Board Paper of Class 12-Science 2012 Chemistry (SET 3) - Solutions
(i) All questions are compulsory
(ii) Question numbers 1 to 8 are very short-answer questions and carry 1 mark each.
(iii) Question numbers 9 to 18 are short-answer questions and carry 2 marks each.
(iv) Question numbers 19 to 27 are also short-answer questions and carry 3 marks.
(v) Question numbers 28 to 30 are long-answer questions and carry 5 marks each.
(vi) Use Log Tables, if necessary. Use of calculators is not allowed.
- Question 1
What are n-types semiconductors?
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- Question 2
- Question 3
- Question 4
- Question 5
Write the IUPAC name of the following.
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- Question 6
Write the IUPAC name of the following.
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- Question 7
Write a reaction which shows that all the carbon atoms in glucose are linked in a straight chain.
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- Question 8
What is the cause of a feeling of depression in human beings? Name a drug which can be useful in treating this depression.
- Question 9
A reaction is of second order with respect to a reactant. How is its rate affected if the concentration of the reactant is (i) doubled (ii) reduced to half?
- Question 10
Express the relation among cell constant, resistance of the solution in the cell and conductivity of the solution. How is molar conductivity of a solution related to its conductivity?
OR
The molar conductivity of a 1.5 M solution of an electrolyte is found to be 138.9S cm2 mol−1.
Calculate the conductivity of the conductivity of this solution.
- Question 11
Explain the role of each of the following:
(i) NaCN in the extraction of silver
(ii) SiO2 in the extraction of copper
- Question 12
- Question 13
Explain the following facts giving appropriate reason in each case:
(i) NF3 is an exothermic compound whereas NCl3 is not.
(ii) All the bonds in SF4 are not equivalen.
- Question 14
Explain the following behaviours:
(i) Alcohols are more soluble in water than the hydrocarbons of comparable molecular masses.
(ii) Ortho-nitrophenol is more acidic than ortho-methoxyphenol.
- Question 15
Explain the mechanism of acid catalysed hydration of an alkene to form corresponding alcohol.
- Question 16
Complete the following chemical reaction equations:
(i) C6H5N2Cl + H3PO2 + H2O →
(ii) C6H5NH2 + Br2(aq.) →
- Question 17
Describe the following giving the relevant chemical equation in each case:
(i) Carbylamine reaction
(ii) Hofmann’s bromamide reaction.
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- Question 18
- Question 19
Copper crystallises with face centred cubic unit cell. If the radius of copper atom is 127.8 pm, calculate the density of copper metal.
(Atomic mass of Cu = 63.55 u and Avogadro’s number NA = 6.02 × 1023 mol−1)
OR
Iron has a body centred cubic unit cell with the cell dimension of 286.65 pm. Density of iron is 7.87 g cm−3. Use this information to calculate Avogadro’s number. (Atomic mass of Fe = 56.0 u)
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- Question 20
The reaction N2(g) + O2(g) 2NO(g), contributes to air pollution whenever a fuel is burnt in air at a high temperature. At 1500 K, equilibrium constant K for it is 1.0 × 10−5. Suppose in a case [N2] = 0.80 mol L−1 and [O2] = 0.20 mol L−1 before any reaction occurs. Calculate the equilibrium concentrations of the reactants and the product after the mixture has been heated to 1500 K.
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- Question 21
The electrical resistance of a column of 0.05 M NaOH solution of diameter 1cm and length 50
cm is 5.55 × 103 ohm. Calculate its resistivity, conductivity and molar conductivity.
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- Question 22
Write three distinct features of chemisorptions which are not found in physisorptions.
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- Question 23
Explain each of the following observations:
(i) With the same d-orbital configuration (d4), Cr2+ is a reducing agent while Mn3+ is an oxidising agent.
(ii) Actinoids exhibit a much larger number of oxidation states than the lanthanoids.
(iii) There is hardly any increase in atomic size with increasing atomic number in a series of transition metals.
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- Question 24
Name of the following coordination entities and describe their structure:
(i) [Fe(CN)6]4−
(ii) [Cr(NH3)4Cl2]+
(iii) [Ni(CN)4]2−
(Atomic numbers Fe = 26. Cr = 24, Ni = 28)
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- Question 25
Answer the following question:
(i) What is meant by chirality of a compound? Give an example.
(ii) Which one of the following compounds is more easily hydrolyzed by KOH and why?
CH3CHCICH2CH3 or CH3CH2CH2Cl
(iii) Which one undergoes S N 2 substitution reaction faster and why?
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- Question 26
Define the following as related to proteins:
(i) Peptide linkage
(ii) Primary structure
(iii) Denaturation
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- Question 27
Differentiate between thermoplastic and thermosetting polymers. Give one example of each.
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- Question 28
(a) Draw the molecular structure of the following compounds.
(i) N2O5
(ii) XeOF4
(b) Explain the following observation:
(i) Sulphur has a greater tendency for catenation than oxygen.
(ii) ICI is more reactive than I2.
(iii) Despite lower value of its electron gain enthalpy with negative sign, fluorine (F2) is a stronger oxidizing agent than Cl2.
OR
(a) Complete the following chemical equation
(i) Cu + HNO3 (dilute) →
(ii) XeF4 + O2F2 →
(b) Explain the following observation:
(i) Phosphorus has greater tendency for catenation than nitrogen.
(ii) Oxygen is a gas but sulphur a solid.
(iii) The halogens are coloured. Why?
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- Question 29
(a) Write a suitable chemical equation to complete each of the following transformations:
(i) Butan-1-ol to butanoic acid
(ii) 4-methylacetophenone to benzene-1, 4-dicarboxylic acid
(b) An organic compound with molecular formula C9H10O forms 2,4-DNP derivative, reduces Tollen’s reagent and undergoes Cannizzaro’s reaction. On vigorous oxidation it gives 1, 2-benzenedicarboxylic acid. Identify the compound.
OR
(a) Give chemical tests to distinguish between
(i) Propanol and propanone
(ii) Benzaldehyde and acetophenone
(b) Arrange the following compounds in an increasing order of their property as indicated:
(i) Acetaldeyde, Acetone, Methyl tert-butyl ketone (reactivity towards HCN)
(ii) Benzoic acid, 3,4-Dinitrobenzoic acid, 4-Methoxybenzoic acid (acid strength).
(iii) CH3CH2CH(Br) COOH, CH3CH (Br) CH2COOH, (CH3)2CHCOOH (acid strength)
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- Question 30
(a) Define the following terms:
(i) Mole fraction
(ii) Ideal solution
(b) 15.0 g of an unknown molecular material is dissolved in 450 g of water. The resulting solution freezes at − 0.34°C. What is the molar mass of the material? (Kf for water = 1.86 K kg mol− 1)
OR
(a) Explain the following:
(i) Henry’s law about dissolution of a gas in a liquid.
(ii) Boiling point elevation constant for a solvent.
(b) A solution of glycerol (C3H8O3) in water was prepared by dissolving some glycerol in 500 g of water. This solution has a boiling point of 100.42° C. What mass if glycerol was dissolved to make this solution? (Kb for water = 0.512 K kg mol−1)
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