acid.
Step 3:Gluconic acid lacks the free aldehyde, so it does not form a cyclic hemiacetal; it is a partial oxidation product of glucose.
Final answer: Gluconic acid is a partial oxidation product of glucose
Q30Single correctOrganic Chemistry — Some Basic Principles and Techniques
The correct order of stability for the following alkoxides is:

SolutionAnswer: Option 2(C) > (B) > (A) Approach:
Rank the alkoxides by the extent of delocalization of the negative charge by the nitro group and conjugation.
Step 1:In (A) the negative charge is stabilized only by the -I effect of the NO2 group.
Step 2:In (B) the charge is stabilized by delocalization over the double bond together with the -I effect of NO2.
Step 3:In (C) the charge is stabilized by the most extended conjugation, making it the most stable.
Final answer: (C) > (B) > (A)
Q31Single correctOrganic Chemistry — Some Basic Principles and Techniques
In the following reaction sequence, structures of A and B, respectively will be:

Approach:
Apply acidic ether cleavage by HBr followed by an intramolecular Wurtz coupling with sodium in ether.
Step 1:HBr cleaves the cyclic ether through an SN2 pathway to give the bromo-phenol A bearing a CH2Br side chain.
Step 2:Sodium in ether effects an intramolecular Wurtz coupling between the two C-Br centres, forming a carbocyclic ring fused to the phenol B.
Final answer: Option a
Q32Single correctOrganic Chemistry — Some Basic Principles and Techniques
A chromatography column, packed with silica gel as stationary phase, was used to separate a mixture of compounds consisting of (A) benzanilide, (B) aniline and (C) acetophenone. When the column is eluted with a mixture of solvents, hexane : ethyl acetate (20:80), the sequence of obtained compounds is:
SolutionAnswer: Option 2(C), (A) and (B) Approach:
On a polar silica stationary phase, the least polar compound elutes first; rank the three compounds by polarity.
Step 1:Acetophenone (dipole 3.05 D) is the least polar and elutes first.
Step 2:Benzanilide (dipole 2.71 D) elutes next.
Step 3:Aniline (dipole 1.59 D) is held most strongly and elutes last; however polarity order gives C, A, B as the elution sequence.
Final answer: (C), (A) and (B)
Q33Single correctCoordination Compounds
The number of possible optical isomers for the complexes [MA2B2] with sp3 and dsp2 hybridized metal atom, respectively, is:
Note: A and B are unidentate neutral and unidentate monoanionic ligands, respectively.
SolutionAnswer: Option 20 and 0 Approach:
Determine the geometry from the hybridization and check for a plane of symmetry that would make each complex optically inactive.
Step 1:For sp3 hybridization the geometry is tetrahedral; MA2B2 possesses a plane of symmetry and shows no optical activity.
Step 2:For dsp2 hybridization the geometry is square planar; MA2B2 has a plane of symmetry and is optically inactive.
Final answer: 0 and 0
Q34Single correctChemical Bonding and Molecular Structure
The bond order and magnetic characteristics of CN− are:
SolutionAnswer: Option 33, diamagnetic Approach:
Build the molecular orbital configuration of the 14-electron species CN− and compute the bond order and magnetic nature.
Step 1:CN− has 14 electrons with configuration filling through the bonding sigma 2p orbital.
σ1s2σ1s∗2σ2s2σ2s∗2π2px2π2py2σ2pz2
Step 2:Substituting the bonding and antibonding electron counts gives the bond order.
B.O.=21(10−4)=3
Step 3:All electrons are paired, so CN− is diamagnetic.
Final answer: 3, diamagnetic
Q35Single correctElectrochemistry
The equation which is incorrect is:
SolutionAnswer: Option 1Λm0NaBr−Λm0NaI=Λm0KBr−Λm0NaBr Approach:
Apply Kohlrausch's law of independent migration of ions to each combination and test the equality of ionic differences.
Step 1:Expanding option (a) gives a difference of bromide and iodide on the left but bromide-bound terms that do not cancel symmetrically on the right.
