CBSE Sample Papers for Class 12 Chemistry Set 2 with Solutions

Students must start practicing the questions from CBSE Sample Papers for Class 12 Chemistry with Solutions Set 2 are designed as per the revised syllabus.

CBSE Sample Papers for Class 12 Chemistry Set 2 with Solutions

Time: 3 hrs
Max. Marks: 70

General Instructions

Read the following instructions carefully.

1. There are 33 questions in this question paper with internal choice.
2. Section A consists of 16 multiple-choice questions carrying 1 mark each.
3. Section B consists of 5 short answer questions carrying 2 marks each.
4. Section C consists of 7 short answer questions carrying 3 marks each.
5. Section D consists of 2 case-based questions carrying 4 marks each
6. Section E consists of 3 long answer questions carrying 5 marks each.
7. All questions are compulsory.

Section A
(The following questions are multiple-choice questions with one correct answer. Each question carries 1 mark. There is no internal choice in this section.)

Question 1.
For d⁴ ions, the fourth electron enters one of the e_g-orbitals giving the configuration \(t_{2 g}^3 e_g^1\), when [1]
(a) ∆₀ > P
(b) ∆₀ < P
(c) ∆₀ = P
(d) ∆₀ ≥ P
Answer:
(b) ∆₀ < P

The fourth electron enters one of theeg-orbitals giving the configuration \(t_{2 g}^3 e_g^1\) when ∆₀ < P.

Question 2.
The product formed during Hell-Volhard-Zelinsky reaction is [1]


Answer:
(a)

Carboxylic acids having an a-hydrogen are halogenated at the a-position on treatment with chlorine or bromine in the presence of small amount of red phosphorus to give a-halocarboxylic acids. This reaction is known as Hell-Volhard-Zelinsky reaction.

Question 3.
The pair of bases in DNA are held together by [1]
(a) ionic bonds
(b) H-bond
(c) phosphate group
(d) deoxyribose group
Answer:
(b) H-bond
The pair of bases in DNA are held with each other by H-bonds.

Question 4.
Which of the following is the most polar compound? [1]
(a) Propanone
(b) Formaldehyde
(c) Propanal
(d) Hexan-3-one
Answer:
(b) Formaldehyde
Among the given compounds, formaldehyde is the most polar due to lowest electron density on C of carboxyl group, whereas in all other cases, the electron density on C is high due to +I effect of alkyl groups.

Question 5.
Identify A B and C in the given sequence of reactions, [1]

Answer:
(b) Addition of bromine in Ccl₄ to an alkene results in discharge of reddish brown colour of bromine. It is an important method for detection of double bond in a molecule.
The electrophilic addition results in the synthesis of vic-dibromictes, which are colourless.

Question 6.
Match the properties with the elements of 3d-series: [1]

(a) (i) – (r), (ii) – (p), (iii) – (q)
(b) (i) – (r), (ii) – (s), (iii) – (p)
(c) (i) – (p), (ii) – (q), (iii) – (r)
(d) (i) – (s), (ii) – (r), (iii) – (p)
Answer:
(a) (i) – (r), (ii) – (p), (iii) – (q)
(i) Osmium(Os) has an oxidation state starting from +2 to +8.
(ii) Mn [Ar] 3d⁵4s² shows +2, +3, +4, + 5, +6 and +7 oxidation state, maximum number in 3d-series.
(iii) Chromium(Cr) has the highest melting point due to its half-filled stable d-orbital and the unpaired electrons form strong intermetallic bonds which are difficult to break immediately.

Question 7.
For a hypothetical reaction, R → P; Rate = -k[R]. The negative sign used in the rate expression indicates [1]
(a) decrease in the concentration of reactant with time.
(b) decrease in the concentration of product with time.
(c) reaction is reversible.
(d) decrease in the rate with time.
Answer:
(a) decrease in the concentration of reactant with time.
For the given reaction, the negative sign indicates the decrease in concentration of reactants with time.

