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CBSE Class 12 Chemistry 2024 question paper (56/3)

Maximum marks 70 · Time 3 hours · 3 sets

Try each question first, then open its model answer. Where the paper offers a choice, both questions are shown with OR between them.

Section A

1 mark each

  1. Q.11 mark
    Which of the following does not show variable oxidation states ?

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  2. Q.21 mark
    The type of isomerism shown by the complex [CoCl2(en)2]+[\mathrm{CoCl_2(en)_2}]^{+} is :

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  3. Q.31 mark
    Which of the following is diamagnetic in nature ? [Atomic number : Co = 27]

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  4. Q.41 mark
    Consider the following reaction : Cl−C6H4−CH2−Cl→KCN?\mathrm{Cl-C_6H_4-CH_2-Cl} \xrightarrow{\mathrm{KCN}} ? The major product of the reaction is :

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  5. Q.51 mark
    Which one of the following compounds has the lowest pKa\mathrm{pK_a} value ?

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  6. Q.61 mark
    (CH3)2CH−O−CH3\mathrm{(CH_3)_2CH-O-CH_3} when treated with HI gives :

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  7. Q.71 mark
    Which of the following compounds on treatment with benzene sulphonyl choride forms an alkali-soluble precipitate ?

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  8. Q.81 mark
    The order of increasing basicities of CH3NH2\mathrm{CH_3NH_2} (I), (CH3)2NH\mathrm{(CH_3)_2NH} (II), (CH3)3N\mathrm{(CH_3)_3N} (III) and C6H5NH2\mathrm{C_6H_5NH_2} (IV) in aqueous media is :

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  9. Q.91 mark
    The vitamin which plays an important role in coagulating blood is :

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  10. Q.101 mark
    When a catalyst increases the rate of a chemical reaction, then the rate constant (k) :

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  11. Q.111 mark
    A 1% solution of solute 'X' is isotonic with a 6% solution of sucrose (molar mass = 342 g mol−1\mathrm{mol^{-1}}). The molar mass of solute 'X' is :

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  12. Q.121 mark
    During the electrolysis of aqueous NaCl, the cathodic reaction is :

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  13. For Questions number 13 to 16, two statements are given — one labelled as Assertion (A) and the other labelled as Reason (R). Select the correct answer to these questions from the codes (A), (B), (C) and (D) as given below.
    Q.131 mark
    Assertion (A) : Addition of ethylene glycol to water lowers its freezing point. Reason (R) : Ethylene glycol is insoluble in water due to lack of its ability to form hydrogen bonds with water molecules.

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  14. Q.141 mark
    Assertion (A) : Order of reaction and molecularity are always same for complex reactions. Reason (R) : Order is determined experimentally and molecularity is applicable only for elementary reactions.

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  15. Q.151 mark
    Assertion (A) : The boiling point of ethanol is higher than that of dimethyl ether. Reason (R) : Ethanol molecules are associated through hydrogen bonding whereas in dimethyl ether, it is not possible.

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  16. Q.161 mark
    Assertion (A) : Aniline does not undergo Friedel-Crafts reaction. Reason (R) : Friedel-Crafts reaction is an electrophilic substitution reaction.