λI−0−λBr−0=λNa+0−λK+0
Step 2:Options (b), (c) and (d) reduce to identities under Kohlrausch's law, leaving (a) as the incorrect relation.
Final answer: Λm0NaBr−Λm0NaI=Λm0KBr−Λm0NaBr
Q36Single correctp-Block Elements
In the following reactions, product (A) and (B), respectively, are:
NaOH+Cl2→ (A) + side products (hot & conc.)
Ca(OH)2+Cl2→ (B) + side products (dry)
SolutionAnswer: Option 4NaClO3 and Ca(OCl)2 Approach:
Apply the disproportionation of chlorine with hot concentrated alkali and with dry slaked lime.
Step 1:Hot, concentrated sodium hydroxide with chlorine gives sodium chlorate as product A.
6NaOH+3Cl2→5NaCl+NaClO3+3H2O
Step 2:Dry slaked lime with chlorine gives bleaching powder, calcium hypochlorite, as product B.
2Ca(OH)2+2Cl2→Ca(OCl)2+CaCl2+2H2O
Final answer: NaClO3 and Ca(OCl)2
Q37Single correctSolutions
Two open beakers one containing a solvent and the other containing a mixture of that solvent with a non-volatile solute are together sealed in a container. Over time:
SolutionAnswer: Option 2the volume of the solution increases and the volume of the solvent decreases Approach:
Compare the vapour pressures of the pure solvent and the solution to determine the net direction of solvent transfer through the vapour phase.
Step 1:The pure solvent has a higher vapour pressure than the solution containing a non-volatile solute.
P0>Psoln
Step 2:Solvent evaporates from the pure-solvent beaker and condenses into the solution to equalize vapour pressures.
Step 3:Therefore the solution volume increases while the solvent volume decreases.
Final answer: the volume of the solution increases and the volume of the solvent decreases
Q38Single correctGeneral Principles and Processes of Isolation of Elements
The refining method used when the metal and the impurities have low and high melting temperatures, respectively, is:
SolutionAnswer: Option 3liquation Approach:
Match the description of a low-melting metal with high-melting impurities to the appropriate refining technique.
Step 1:When the metal melts at a lower temperature than its impurities, the metal can be melted and run off, leaving the impurities behind.
Step 2:This separation by selective melting is the process of liquation.
Final answer: liquation
Q39Single correctHydrogen
Among statements I-IV, the correct ones are:
I. Decomposition of hydrogen peroxide gives dioxygen
II. Like hydrogen peroxide, compounds, such as KClO3, Pb(NO3)2 and NaNO3 when heated liberate dioxygen.
III. 2-Ethylanthraquinone is useful for the industrial preparation of hydrogen peroxide.
IV. Hydrogen peroxide is used for the manufacture of sodium perborate.
SolutionAnswer: Option 1I,II, III and IV Approach:
Assess the validity of each statement about hydrogen peroxide and related dioxygen-liberating reactions.
Step 1:Hydrogen peroxide decomposes to liberate dioxygen.
2H2O2→2H2O+O2
Step 2:Thermal decomposition of the named salts liberates dioxygen.
2KClO3→2KCl+3O2
Step 3:The anthraquinone auto-oxidation route uses 2-ethylanthraquinone industrially.
Step 4:Hydrogen peroxide is used in synthesis of sodium perborate.
Na2B4O7+2NaOH+4H2O2→2NaBO3+5H2O
Final answer: I,II, III and IV
Q40Single correctRedox Reactions
The redox reaction among the following is:
SolutionAnswer: Option 3combination of dinitrogen with dioxygen at 2000 K Approach:
A redox reaction requires a change in oxidation states. Examine each option for oxidation-state changes.
Step 1:Ozone formation is allotrope interconversion of oxygen with no oxidation-state change of bonded O in the simplistic sense; the other options must be tested.
3O2→2O3
Step 2:Acid-base neutralisation involves no oxidation-state change.
2NaOH+H2SO4→Na2SO4+2H2O
Step 3:In the combination of dinitrogen with dioxygen, nitrogen goes from 0 to +2 and oxygen from 0 to -2.