Question 8.
Which of the following is not correct for amines? [1]
(a) Ethyl methylamine cannot be prepared by Gabriel phthalimide synthesis.
(b) N-ethylbenzene sulphonamide is insoluble in alkali.
(c) Amines are less volatile than hydrocarbons.
(d) Amides can be converted into amines with same number of carbon atoms by LiAlH₄ /ether.
Answer:
(b) N-ethylbenzene sulphonamide is insoluble in alkali.
N-ethylbenzene sulphonamide is soluble in alkali because hydrogen attached to nitrogen in sulphonamide is strongly acidic and forms a salt during reaction between these two.

Question 9.
Hydroboration oxidation of 4-methyloctene would give [1]
(a) 4-methyloctanol
(b) 2-methyldecane
(c) 4-methylheptanol
(d) 4-methyl-2-octanone
Answer:
(a) 4-methyloctanol
Terminal alkenes react rapidly with diborane to form primary trialkyl boranes which on oxidation gives primary alcohols.

(In general, hydroboration oxidation involves the addition of water according to anti-Markownikoff’s rule).

Question 10.
The half-life period of a first order reaction is 4 minutes, the time after which 99.9% reaction gets completed is [1]
(a) 16 min
(b) 8 min
(c) 32 min
(d) 40 min
Answer:
(d) 40 min
Given, t_1/2 = 4min and a = 100; a – x = 0.1
Now, t_1/2 = \(\frac{0.693}{k}\) [For first order reaction]
∴ k = \(\frac{0.693}{4}\) …… (i)
As we know that, k = \(\frac{2.303}{t}\)log\(\frac{a}{a-x}\)
t = \(\frac{2.303 \times 4}{0.693}\)log\(\frac{100}{0.1}\) [From Eq.(i)]
t = 39.88 min ≈ 40 min

Question 11.
Boiling point of alcohol is comparatively higher than that of corresponding alkane due to [1]
(a) intermolecular hydrogen bonding
(b) intramolecular hydrogen bonding
(c) volatile nature
(d) None of the above
Answer:
(a) intermolecular hydrogen bonding
Due to intermolecular hydrogen bonding in alcohols, they exist as associated molecules.
Consequently, a large amount of energy is required to break these bonds and, therefore, their boiling points are higher than that of the corresponding hydrocarbons (hydrogen bonding is absent in hydrocarbons).

Question 12.
Which type of electrolyte are used in A and B ? [1]

Answer:
(a) In the given graph, ‘A’ represents weak electrolyte like CH₃COOH as Λ_m increases steeply on dilution at low concentration region and ‘6 ’ represents strong electrolyte like NaCl as Λ_m increases slowly with dilution.

Direction (Q. Nos. 13-16) In the following questions as Assertion (A) is followed by a corresponding Reason (R). Use the following keys to choose the appropriate answer.
(a) Both (A) and (R) are true, (R) is the correct explanation of (A).
(b) Both (A) and (R) are true, (R) is not the correct explanation of (A).
(c) (A) is true, (R) is false.
(d) (A) is false, (R) is true.

Question 13.
Assertion (A) p-nitrophenol is more acidic than phenol.
Reason (R) Nitro group helps in the stabilisation of the phenoxide ion by dispersal of negative charge due to resonance. [1]
Answer:
(a) Both (A) and (R) are true, (R) is the correct explanation of (A).

Question 14.
Assertion (A) In electrolysis, the quantity of electricity needed for depositing 1 mole of silver is different from that required for 1 mole of copper.
Reason (R) The molecular weights of silver and copper are different. [1]
Answer:
(b) Both (A) and (R) are true, (R) is not the correct explanation of (A).
According to Faraday’s law of electrolysis the weight of ion deposited on an electrode is directly proportional to the quantity of electricity passed. So, 1 mole of silver = 1g equivalent of silver and 1 mole of copper = 2g equivalent of copper.

Question 15.
Assertion (A) All naturally occurring α-amino acids except glycine are optically active.
Reason (R) Most naturally occurring amino acids have L-configuration. [1]
Answer:
(b) Both (A) and (R) are true, (R) is not the correct explanation of (A).
All naturally occurring α-amino acids except glycine are optically active. Glycine is optically inactive because glycine does not have all four different substituents as shown below.

Question 16.
Assertion (A) The a-hydrogen atom in carbonyl compounds is less acidic.
Reason (R) The anion formed after the loss of a-hydrogen atom is resonance stabilised. [1]
Answer:
(d) (A) is false, (R) is true.