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Section B

2 marks each

  1. Q.17 (a)2 marks
    Define molal depression constant. How is it related to enthalpy of fusion ?
  2. OR

    Q.17 (b)2 marks
    What type of deviation is shown by ethanol and acetone mixture ? Give reason. What type of azeotropic mixture is formed by that deviation ?
  3. Q.182 marks
    (a) In a reaction, if the concentration of reactant 'X' is tripled, the rate of reaction becomes twenty-seven times. What is the order of the reaction ? (b) State a condition under which a bimolecular reaction is kinetically a first-order reaction. Give an example of such a reaction.
  4. Q.192 marks
    Complete the following ionic equations : (a) 2MnO4−+5SO32−+6H+⟶\mathrm{2MnO_4^{-} + 5SO_3^{2-} + 6H^{+} \longrightarrow} (b) Cr2O72−+14H++6Fe2+⟶\mathrm{Cr_2O_7^{2-} + 14H^{+} + 6Fe^{2+} \longrightarrow}
  5. Q.202 marks
    (a) Which halogen compound in the following pair will react faster in SN2\mathrm{S_N2} reactions and why ? CH3−CH2−I\mathrm{CH_3-CH_2-I} OR CH3−CH2−Br\mathrm{CH_3-CH_2-Br} (b) Why is chloroform stored in closed dark coloured bottles ?
  6. Q.212 marks
    Give reaction of glucose with the following : (a) HCN (b) Conc. HNO3\mathrm{HNO_3}

Section C

3 marks each

  1. Q.223 marks
    A solution is prepared by dissolving 5 g of a non-volatile solute in 200 g of water. It has a vapour pressure of 31⋅8431{\cdot}84 mm Hg at 300 K. Calculate the molar mass of the solute. (Vapour pressure of pure water at 300 K = 32 mm Hg)
  2. Q.233 marks
    The conductivity of 0⋅20{\cdot}2 M solution of KCl is 2⋅48×10−22{\cdot}48 \times 10^{-2} S cm−1\mathrm{cm^{-1}}. Calculate its molar conductivity and degree of dissociation (α)(\alpha). Given : λK+o=73⋅5\lambda^{o}_{\mathrm{K^{+}}} = 73{\cdot}5 S cm2 mol−1\mathrm{cm^{2}\,mol^{-1}} λCl−o=76⋅5\lambda^{o}_{\mathrm{Cl^{-}}} = 76{\cdot}5 S cm2 mol−1\mathrm{cm^{2}\,mol^{-1}}
  3. Q.243 marks
    A first-order reaction is 25% complete in 40 minutes. Calculate the value of rate constant. In what time will the reaction be 80% complete ? [Given : log 2 = 0⋅300{\cdot}30, log 3 = 0⋅480{\cdot}48, log 4 = 0⋅600{\cdot}60, log 5 = 0⋅690{\cdot}69]
  4. Q.253 marks
    (a) What type of nucleophilic substitution (SN1\mathrm{S_N1} or SN2\mathrm{S_N2}) occurs in the hydrolysis of 2-Bromobutane to form (±)(\pm)-Butan-2-ol ? Give reason. (b) What happens when chlorobenzene and methyl chloride are treated with sodium metal in dry ether ?
  5. Q.263 marks
    (a) Write the equations of the reactions involved in the following : (i) Reimer-Tiemann reaction (ii) Kolbe's reaction (b) Name the reagent used in the bromination of phenol to form 2,4,6-Tribromophenol.
  6. Q.273 marks
    How will you bring about the following conversions ? (any three) (a) Benzoic acid to Benzaldehyde (b) Ethanal to Propanone (c) Acetophenone to Benzoic acid (d) Bromobenzene to 1-Phenylethanol
  7. Q.283 marks
    Give the structures of A, B and C in the following reactions : (a) CH3CH2Cl→KCNA→LiAlH4B→0∘CHNO2C\mathrm{CH_3CH_2Cl} \xrightarrow{\mathrm{KCN}} \mathrm{A} \xrightarrow{\mathrm{LiAlH_4}} \mathrm{B} \xrightarrow[0^{\circ}\mathrm{C}]{\mathrm{HNO_2}} \mathrm{C} (b) Nitrobenzene →Fe/HClA→273 KNaNO2+HClB→C6H5OHC\xrightarrow{\mathrm{Fe/HCl}} \mathrm{A} \xrightarrow[273\ \mathrm{K}]{\mathrm{NaNO_2 + HCl}} \mathrm{B} \xrightarrow{\mathrm{C_6H_5OH}} \mathrm{C}

