SAMPLE PAPER-2 Chemistry

Section A

21. Select and write the correct answers to the following questions:

(i) Molecular solids are

(a) Crystalline solids

(b) Amorphous solids

(c) Ionic solids

(d) Metallic solids

(ii) On which electrode the oxidation reaction takes place?
(a) Anode
(b) Cathode
(c) Salt bridge
(d) None of them

(iii) Isobutylamine is an example of



(b) amine

(c) amine

(d) Quaternary ammonium salt

(iv) Two solutions have the ratio of their concentrations 0.4 and ratio of their conductivities 0.216 . The ratio of their molar conductivities will be
(a) 0.54
(b) 11.574
(c) 0.0864
(d) 1.852

(v) Identify the chiral molecule from the following.

(a) 1-bromobutane

(b) 1,1-dibromobutane

(c) 2,3-dibromobutane

(d) 1,3-bromobutane

(vi) A living cell contains a solution which is isotonic with sugar solution. What osmotic pressure develops when the cell is placed in solution at body temperature?

(vii) Formula for the compound sodium hexacynoferrate (iii) is

(viii) Components of Nichrome alloy are
(b) Ni, Cr, Fe, C

(ix) Which of the following has highest electron gain enthalpy?
(a) Fluorine
(b) Chlorine
(c) Bromine
(d) lodine

(x) Which of the Na following is a buffer solution?

(a) in water

(b) in water

(c) in water

(d) in water

  1. Answer the following questions:

(i) What is standard cell potential for the reaction?

(ii) Write IUPAC name of

(iii) Name some chain growth polymers.

(iv) Which amide does produce ethanamine by Hofmann bromamide degradation reaction?

(v) Give two uses of .

(vi) What is meant by ‘shielding of electrons’ in an atom?

(vii) Name a compound where Frenkel defect is found.

(viii) Write the formula for tetra ammine platinum (ii) chloride.

22. Section B

23. Attempt any Eight of the following questions:

  1. Give the structures of Thiosulphuric acid and Peroxy monosulphuric acid.
  2. Explain the role of green chemistry.
  3. How many moles of electrons are passed when 0.8 Ampere current is passed for 1 hour through molten ?
  4. Write formulae of the following complexes.

(i) Potassium ammine trichloroplatinate (ii)

(ii) Dicyanoaurate (i) ion

  1. Explain the basic nature of amines with suitable example.
  2. Discuss the structure of sulphure dioxide.
  3. What is the enthalpy of atomisation? Give an example.
  4. What is lanthanoid contraction?
  5. Why formic acid is stronger than acetic acid?
  6. Give the following named reactions.

(i) Wurtz-Fittig reaction

(ii) Fittig reaction

  1. Why p-nitrophenol is a stronger acid than phenol?
  2. How vapour pressure lowering is related to a rise in boiling point of solution?

24. Section C

25. Attempt any Eight of the following questions:

  1. What is the action of hydrazine on cyclopentanone in presence of in ethylene glycol? How ketones are prepared from nitriles?
  2. Aluminium crystallises in cubic close packed structure with unit cell edge length of . What is the radius of Al atom? How many unit cells are there in of Al?
  3. Distinguish between and mechanism of substitution reaction.
  4. The vapour pressure of water at is . What is the vapour pressure of solution containing urea in of water?
  5. Write reaction showing conversion of acetaldehyde into acetaldehyde dimethyl acetal.
  6. Give valence bond description for the bonding in the complex : Draw box diagrams for free metal ion. Which hybrid orbitals are used by the metal? State the number of unpaired electrons.
  7. Obtain the relationship between the rate constant and half-life of a first order reaction.

State Hess’s law of constant heat summation. Illustrate with an example. State its applications.

  1. Write structure of natural rubber and neoprene rubber along with the name and structure of their monomers.
  2. What are pseudo-first order reactions? Give one example and explain why it is pseudo-first order.
  3. Why it is impossible to measure the potential of a single electrode?
  4. (i) Calculate the standard enthalpy of:

(ii) The enthalpy change of the following reaction:


Calculate bond enthalpy. The bond enthalpies are:


26. Section D

27. Attempt any Three of the following questions:

  1. (i) In solution is . Calculate the of solution.

(ii) The solubility product of is . Calculate its solubility in and (Molar mass of )

  1. Draw a neat diagram for the Haworth formula of glucopyranose. Give the industrial applications of enzyme catalysis.
  2. Distinguish between rhombic sulphur and monoclinic sulphur.
  3. Write structural formulae for:

(i) Pentane-1,4-diol

(ii) Cyclohex-2-en-1-ol.