(A) is false because the a-hydrogens in carbonyl compounds are generally acidic in nature and there will be an easy loss of these in form of H⁺ ions.
The anion formed after loss of α-hydrogen atom is resonance stabilised.

Section B
(This section contains 7 questions with internal choice in one question. The following questions are very short answer type and carry 2 marks each.)

Question 17.
At first order reaction is 25% complete in 40 minutes.
(a) Calculate the value of rate constant.
(b) In what time will the reaction be 80% completed? [2]
Answer:
(a) For first order reaction,
k = \(\frac{2.303}{t}\)log\(\frac{a}{a-x}\)
The given first order reaction completes 25% in 40 min.
Let a = 100
a – x = 100 – 25 = 75
∴ k = \(\frac{2.303}{40}\)log \(\frac{100}{75}\) = \(\frac{2.303}{40}\)(log 4 – log 3)
k = 0.0072 min^-1

(b) For 80% completion of reaction,
a = 100
a – x = 100 – 80 = 20
k = 0.0072 min^-1
t = \(\frac{2.303}{0.0072}\)log\(\frac{100}{20}\) = 223.6 min

Question 18.
A solution containing 25.6 g of sulphur dissolved in 1000 g of naphthalene, whose melting point is 80.1°C gave a freezing point lowering of 0.680°C. Calculate the molecular weight of sulphur, K_f for naphthalene is 6.8 K kg mol^-1. [2]
Answer:
∆T_f = K_f ∙ m = K_f ∙ \(\frac{W_B}{M_B \cdot W_A(\text { in kJ })}\)
0.68 = 6.8 × \(\frac{25.6}{M_B}\) × \(\frac{1000}{1000}\)
M_B = \(\frac{6.8 \times 25.6}{0.68}\) = 256 g

Question 19.
(a) Name the suitable haloarene and reagent from which 2-chloroacetophenone can be prepared.
(b) Out of chlorobenzene and cyclohexyl chloride, which one has higher dipole moment? [2]
Answer:
(a) 2-chloroacetophenone can be obtained from chlorobenzene and acetyl chloride in the presence of anhyd. AlCl₃.

(b) In chlorobenzene, the Cl-atom is linked to a sp²-hybridised carbon atom, whereas in cyclohexyl chloride, the Cl-atom is linked to a sp³-hybridised
carbon atom.
As, sp²-hybridised carbon has more s-character so, it is more electronegative, thus the density of electrons of C—Cl bond near the Cl-atom is less in chlorobenzene than in cyclohexyl chloride.
Hence, the C—Cl bond of cyclohexyl chloride is more polar, i.e. it has higher dipole moment.

Question 20.
(a) Give chemical tests to distinguish between phenol and benzoic acid. [2]
(b) Write IUPAC name of

Or
Convert the following. [2]
(a) Ethyl cyanide to ethanoic acid
(b) Butan-l-ol to butanoic acid
Answer:
(a) Phenol and benzoic acid can be distinguished by ferric chloride test. Phenol reacts with neutral FeCl₃ to form ferric phenoxide complex giving violet colouration.

But benzoic acid reacts with neutral FeCl₃ to give a buff coloured precipitate of ferric benzoate.

Question 21.
(a) Account for the following. [2]
Pentaacetate of glucose does not react with hydroxyl amine.
(b) What happens when oxidation of gluconic acid takes place?
Answer:
(a) “Pentaacetate of glucose does not react with hydroxylamine” due to the absence of free CHO group.
(b) Glucose and gluconic acid, both on oxidation yields a dicarboxylic acid, saccharic acid.
Reaction involved is as follows

Section C
(This section contains 7 questions with internal choice in one question. The following questions are short answer type and carry 3 marks each.)