Section D

  1. The involvement of (n−1)d(n-1)d electrons in the behaviour of transition elements impart certain distinct characteristics to these elements. Thus, in addition to variable oxidation states, they exhibit paramagnetic behaviour, catalytic properties and tendency for the formation of coloured ions. The transition metals react with a number of non-metals like oxygen, nitrogen and halogens. KMnO4\mathrm{KMnO_4} and K2Cr2O7\mathrm{K_2Cr_2O_7} are common examples. The two series of inner transition elements, lanthanoids and actinoids, constitute the f-block of the periodic table. In the lanthanoids, there is regular decrease in atomic size with increase in atomic number due to the imperfect shielding effect of 4f-orbital electrons which causes contraction.
    Q.29 (a)1 mark
    Why do transition metals and their compounds act as good catalysts ?
  2. Q.29 (b)1 mark
    What is the cause of contraction in the atomic size of lanthanoids ?
  3. Q.29 (c)2 marks
    Define lanthanoid contraction. How does it affect the atomic radii of the third transition series and the second transition series ?
  4. OR

    Q.29 (c) OR2 marks
    In aqueous media, which is a stronger reducing agent — Cr2+\mathrm{Cr^{2+}} or Fe2+\mathrm{Fe^{2+}} and why ?
  5. Proteins are the most abundant biomolecules of the living system. Proteins are the polymers of about twenty different α\alpha-amino acids which are linked by peptide bonds. Ten amino acids are called essential amino acids. In zwitter ionic form, amino acids show amphoteric behaviour as they react both with acids and bases. On the basis of their molecular shape, proteins are classified into two types : Fibrous and Globular proteins. Structure and shape of proteins can be studied at four different levels i.e., primary, secondary, tertiary and quaternary, each level being more complex than the previous one. The secondary or tertiary structure of proteins get disturbed on change of pH or temperature and they are not able to perform their functions. This is called denaturation of proteins.
    Q.30 (a)1 mark
    What are essential amino acids ?
  6. Q.30 (b)1 mark
    What is meant by zwitter ionic form of amino acids ?
  7. Q.30 (c)2 marks
    (i) Give one example each for Fibrous protein and Globular protein. (ii) What type of linkages hold monomers of proteins together ?
  8. OR

    Q.30 (c) OR2 marks
    (i) What is the structural feature which characterises a reducing sugar ? (ii) What is the structural difference between nucleoside and nucleotide ?

Section E

5 marks each

  1. Q.31 (a)5 marks
    (i) Calculate emf of the following cell at 25∘C25^{\circ}\mathrm{C} : Zn (s) ∣ Zn2+ (0⋅001M) ∣∣ Cd2+ (0⋅1 M) ∣ Cd (s)\mathrm{Zn\,(s)}\,|\,\mathrm{Zn^{2+}}\,(0{\cdot}001\mathrm{M})\,||\,\mathrm{Cd^{2+}}\,(0{\cdot}1\ \mathrm{M})\,|\,\mathrm{Cd\,(s)} Given : EZn2+/Zno=− 0⋅76\mathrm{E^{o}_{Zn^{2+}/Zn}} = -\,0{\cdot}76 V, ECd2+/Cdo=− 0⋅40\mathrm{E^{o}_{Cd^{2+}/Cd}} = -\,0{\cdot}40 V [log 10 = 1] (ii) State Faraday's second law of electrolysis. How will the pH of aqueous NaCl solution be affected when it is electrolysed ?
  2. OR