(iii) -Nitrophenol

(iv) Salicylic acid

  1. Explain the trends in atomic radii of -block elements.

28. [A]] Answer Key

29. Section A

  1. (i) (a) Crystalline solids

(ii) (a) Anode

(iii) (c) Amine

(iv) (a) 0.54

(v) (c) 2,3-Dibromobutane

(vi) (b)

(vii) (d)

(viii) (c)

(ix) (b) Chlorine

(x) (c) in water

  1. (i) The standard cell potential for the reaction is .

(ii) 2-Bromo-3-methylpent-3-ene

(iii) Chain growth polymers are polyacrylonitrile, polyvinylchloride, polythene, etc. (iv) Propanamide produces ethanamine by Hofmann bromamide degradation reaction

(v) Uses of chlorine dioxide are as follows:

(a) Bleaching agent for paper pulp and textiles.

(b) In water treatment.

(vi) (a) The decrease in the force of attraction exerted by the nucleus on the valence electrons due to the presence of electrons in the inner shells is called the shielding effect.

(b) As a result of the shielding effect, the effective nuclear charge experienced by the valence electron is less than the actual nuclear charge.



30. Section B

  1. (i) Thiosulphuric acid, .

(ii) Peroxy monosulphuric acid,

  1. (i) To promote innovative chemical technologies that reduce or eliminate the use or generation of hazardous substances in the design, manufacture, and use of chemical products.

(ii) The green chemistry helps to reduce capital expenditure to prevent pollution.

(iii) Green chemistry incorporates pollution, prevention practices in the manufacture of chemicals and promotes pollution prevention and industrial ecology.

(iv) Green chemistry is a new way of looking at chemicals and their manufacturing process to minimise any negative environmental effects.

Calculate: Using formula (i).

Quantity of electricity passed

Using formula (ii),

Number of moles of electrons passed

Number of moles of electrons passed through molten is 0.03 mol .

  1. (i)


  1. Nitrogen atom of amines contains a lone pair of electrons which can be donated. Thus, amines act as bases and nucleophiles.


(i) The reaction of ethylamine with dilute hydrochloric acid results in the formation of ethyl ammonium chloride.

  1. Sulphur dioxide is angular with bond angle of

The S-O double bond arises from bonding. It is a resonance hybrid of two canonical forms.

  1. The enthalpy change accompanying the dissociation of all molecules in one mole of gas phase substance into gaseous atoms is called enthalpy of atomisation.

For example: Atomisation of methane molecule.

  1. As we move from to , the atomic and ionic radii of trivalent lanthanoid show steady decrease because with increase in atomic number, the nuclear charge increases and electrons are added to shell which show poor shilding effect. As a result there is gradual increase in nuclear charge and decrease in radii. This is known as lanthanoid contraction.
  2. (i) The negatively charged acetate ion (i.e., the conjugate base of acetic acid) gets destabilised by + I effect of group.

(ii) Lesser is the stabilisation of the conjugate base, weaker is the acid.

(iii) In formate ion, there is no such destabilisation effect.

Thus, formic acid is stronger than acetic acid.

31. 2. (i) Wurtz-Fitting Reaction:

(ii) Fitting reaction:

  1. The conjugate base of -nitrophenol is better resonance stabilised due to six resonance structures compared to the five resonance structures of the conjugate base of phenol. The resonance structure has a negative charge on only electgronegative oxygen atoms. Hence, -nitrophenol is a stronger acid than phenol.
  2. (i) At the boiling point of a liquid, its vapour pressure is equal to .

(ii) In order to reach boiling point the solution and solvent must be heated to a temperature at which their respective vapour pressures attain .

(iii) At any given temperature the vapour pressure of a solution is lower than that of pure solvent. Hence, the vapour pressure of solution needs a higher temperature to reach than that needed for vapour pressure of solvent. Therefore, vapour pressure lowering causes a rise in the boiling point of a solution.

Section C

  1. Ketones are prepared by reacting nitriles with Grignard reagent in dry ether as solvent followed by acid hydrolysis.


  1. (i) Using formula (i),

(ii) Using formula (ii),

Number of unit cells in volume of metal

Number of unit cells in of

(a) Radius of Al atom ( ) is 125 pm.

(b) Number of unit cells in of is .