Question 22.
(a) What kind of isomerism exists between [Cr(H₂O)₆]Cl₃ (violet) and [Cr(H₂O)₅Cl]Cl₂ ∙ H₂O (greyish-green)? [3]
(b) Write the formula of diamminechlorido- nitrito-N-platinum (II).
(c) Different colours observed in octahedral and tetrahedral complexes for the same metal and same ligands. Explain.
Answer:
(a) Coordination compound [Cr(H₂O)₆]Cl₃ and [Cr(H₂O)₅Cl]Cl₂ ∙ H₂O are solvate isomers, because water is exchanged by chloride ion. This is why both of them show different colour on exposure to sunlight.
(b) The formula is [Pt(NH₃)₂Cl(NO₂)].
(c) Crystal field splitting energy in the octahedral and tetrahedral field are closely related as
∆_t = \(\left(\frac{4}{9}\right) \Delta_0\)
Higher the CFSE, higher will be the energy radiated in d-d transition.
Hence, lower wavelength is absorbed in octahedral complex than tetrahedral complex for the same metal and ligands. Thus, different colours are observed.

Question 23.
(a) What happens if external potential applied becomes greater than E°_cell of electrochemical cell? [3]
(b) Write the relation among the conductivity of a solution in the cell constant and the resistance of solution in the cell.
(c) The resistance of a conductivity cell containing 0.001 M KCl solution at 298 K is 1500 Ω. What is the cell constant if the conductivity of 0.001 M KCl solution at 298 K is 0146 × 10^-3 S cm^-1?
Answer:
(a) When external potential applied becomes greater than E°_cell of electrochemical cell, electrons flow from cathode to anode, i.e. electrolytic cell.

(b) The resistance, R of a conductor varies directly with length (l) and inversely with area of cross-section A,
i.e. R ∝ \(\frac{1}{A}\)
or R = \(\rho \frac{1}{A}\)
where ρ = resistivity ρ = \(\frac{R A}{1}\)

(c) Given, conductivity, \(\kappa\) = 0.146 × 10^-3 S cm^-1
Resistance, R = 1500Ω
∴ Cell constant, G* = K × R
= 0.146 × 10^-3 × 1500
= 0.219 cm^-1

Question 24.
Write the equation for the following reactions. [3]
(a) Conversion of propan-2-ol to 2-methyl propan-2-ol
(b) Phenol is treated with Na₂Cr₂O₇ in the presence of sulphuric acid.
Answer:
(a) Propan-2-ol to 2-methylpropan-2-ol

Oxidation of phenol is done with Na₂Cr₂O₇ in the presence of sulphuric acid and benzoquinone is formed along with water.

Question 25.
An organic compound (P) having molecular formula C₉H₁₀O forms an orange precipitate (Q) with 2, 4-DNP reagent. Compound (P) gives a yellow precipitate (R) when heated in the presence of iodine and NaOH along with colourless compound (S).
Identify (P), (Q), (R) and (S). Write down the reaction for their formation. [3]

Or

An unknown aldehyde ‘A’ on reacting with alkali gives a β-hydroxy aldehyde, which loses water to form an unsaturated aldehyde, but-2-enal.
Another aldehyde ‘B’ undergoes disproportionation reaction in the presence of conc. alkali to form products C and D. C is an aryl alcohol with the formula C₇H₈O. Identify A and B. Write the sequence of reactions involved. [3]
Answer:
P = Phenyl acetone
Q = 2, 4-dinitrophenyl hydrazone
R = Methyl iodide
S = Phenyl acetic acid

Or

A is CH₃CHO (ethanal).
B is C₆H₅CHO (benzaldehyde).

Question 26.
A simplified version of nucleic acid chain is as shown below. [3]

(a) Write the main structural difference between nucleoside and nucleotide.
(b) How do two nucleic acid chains bond with each other?
(c) Name the bases present in DNA.
Answer:
(a) Nucleosides contain only sugar and a base, whereas nucleotides contain sugar, base and a phosphate group as well.
(b) Two nucleic acid chains are held together by hydrogen bonds between pairs of bases.
(c) There are four nucleotides, or bases, in DNA: adenine (A), cytosine (C), guanine (G), and thymine (T).

Question 27.
An alcohol having formula C₂H₆O reacts with HBr and forms products. Write the name and structure of both products and the mechanism of the reaction. [3]
Answer:
The involved chemical reaction is

The mechanism of the given reaction is as follows
step 1 HBr → H⁺ + Br^–
Step 2 Protonation of alcohol

Step 3 Nucleophilic attack of Br^–

Question 28.
Prove that time required to complete 3/4 of a first order reaction is twice its half-life period. [3]
Answer:
For first order reaction, rate constant

Thus, time needed to compare 3/4 of reaction is twice its half-life period.