    Q.31 (b)5 marks
    (i) Calculate the ΔrGo\Delta_{\mathrm{r}}\mathrm{G^{o}} and log⁡Kc\log \mathrm{K_c} for the following cell reaction : Fe (s)+Ag+ (aq)⇌Fe2+(aq)+Ag (s)\mathrm{Fe\,(s)} + \mathrm{Ag^{+}\,(aq)} \rightleftharpoons \mathrm{Fe^{2+}(aq)} + \mathrm{Ag\,(s)} Given : EFe2+/Feo=− 0⋅44\mathrm{E^{o}_{Fe^{2+}/Fe}} = -\,0{\cdot}44 V, EAg+/Ago=+ 0⋅80\mathrm{E^{o}_{Ag^{+}/Ag}} = +\,0{\cdot}80 V, 1 F = 96500 C mol−1\mathrm{mol^{-1}} (ii) Write any two advantages of the fuel cells over primary and secondary batteries ? (iii) How many Faradays are required for the oxidation of 1 mole of H2O\mathrm{H_2O} to O2\mathrm{O_2} ?
  3. Q.32 (a)5 marks
    (i) Write the major product(s) in the following reactions : (1) Ethylbenzene →b) H+a) KMnO4 , KOH\xrightarrow[\mathrm{b)\ H^{+}}]{\mathrm{a)\ KMnO_4\,,\ KOH}} ? (2) Benzaldehyde + CH3−CO−CH3→dil NaOH+\ \mathrm{CH_3-CO-CH_3} \xrightarrow{\text{dil NaOH}} ? (3) Benzoic acid →Br2/FeBr3\xrightarrow{\mathrm{Br_2/FeBr_3}} ? (ii) Give simple chemical tests to distinguish between the following pairs of compounds : (1) Acetophenone and Propiophenone (2) Pentanal and Pentan-3-one
  4. OR

    Q.32 (b)5 marks
    (i) Give reasons for the following : (1) In semicarbazide, only one −NH2-\mathrm{NH_2} group is involved in the formation of semicarbazone. (2) Acetaldehyde is more reactive than acetone towards addition of HCN. (ii) (1) Arrange the following in decreasing order of their acidic strength : CH3COOH\mathrm{CH_3COOH}, O2N−CH2−COOH\mathrm{O_2N-CH_2-COOH}, HCOOH\mathrm{HCOOH} (2) Name the reagent in the following reaction : CH3−CH=CH−CH2−CN→?CH3−CH=CH−CH2−CHO\mathrm{CH_3-CH=CH-CH_2-CN} \xrightarrow{?} \mathrm{CH_3-CH=CH-CH_2-CHO} (iii) Write the reaction involved in Hell-Volhard-Zelinsky reaction.
  5. Q.335 marks
    Attempt any five of the following : (a) Write the IUPAC name of the complex : [Co(H2O)(CN)(en)2]2+[\mathrm{Co(H_2O)(CN)(en)_2}]^{2+} (b) Why is geometrical isomerism not possible in tetrahedral complexes having two different types of unidentate ligands coordinated with the central metal ion ? (c) Arrange the following complex ions in increasing order of their crystal field splitting energy (Δo)(\Delta_{\mathrm{o}}) : [Co(NH3)6]3+[\mathrm{Co(NH_3)_6}]^{3+}, [CoF6]3−[\mathrm{CoF_6}]^{3-}, [Co(CN)6]3−[\mathrm{Co(CN)_6}]^{3-} (d) Write the hybridization and magnetic character of the complex [Ni(CO)4][\mathrm{Ni(CO)_4}] on the basis of valence bond theory. [Atomic No. : Ni = 28] (e) Out of [CoF6]3−[\mathrm{CoF_6}]^{3-} and [Co(C2O4)3]3−[\mathrm{Co(C_2O_4)_3}]^{3-}, which one complex is : (i) more stable ? (ii) the high spin complex ? (f) What is the difference between an ambidentate ligand and bidentate ligand ? (g) Write the electronic configuration of d5\mathrm{d^5} in terms of t2g\mathrm{t_{2g}} and eg\mathrm{e_g} in an octahedral field when : (i) Δo>P\Delta_{\mathrm{o}} > \mathrm{P}, and (ii) Δo<P\Delta_{\mathrm{o}} < \mathrm{P}