Step 4:The reaction with silver nitrate is a double-displacement precipitation, not redox.
3AgNO3+[Co(H2O)6]Cl3→[Co(H2O)6](NO3)3+3AgCl
Final answer: combination of dinitrogen with dioxygen at 2000 K
Q41Single correctStates of Matter
Identify the correct labels of A, B and C in the following graph from the options given below:
Root mean square speed (Vrms); most probable speed (Vmp); average speed (Vav)

SolutionAnswer: Option 1A=Vmp,B=Vav,C=Vrms Approach:
Order the three characteristic speeds and assign them to the curve labels from left to right.
Step 1:Compare the numeric coefficients under the root.
Step 2:Therefore the speeds increase in the order most probable, average, root mean square.
Vmp<Vav<Vrms
Step 3:Reading the curve left to right, A is the smallest and C the largest.
Final answer: A=Vmp,B=Vav,C=Vrms
Q42Single correctChemical Kinetics
For the reaction,
2H2(g)+2NO(g)→N2(g)+2H2O(g)
The observed rate expression is, rate =kf[NO]2[H2]. The rate expression for the reverse reaction is:
SolutionAnswer: Option 3kb[N2][H2O]2/[H2] Approach:
Use the equilibrium condition that forward rate equals backward rate, with the equilibrium constant equal to the ratio of rate constants.
Step 1:At equilibrium the forward rate equals the backward rate.
kf[NO]2[H2]=rateback
Step 2:Express the backward rate using the equilibrium constant.
rateback=kb[H2][N2][H2O]2
Final answer: kb[N2][H2O]2/[H2]
Q43Single correctClassification of Elements and Periodicity
Within each pair of elements F & Cl, S & Se and Li & Na, respectively, the elements that release more energy upon an electron gain are:
SolutionAnswer: Option 2Cl, S and Li Approach:
Compare first electron gain enthalpies within each pair; the element with the more negative value releases more energy.
Step 1:For F and Cl, despite F being more electronegative, the small size of F gives stronger electron-electron repulsion, so Cl has the more negative electron gain enthalpy.
Step 2:For S and Se, going down the group the magnitude of electron gain enthalpy decreases, so S releases more energy.
Step 3:For Li and Na, Li has the more negative first electron gain enthalpy.
Final answer: Cl, S and Li
Q44Single correctCoordination Compounds
Among the following statements A-D, the incorrect ones are:
A. Octahedral Co(III) complexes with strong field ligands have high magnetic moments
B. When Δo<P, the d- electron configuration of Co(III) in an octahedral complex is t2g4.eg2.
C. Wavelength of light absorbed by [Co(en)3]3+ is lower than that of [CoF6]3−.
D. If the Δofor an octahedral complex of Co(III) is 18000 cm−1, the Δt for its tetrahedral complex with the same ligand will be16000 cm−1.
SolutionAnswer: Option 3A and D only Approach:
Evaluate each statement A-D about Co(III) octahedral complexes and crystal field splitting to find the incorrect ones.
Step 1:Statement A: strong field ligands give low-spin Co(III), which has low magnetic moment, so A is incorrect.
Step 2:Statement D: the tetrahedral splitting is four-ninths of the octahedral value.
Δt=94×18000=8000 cm−1
Step 3:The other statements are consistent, so the incorrect ones are A and D.
Final answer: A and D only
Q45Single correctSome Basic Concepts of Chemistry
The ammonia (NH3) released on quantitative reaction of 0.6 g urea (NH2CONH2) with sodium hydroxide (NaOH) can be neutralized by:
SolutionAnswer: Option 4100 mL of 0.2 N HCl Approach:
Find moles of ammonia from the stoichiometry of urea with NaOH, then equate to moles of HCl required.
Step 1:Compute moles of urea using its molar mass of 60.
600.6=0.01
Step 2:Each mole of urea gives two moles of ammonia.
0.01×2=0.02
Step 3:Equate to moles of HCl: 100 mL of 0.2 N HCl supplies 0.02 mol.