Kinetics2nd order1st order
Number of stepsOne stepTwo step

Bond makingand bondbreaking
First the bond in thereactant breaks andthen a new bond inproduct is formed
Transition state
One step, onetransition state

Two steps, twotransition state

Directionof attack ofnucleophile

Only back sideattack

Back side attack andfront side attak

Weak Nucleophilefavourable.
  1. Molar mass of urea

Molar mass of water

Now, using formula,

  1. Step 1:

33. Step 2:

  1. (i) The oxidation state of vanadium is +3 .

(ii) Valence shell electronic configuration of free metal ion,

(iii) The number of ligands is 4. Therefore, the number of vacant metal ion orbitals required for bonding with ligands must be four.

(iv) Four orbitals on metal available for hybridisation are one and three . The complex is tetrahedral.

(v) The four metal ion orbitals for bonding with ligands are derived from the hybridization.

(vi) Four vacant hybrid orbitals of overlap with four orbitals of ions.

(vii) Configuration after complex formation would be

(viii) The complex has two unpaired electrons. The structure of

  1. The integrated rate law for the first order reaction is given by the equation

Where initial concentration of the reactant at The concentration falls to , at time from the start of the reaction. The concentration of the reactant falls to at time .


So, the equation can be written as

34. Hess’s law of constant heat summation:

Hess’s law of constant heat summation states that, “Overall the enthalpy change for a reaction is equal to sum of enthalpy changes of individual steps in the reaction”

35. For example:

The enthalpy changes for a chemical reaction is the same regardless of the path by which the reaction occurs. Hess’s law is a direct consequence of the fact that enthalpy is state function. The enthalpy change of a reaction depends only on the initial and final states and not on the path by which the reaction occurs.

To determine the overall equation of reaction, reactants and products in the individual steps are added or subtracted like algebraic entities.

Consider the synthesis of .




The sum of the enthalpy changes for steps (1) and (2) is

Natural RubberNeoprene


equal to enthalpy change for the overall reaction.

36. Application of Hess’s Law:

The Hess’s law has been useful to calculate the enthalpy the enthalpy changes for the reactions with their enthalpies being not known experimentally.

  1. A reaction which has higher order true rate law but experimentally found to behave as first order are called pseudo first order reaction. For example: Hydrolysis of sucrose.

is an example of pesudo first order reaction, because water takes part in the reaction the true rate law rate indicates that the reaction must be second order. Similarly to the hydrolysis of ester, . It is constant and the rate law became rate Thus, the second order true law is converted, to first order rate law.

  1. (i) Every oxidation reaction needs to be accompanied by a reduction reaction.

(ii) The occurrence of only oxidation or only reduction is not possible.

(iii) In galvanic cell oxidation and reduction occur simultaneously.

(iv) The potential associated with the redox can be experimentally measured. For the measurement of potential two electrodes need to be combined together where the redox reaction occurs.

Hence, it is impossible to measure the potential of a single electrode.

  1. (i)

37. Section D

  1. (i)


38. Calculation:

From formula (i).

From formula (ii).

(ii) The solubility product of is:

The solubility in molar solubility in molar mass


( – D- (+) – Glucopyranose) ( -D- (+) – Glucopyranose) Some examples of industrial application of enzyme catalysis are:

(i) Conversion of glucose to sweet-tasting fructose, using glucose isomerase.

(ii) Manufacture of new antibiotics, using pencillin G acylase.

(iii) Manufacture of laundry detergents, using proteases.

(iv) Manufacture of esters used in cosmetics, using genetically engineered enzyme.




It is a pale yellow colouredsoild.
It is bright yellow soild
It forms orthorhombic crystals
It forms needle-shapedmonoclinic crystals
Its melting point is Its melting point is
Its density is Its density is

It is insoluble in water andsoluble in
Soluble in

It is stable below andtransforms to -sulphur abovethis temperature

It is stable above andtransforms into -sulphurbelow this temperature.

It is prepared by theevaporation of rolls sulphurin .

It is prepared from rhombicsulphur.
  1. (i)

Pentane-1, 4-diol





  1. (i) Atomic radii of the elements of the transition series decrease gradually from left to right.

(ii) As we move across a transition series from left to right, the nuclear charge increases by one unit at a time.

(iii) The last filled electron enters a penultimate subshell. However, orbitals in an atom are less penetrating or more diffused and, therefore electrons offer smaller screening effects.

(iv) The result is that effective nuclear charge also increases as the atomic number increases along with a transition series. Hence the atomic radii gradually decrease across a transition series from left to right.

Trends in atomic radii of -block elements