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Maharashtra HSC Class 12 Chemistry July 2024 question paper

Maximum marks 70 · Time 3 hours

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. Select and write the correct answer for the following multiple choice type of questions :
    Q.1 (i)1 mark
    Integrated rate law equation for a zero order reaction is −-

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  2. Q.1 (ii)1 mark
    The spin only magnetic moment of Fe2+\mathrm{Fe^{2+}} ion is ____.

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  3. Q.1 (iii)1 mark
    The relation between radius of sphere and edge length in simple cubic lattice is ____.

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  4. Q.1 (iv)1 mark
    The monomer used in the preparation of thermocol is ____.

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  5. Q.1 (v)1 mark
    The pH of 0.01 M solution of HCl is −-

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  6. Q.1 (vi)1 mark
    Which of the following α\alpha-amino acids do not contain chiral centre?

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  7. Q.1 (vii)1 mark
    Among the following benzylic halide is ____. (The four options are drawn structures — see the figure.)

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  8. Q.1 (viii)1 mark
    Neutral complex in the following is _____

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  9. Q.1 (ix)1 mark
    The reaction used to convert toluene to benzaldehyde is known as :

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  10. Q.1 (x)1 mark
    A better reagent to convert primary alcohol to aldehyde is ____.

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  11. Answer the following questions :
    Q.2 (i)1 mark
    Write the name of insecticide which is effectively used instead of DDT.
  12. Q.2 (ii)1 mark
    Write the name of hydrocarbon formed when methyl magnesium iodide is treated with ammonia.
  13. Q.2 (iii)1 mark
    Calculate the standard potential of the following cell at 25°C : Zn(s)∣Zn2+(0.08 M)∥Cr3+(0.1 M)∣Cr(s)\mathrm{Zn_{(s)} \mid Zn^{2+}(0.08\,M) \parallel Cr^{3+}(0.1\,M) \mid Cr_{(s)}} EZn∘=−0.76 VE^{\circ}_{\mathrm{Zn}} = -0.76\ \mathrm{V}, ECr∘=−0.74 VE^{\circ}_{\mathrm{Cr}} = -0.74\ \mathrm{V}
  14. Q.2 (iv)1 mark
    Write the IUPAC name of Na3[AlF6]\mathrm{Na_3[AlF_6]}.
  15. Q.2 (v)1 mark
    Write the electronic configuration of Zn2+\mathrm{Zn^{2+}} ion. (Atomic number of zinc is 30).
  16. Q.2 (vi)1 mark
    Write the IUPAC name of amine formed when acetamide undergoes Hofmann bromamide degradation.
  17. Q.2 (vii)1 mark
    Write the condition for spontaneity of reaction with respect to entropy.
  18. Q.2 (viii)1 mark
    Write the relation between van't Hoff factor and degree of dissociation of an electrolyte.

Section B

2 marks each · attempt any 8

  1. Q.32 marks
    The normal boiling point of ethyl acetate is 77.06 °C. A solution of 50 g of non-volatile solute in 150 g ethyl acetate boils at 82.60 °C. Calculate molar mass of solute. [Kb=2.77 ∘C kg mol−1][K_b = 2.77\ \mathrm{{}^{\circ}C\ kg\ mol^{-1}}]
  2. Q.42 marks
    Deduce first law of thermodynamics for : (a) isothermal process (b) isochoric process
  3. Q.52 marks
    Complete the following equations : (i) XeF2+H2O⟶ ?\mathrm{XeF_2 + H_2O \longrightarrow\ ?} (ii) Xe+F2→Low temperatureElectric discharge ?\mathrm{Xe + F_2 \xrightarrow[\text{Low temperature}]{\text{Electric discharge}}\ ?}
  4. Q.62 marks
    Differentiate between ionic crystals and covalent crystals.
  5. Q.72 marks
    What is the mass of Cu metal produced at the cathode during the passage of 5 ampere of current through CuSO4\mathrm{CuSO_4} solution for 100 minutes? [Molar mass of Cu = 63.5 g mol−163.5\ \mathrm{g\ mol^{-1}}]
  6. Q.82 marks
    Define Buffer solution. Write the Henderson Hasselbalch equation for acidic buffer.
  7. Q.92 marks
    Write two principles of green chemistry.
  8. Q.102 marks
    Write the preparation of Nylon-6 polymer and its two uses.
  9. Q.112 marks
    Define : (a) Pyrometallurgy. (b) Roasting.
  10. Q.122 marks
    Write salient features of SN1S_N1 mechanism.
  11. Q.132 marks
    What is the denaturation of proteins? Write the name of only pyrimidine base in RNA.
  12. Q.142 marks
    Write the reaction when ethylamine is treated with : (a) excess of ethyl bromide (b) Hinsberg's reagent