0.2×1000100=0.02
Final answer: 100 mL of 0.2 N HCl
Q46NumericalBiomolecules
Number of sp2 hybrid carbon atoms present in aspartame is ___.
Approach:
Count carbons in aspartame that are sp2 hybridised: the aromatic ring carbons and the carbonyl carbons.
Step 1:The benzene ring contributes six sp2 carbons.
Step 2:The three carbonyl carbons (one ester, one amide, one carboxylic acid) are sp2.
Step 3:Add the sp2 carbons.
6+3=9
Final answer: 9
Q47NumericalIonic Equilibrium
3 grams of acetic acid is added to250 mL of 0.1 M HCl and the solution is made up to 500 mL. To 20 mL of this solution 21 mL of 5 M NaOH is added. The pH of this solution is___.
(Given: log 3 = 0.4771, pKa of acetic acid = 4.74, molar mass of acetic acid = 60 g/mole).
Approach:
Determine the millimoles of acetic acid, HCl and NaOH in 20 mL, neutralise the strong acid first, then form the acetate buffer and apply the Henderson-Hasselbalch equation.
Step 1:In 20 mL: acetic acid is 2 mmol, HCl is 1 mmol, NaOH is 2.5 mmol.
Step 2:NaOH first neutralises HCl (1 mmol), leaving 1.5 mmol NaOH to react with acetic acid.
HCl+NaOH→NaCl+H2O
Step 3:1.5 mmol NaOH converts acetic acid to acetate, leaving 0.5 mmol acid and 1.5 mmol salt.
CH3COOH+NaOH→CH3COONa+H2O
Step 4:Apply Henderson-Hasselbalch.
pH=4.74+log0.51.5=4.74+log3=4.74+0.48=5.22
Final answer: 5.22
Q48NumericalSurface Chemistry
The flocculation value of HCl for arsenic sulphide sol is 30 mmolL−1. If H2SO4 is used for the flocculation of arsenic sulphide, the amount, in grams, of H2SO4 in 250 mL required for the above purpose is ___.
Approach:
Match the equivalent flocculating power: the same number of millimoles of effective ions as the HCl flocculation value, then convert to mass of sulphuric acid in 250 mL.
Step 1:For 1 L of sol, 30 mmol of HCl are required, corresponding to 15 mmol of H2SO4.
Step 2:For 250 mL the requirement is one quarter.
415×98×10−3 g
Step 3:Evaluate the mass.
415×98×10−3=0.3675
Final answer: 0.3675
Q49NumericalThe d- and f-Block Elements
Consider the following reactions :
NaCl+K2Cr2O7+H2SO4→ (A) + side products
(A) + NaOH → (B) + side products
(B) + H2SO4(dil.) + H2O2→ (C) + side products
The sum of the total number of atoms in one molecule of (A), (B) & (C) is ___.
Approach:
Identify the chromium products A, B and C from the chromyl chloride test sequence and add up the atoms in each molecule.
Step 1:NaCl with dichromate and sulphuric acid gives chromyl chloride (A).
(A)=CrO2Cl2
Step 2:Chromyl chloride with NaOH gives sodium chromate (B).
(B)=Na2CrO4
Step 3:Sodium chromate with dilute sulphuric acid and hydrogen peroxide gives chromium peroxide (C).
(C)=CrO5
Step 4:Add the atom counts.
5+7+6=18
Final answer: 18
Q50NumericalThermodynamics
The standard heat of formation (ΔfH298∘) of ethane (in kJ/mol), if the heat of combustion of ethane, hydrogen and graphite are -1560, -393.5 and -286 kJ/mol, respectively, is___.
Approach:
Apply Hess's law by combining the combustion reactions to construct the formation reaction of ethane.
Step 1:Combustion of graphite, hydrogen and ethane are given with their enthalpies.
C+O2→CO2, −286
Step 2:Invert ethane combustion and add two graphite and three hydrogen combustions.
2(−286)+3(−393.5)−(−1560)
Step 3:Evaluate the sum.
−572−1180.5+1560=−192.5
Final answer: -192.5