Section D
(The following questions are case-based questions. Each question has an internal choice and carries 4(1+1+2) marks each. Read the passage carefully and answer the questions that follow.)

Question 29.
Crystal field theory is a theory that describes the breaking of the degeneracy of electronic orbitals that occurs in transition metal coordination complexes, most often as a consequence of the presence of ligands.
Crystal field splitting energy (CFSE) is the parameter that is used to correlate a variety of spectroscopic, thermodynamic, and magnetic properties of complexes. The essential feature of crystal field theory is that there is a competition between the magnitude of the CFSE and the pairing energy, which is the energy required to accommodate two electrons in one orbital.
The energy splitting is shown schematically in the figure given below.

Answer the following questions. [4]

(a) On the basis of this theory, write the electronic configuration of d⁴ system in terms of t_2g and e_g if ∆₀ < P.

Or

Write the electronic configuration of the central atom K₄[Fe(CN)₆] w.r.t crystal field theory. [4]
(b) What is the crystal field stabilisation energy for high spin d⁴ octahedral complex?
(c) How does the magnitude of the splitting decide the actual configuration of d-orbitals in an octahedral field for a coordination entity?
Answer:
(a) If ∆₀ < P, the fourth electron enters one of the eg orbitals giving the configuration \(t_{2 g}^3 e_g^1\).

Or

The electronic configuration of the central atom is K₄[Fe(CN]₆ on the basis of crystal field theory is \(t_{2 g}^6 e_g^0\)

(b) CFSE = 3(-0.4)∆₀ + 0.6∆₀
= -1.2∆_o + 0.6∆_o = -0.6∆₀

(c) The magnitude of splitting decides the actual configuration of d-orbital in an octahedral field for a coordination entity on the following basis.
If ∆_o < P (P is the energy required for pairing of electrons), then fourth electron enters one of the e_g orbitals giving the configuration \(t_{2 g}^3 e_g^1\). It means first four orbitals are singly occupied and no pairing will take place, forming high spin complexes. Such ligands for which ∆₀ < P are called weak field ligands.

If ∆₀ > P, the 4^th electron pairs up in one of the t_2g orbitals giving the configuration \(t_{2 g}^4 e_g^0\) thereby forming low spin complexes. Such ligands for which
∆₀ > P are called strong field ligands.

Question 30.
Electrochemical cell potentials have no simple relationship with temperature but depend on the interplay between the sign and magnitude of the isothermal temperature coefficient, dE°/dT, and on the magnitude of the reaction quotient, Q. An electrochemical cell is said to act reversibly if the net cell reaction is reversed when the current through the cell is made to flow in the opposite direction.

When no current is being drawn, such a cell is in a true equilibrium state. When no current is being drawn from a reversible cell, the potential difference across its terminal, or open-circuit potential, is known as the electromotive force or emf of the cell.

The emf of any particular reversible cell is a quantitative measure of the tendency of the cell reaction to occur and may be related to the free energy change for this process.

The Daniell cell is a type of electrochemical cell invented in 1836 by John Frederic Daniell, a British chemist and meteorologist, and consists of a copper pot filled with a copper (II) sulphate solution, in which is immersed an unglassed earthenware container filled with sulphuric acid and a zinc electrode.

Several scientists performed experiments that used a Daniell galvanic cell working in different electrolyte concentrations for comparing results with the theoretical values calculated by the Nernst equation. The cell potential decreases drastically when the Cu²⁺ concentration was reduced and the temperature was above 80°C.

In addition, temperature indirectly has an influence through the activity coefficients, ionic strength and dilution of the solution.

Answer the following questions. [4]

(a) An electrochemical cell generally consists of a cathode and an anode. Where is the reduction takes place?
(b) What is the effect of increase in concentration of zinc ions on the electrode potential of zinc electrode for which \(E_{\mathrm{Zn}^{2+} / \mathrm{Zn}}^{\circ}\) equals -0.76 V ?
(c) How does the reduction potential increase w.r.t. Nernst equation?

Or

Imagine you are a member of a project based on electrochemical cell and you are asked to construct an electrochemical cell. What will be its main four components? [4]
Answer:
(a) Cathodes are usually metal electrodes. It is the electrode where reduction takes place.
(b) According to Nernst equation, the electrode potenial of zinc depends on the concentration of zinc ions.