Section C

3 marks each · attempt any 8

  1. Q.153 marks
    Construct a cell using standard hydrogen electrode and zinc electrode. Write its cell reaction and cell representation. Calculate cell potential of a cell with 0.01 M Zn2+0.01\ \mathrm{M}\ \mathrm{Zn^{2+}} ions. Standard potential of a cell is +0.76+0.76 V.
  2. Q.163 marks
    State Henry's Law. Write four conditions for ideal solutions.
  3. Q.173 marks
    Write one example of each of ionisation, linkage and hydrated isomerism.
  4. Q.183 marks
    Calculate the standard enthalpy of the reaction : SiO2(s)+3C(graphite)→SiC(s)+2CO(g)\mathrm{SiO_{2(s)} + 3C_{(graphite)} \rightarrow SiC_{(s)} + 2CO_{(g)}} from the following reactions : (i) Si(s)+O2(g)→SiO2(s)\mathrm{Si_{(s)} + O_{2(g)} \rightarrow SiO_{2(s)}}, ΔrH∘=−911 kJ\Delta_r H^{\circ} = -911\ \mathrm{kJ} (ii) 2C(graphite)+O2(g)→2CO(g)\mathrm{2C_{(graphite)} + O_{2(g)} \rightarrow 2CO_{(g)}}, ΔrH∘=−221 kJ\Delta_r H^{\circ} = -221\ \mathrm{kJ} (iii) Si(s)+C(graphite)→SiC(s)\mathrm{Si_{(s)} + C_{(graphite)} \rightarrow SiC_{(s)}}, ΔrH∘=−65.3 kJ\Delta_r H^{\circ} = -65.3\ \mathrm{kJ}
  5. Q.193 marks
    Derive Ostwald's dilution law for weak acid. Obtain relation between solubility product and its solubility for Al(OH)3\mathrm{Al(OH)_3}.
  6. Q.203 marks
    60% of the reactant decomposes in 45 minutes in a first order reaction. Calculate the half life period of the reaction. Write the relation between half life period and initial concentration for zero order reaction.
  7. Q.213 marks
    Write the conditions of colour of transition metal ion. Write the alloy used in Fischer Tropsch process.
  8. Q.223 marks
    Explain anomalous behaviour of oxygen with respect to atomicity, magnetic property and oxidation state.
  9. Q.23 (i)3 marks
    Explain cross Cannizzaro reaction.
  10. Q.23 (ii)
    Draw structure of Zwitter ion of sulfanilic acid.
  11. Q.243 marks
    Identify A, B, C and rewrite the chemical reactions : H3C−CH2Cl+KOH(aq)→Δ′A′→hot Cu powder′B′\mathrm{H_3C{-}CH_2Cl + KOH_{(aq)} \xrightarrow{\Delta} 'A' \xrightarrow{\text{hot Cu powder}} 'B'}, and ′B′→K2Cr2O7/dil. H2SO4′C′\mathrm{'B' \xrightarrow{K_2Cr_2O_7 / dil.\ H_2SO_4} 'C'}
  12. Q.253 marks
    Explain optical isomerism in 2-chlorobutane.
  13. Q.263 marks
    Write Clemmenson's reduction reaction of propanone. Write Fehling solution test for ethanal.

Section D

4 marks each · attempt any 3

  1. Q.27 (i)4 marks
    How is dioxygen prepared in laboratory from KClO3\mathrm{KClO_3}?
  2. Q.27 (ii)
    Write the chemical reaction to convert : (a) phenol to benzoquinone (b) phenol to cyclohexanol
  3. Q.28 (i)4 marks
    Define : (a) Standard enthalpy of combustion. (b) Enthalpy of atomization.
  4. Q.28 (ii)
    Draw the structure of D-ribose sugar.
  5. Q.28 (iii)
    Write the uses of bronze alloy.
  6. Q.29 (i)4 marks
    Distinguish between order and molecularity of a reaction.
  7. Q.29 (ii)
    Write gases liberated at cathode and anode during electrolysis of aqueous NaCl solution.
  8. Q.29 (iii)
    Write two uses of neon.
  9. Q.30 (i)4 marks
    When gold crystallizes, it forms face-centred cubic cell. The unit cell edge length is 408 pm. Calculate the density of gold. [Molar mass of gold = 197 g mole−1197\ \mathrm{g\ mole^{-1}}]
  10. Q.30 (ii)
    Which flower is an example of self cleaning?
  11. Q.314 marks
    Explain the formation of [Co(NH3)6]3+\mathrm{[Co(NH_3)_6]^{3+}} ion on the basis of Valence bond theory. Convert the following : (a) acetic acid to ethyl acetate (b) acetic acid to ethyl alcohol.