This document contains sample questions from an IIT-JEE Advanced chemistry exam. It includes 12 questions on topics like oxidation-reduction reactions, isomerism, hydrogen bonding, electrochemistry, transition metals, and solutions. The total number of reagents that can oxidize iodide to iodine is 7. The molality of a 3.2 molar solution of a compound with molar mass 80 g/mol dissolved in a solvent with density 0.4 g/mL is 8.

1. JEE MANTRA
IITJEE –ADVANCED 2014 PAPER 1 CHEMISTRY

2. INORGANIC
• 1.QUESTION. Consider the following list of reagents:
• Acidified K2Cr2O7, alkaline KMnO4, CuSO4, H2O2, CI2, O3, FeCI3, HNO3 and
Na2S2O3.
• The total number of reagents that can oxidise aqueous iodide to iodine is
• ANS. [7]
• H+
• / K2Cr2O7 , OH / KMnO4 , CuSO4 , H2O2 , Cl2 , O3, HNO3

3. ISOMERISM
• 2. The correct combination of names for isomeric alcohols with molecular formula C4H10O
• is/are
• (A) tert−butanol and 2−methylpropan−2−ol
• (B) tert−butanol and 1, 1−dimethylethan−1−ol
• (C) n−butanol and butan−1−ol
• (D) isobutyl alcohol and 2−methylpropan−1−ol
• 2. (A), (C), (D)
• Factual.

4. H-BONDING
• 3. Hydrogen bonding plays a central role in the following phenomena :
• (A) Ice floats in water.
• (B) Higher Lewis basicity of primary amines than tertiary amines in aqueous
solutions.
• (C) Formic acid is more acidic than acetic acid.
• (D) Dimerisation of acetic acid in benzene.
• 3. (A), (B), (D)
• Formic acid is more acidic than acetic acid due to electronic effect.

5. ELECTROCHEMISTRY
• 4. In a galvanic cell, the salt bridge
• (A) does not participate chemically in the cell reaction.
• (B) stops the diffusion of ions from one electrode to another.
• (C) is necessary for the occurrence of the cell reaction.
• (D) ensures mixing of the two electrolytic solutions.
• 4. (A), (B), (C)
• Properties of salt bridge.

6. INORGANIC CHEMISTRY –TRANSITION
ELEMENT
• 5 Upon heating with Cu2S, the reagent(s) that give copper metal is/are
• (A) CuFeS2 (B) CuO (C) Cu2O (D) CuSO4
• 5. (C)
• Cu2S + 2Cu2O ⎯⎯→ 6Cu + SO2

7. INORGANIC
• 6The correct statement(s) for orthoboric acid is/are
• (A) It behaves as a weak acid in water due to self ionization
• (B) Acidity of its aqueous solution increases upon addition of ethylene
glycol.
• (C) It has a three dimensional structure due to hydrogen bonding.
• (D) It is a weak electrolyte in water.
• 6. (B), (D)
• Properties of orthoboric acid.

8. OXIDATION -REDUCTION
• 29. For the reaction :
I−+ CIO3+H2SO4 → CI−+ HSO4 + I2
• The correct statement(s) in the balanced equation is/are:
• (A) Stoichiometric coefficient of HSO4
is 6.
• (B) lodide is oxidized.
• (C) Sulphur is reduced.
• (D) H2O is one of the products.

9. C-bonding
• 8. The pair(s) of reagents that yield paramagnetic species is/are
• (A) Na and excess of NH3
• (B) K and excess of O2
• (C) Cu and dilute HNO3
• (D) O2 and 2-ethylanthraquinol
• 8 (A), (B), (C)
• K excess O KO (Superoxide) 2 2 + ⎯⎯→ → Paramagnetic
• 3 32 2 3Cu 8HNO 3Cu(NO ) 2NO 4H O + ⎯⎯→ + + → Paramagnetic

10. 9. A list of species having the formula XZ4 is given below.
• XeF4, SF4, SiF4, BF4−, [Cu(NH3)4]2+, [FeCI4]2−, [CoCl4]2− and [PtCI4]2−.
• Defining shape on the basis of the location of X and Z atoms, the total
number of species
• having a square planar shape is
• 9 [4]
• XeF4 , BrF4− , [Cu(NH3)4]+2 , [PtCl4]2−

11. inorganic
• 10. Among PbS, CuS, HgS, MnS, Ag2S, NiS, CoS, Bi2S3 and SnS2, the total
number of
• BLACK coloured sulphides is
• 10. [7]
• PbS , CuS, HgS, Ag2S, NiS, CoS, Bi2S3

12. inorganic
• 11. Consider the following list of reagents:
• Acidified K2Cr2O7, alkaline KMnO4, CuSO4, H2O2, CI2, O3, FeCI3, HNO3 and
Na2S2O3.
• The total number of reagents that can oxidise aqueous iodide to iodine is
• 11. [7]
• H+
• / K2Cr2O7 , OH / KMnO4 , CuSO4 , H2O2 , Cl2 , O3, HNO

13. Physical chemistry -solution
• 12. A compound H2X with molar weight of 80 g is dissolved in a solvent having density of
• 0.4 g ml−1
• . Assuming no change in volume upon dissolution, the molality of a 3.2 molar
• solution is
• 12. [8]
• Let us consider, volume of solution = 1 litre = 1000 mL
• wt. of solvent = 0.4 × 1000 = 400 g = 0.4 kg
• wt. of solute = 80 g ; no. of moles of solute = 3.2 moles
• molality of solution = 3.2