Hence, electrode potential will increase with increase in concentration of Zn²⁺ ions.
(c) For the electrode reaction,

∴ Electrode potential can be increased either by increasing metal ion concentration, [Mⁿ⁺] or temperature T.

Or

The four components of an electrochemical cell are as follows
(a) Anode An electrode where oxidation occurs.
(b) Cathode An electrode where reduction occurs.
(c) Electrolyte An electrolyte is a charged mobile ion that functions as a conducting medium.
When dissolved in polar solvents such as water, an electrolyte produces ions, resulting in an electrically conducting solution.
(d) Salt-bridge A salt-bridge connects the oxidation and reduction halves of an electrochemical cell, completing the electrochemical circuit. It contains a saturated salt solution, such as KCl.

Section E
(The following questions are long answer type and carry 5 marks each. All questions have an internal choice.)

Question 31.
Attempt any five of the following. [5]
(a) Why Mn²⁺ is more stable than Fe²⁺ towards +3 oxidation state?
(b) Why the enthalpy of atomisation is lowest for Zn in 3d-series of the transition elements?
(c) Identify the metal in MO₃F and justify your answer.
(d) Explain why transition metals form a large number of complexes.
(e) Why the E° value for the Mn³⁺ /Mn²⁺ couple is much more positive than that for Cr³⁺ /Cr²⁺ couple?
(f) Complete the following.
3Mn\(\mathrm{O}_4^{2-}\) + 4H⁺ →
(g) Which of the following cations are coloured in aqueous solution and why?
Sc³⁺, V³⁺, Ti⁴⁺, Mn²⁺
Answer:
(a) Electronic configuration of Mn²⁺ = [Ar]₁₈3d⁵
Electronic configuration of Fe²⁺ = [Ar]₁₈3d⁶
Mn²⁺ having half-filled d-orbitals will be more stable than Fe²⁺, as it has half-filled d-orbitals.
(b) Zinc has completely filled d-orbitals, which limits its tendency to form metallic bonds. Thus, it requires least enthalpy to get atomised.
(c) MO₃F is MnO₃F. In MO₃F,
Let the oxidation state of M is x.
x + 3 × (-2) + (-1) = 0
or, x = + 7, i.e. M is in oxidation state of +7. Hence, the given compound is MnO₃F.
(d) Transition elements form a large number of complexes due to the comparatively smaller sizes of the metal ions, their high ionic charges and the availability of d-orbitals for bond formation.
(e) The value of \(E_{\mathrm{Cr}^{3+} / \mathrm{Cr}^{2+}}^{\circ}\) is negative (-0.4 V).
It shows the stability of \(E_{\mathrm{Cr}^{3+}}^0\) ions in solution cannot be reducing agent of Mn³⁺ has high positive value due to extra stability of half-filled electronic configuration. Thus, Cr³⁺ is the most stable, Mn³⁺ is least stable.
(f) 3Mn\(\mathrm{O}_4^{2-}\) + 4H⁺ → 2Mn\(\mathrm{O}_4^{-}\) + MnO₂ + 2H₂O
(g) Electronic configurations of the ions are :
Sc³⁺ = [Ar]3d⁰4s⁰, V³⁺ = [Ar]3d²4s⁰,
Ti⁴⁺ = [Ar]3d⁰4s⁰, Mn²⁺ = [Ar]3d⁵4s⁰
Only V³⁺ and Mn²⁺ can undergo d-d transition, hence they are coloured, while Ti⁴⁺ and Sc³⁺ do not have any electron, thus they are colourless.

Question 32.
(a) Gas (A) is more soluble in water than gas (B) at the same temperature. Which one of the two gases will have the higher value of K_H (Henry’s constant) and why?
(b) In non-ideal solution, what type of  deviation shows the formation of maximum boiling azeotropes?
(c) What type of azeotropic mixture will be formed by a solution of acetone and chloroform? Justify on the basis of strength of intermolecular interactions that develop in the solution. [5]

Or

(a) How is the vapour pressure of a solvent affected when a non-volatile solute is dissolved in it?
(b) When 2.56 g of sulphur was dissolved in 100 g of CS₂, the freezing point gets lowered by 0.383 K. Calculate the formula of sulphur (S_x).
(K_f for CS₂ = 3.83 K kg mol^-1,
Atomic mass of sulphur =32 g mol^-1) [5]
Answer:
Solubility is inversely proportional to K_H, i.e. Henry’s constant of the gas.
(a) Greater the value of K_H, lower is the solubility of the gas. As gas (A) is more soluble in water than gas (B) at the same temperature, hence the gas (A) has lower value of K_H. In other words, gas (B) has higher value of K_H than gas (A) at the same temperature.
(b) In non-ideal solutions, the solutions that show large negative deviation from Raoult’s law form maximum boiling azeotropes, e.g. Mixture of nitric acid and water.
(c) The mixture of acetone and chloroform is an example of maximum boiling azeotrope. It shows negative deviation from Raoult’s law because of increase in intermolecular forces of attraction between acetone and chloroform, since they form hydrogen bonds between them.

Or

(a) When a non-volatile solute is added to a solvent, its vapour pressure decreases because some of the surface sites are occupied by solute molecules. Thereby, the fraction of the surface covered by the solvent molecules gets reduced.
Thus, less space is available for the solvent molecules to vaporise. Therefore, vapour pressure is also reduced.

(b) Given, Weight of solvent (W₁) = 100g
Weight of solute (w₂) = 2.56 g

Question 33.
(a) Give reasons for the following observations.
(i) Aniline is a weaker base than cyclohexyl amine.
(ii) It is difficult to prepare pure amines by ammonolysis of alkyl halides.
(iii) Ethylamine is soluble in water, whereas aniline is not soluble in water.
(b) Arrange the following in
(i) increasing order of their solubility in water.
C₆H₅NH₂, C₂H₅NH₂, (C₂H₅)₂NH
(ii) increasing order of basic strength. Aniline, p-nitroaniline and p-toluidine [5]

Or

An organic compound A’ with molecular formula C₆H₇N is treated with NaNO₂ and dil. HCl and compound ‘B’ is formed. The compound ‘B’ further reacts with H₃PO₂ and water, an aromatic compound ‘C’ is formed. On Friedel-Crafts alkylation, the compound ‘C’ gets converted into compound ‘D’ having molecular formula C₇H₈. In the presence of sunlight, this compound gets converted into another compound Write the structure of compounds A to E. Write the chemical equations involved. [5]
Answer:
(a) (i) In aniline, the lone pair present on nitrogen is involved in delocalisation. Thus, electrons are not available for donation. There is no such delocalisation in cyclohexylamine. Hence, aniline is weaker base than cyclohexylamine.
(ii) It is difficult to prepare pure amines by ammonolysis of alkyl halides because it is a nucleophilic substitution reaction and ammonia behaves as a nucleophile to form 1° amine.
Now, this T amine behaves as a \(\mathrm{Nu}^{\ominus}\) and reacts with alkyl halide to give 2° amine, which on further reaction yields 3° amine and quaternary ammonium salt.
(iii) Solubility of compound in water, depends on H-bonding. Bulkiness of the group attached to such bond decreases the extent of H-bonding.
Aniline is not soluble in water, while ethylamine is soluble. This is because ethylamine forms intermolecular hydrogen bonds with water, while in aniline, the aryl group possesses steric hindrance and also high molar mass and hence, does not resuit in the formation of H-bonding. (1)

(b) (i) C₆H₅NH₂ < (C₂H₅)₂NH < C₂H₅NH₂
Aromatic amines are insoluble in water because of bulky hydrocarbon part (hydrophobic) which retards the formation of H-bonding. However, increase in size of hydrophobic alkyl part in aliphatic amines decreases solubility in water.
(ii) p-nitroaniline < aniline < p-toluidine.
The presence of electron-donating —CH₃ group increases the electron density on N-atom in p-toluidine. Hence, p-toluidine is more basic than aniline. In p-nitroaniline, —NO₂ group decreases the electron density over the N-atom. Hence, p-nitroaniline is less basic than aniline.

Or

A = Aniline;
B = Benzene diazonium chloride;
C = Benzene;
D = Toluene and
E = Benzyl chloride.