CUET UG Chemistry Syllabus

Chemistry syllabus — full chapter and topic list

Expand any chapter to see its topics and sub-topics. This is the whole examinable outline for Chemistry in CUET UG, not a summary of it.

1. 1

   Physical Chemistry

   3 topics

   • Solutions
     • Concentration and Raoult's law
     • Colligative properties
     • Abnormal molar mass and van't Hoff factor
   • Electrochemistry
     • Electrochemical cells and EMF
     • Nernst equation and conductance
     • Electrolysis and batteries
   • Chemical Kinetics
     • Rate of reaction and order
     • Integrated rate equations
     • Arrhenius equation and collision theory
2. 2

   Inorganic Chemistry

   3 topics

   • The d- and f-Block Elements
     • Transition metal properties
     • Lanthanoids and actinoids
     • Important compounds (KMnO4, K2Cr2O7)
   • Coordination Compounds
     • Werner's theory and nomenclature
     • Isomerism in coordination compounds
     • Valence bond and crystal field theory
   • p-Block Elements
     • Group 15 to 18 trends
     • Oxoacids and important compounds
3. 3

   Organic Chemistry

   4 topics

   • Haloalkanes and Haloarenes
     • Nomenclature and preparation
     • SN1 and SN2 mechanisms
   • Alcohols, Phenols and Ethers
     • Preparation and properties
     • Reactions of phenols
   • Aldehydes, Ketones and Carboxylic Acids
     • Nucleophilic addition reactions
     • Acidity of carboxylic acids
   • Amines and Nitrogen Compounds
     • Classification and basicity
     • Diazonium salts
4. 4

   Biomolecules and Applied Chemistry

   3 topics

   • Biomolecules
     • Carbohydrates and proteins
     • Nucleic acids and vitamins
   • Polymers
     • Classification and types of polymerisation
     • Important synthetic polymers
   • Chemistry in Everyday Life
     • Drugs and medicines
     • Cleansing agents

Chemistry flashcards for CUET UG

21 of 78 cards from the Chemistry deck — real questions with worked answers.

1. What is the relationship between relative lowering of vapour pressure and mole fraction of solute (Raoult's law for non-volatile solute)?

   The relative lowering of vapour pressure equals the mole fraction of the solute: (p°−p)/p° = x_solute.

2. Define molality and give its formula.

   Molality (m) is the number of moles of solute per kilogram of solvent: m = (moles of solute) / (mass of solvent in kg). It is independent of temperature.

3. What is the van't Hoff factor (i) and what does i>1 versus i<1 indicate?

   i = (observed colligative property)/(calculated value). i>1 indicates dissociation of solute; i<1 indicates association of solute.

4. Write the formula for elevation of boiling point and depression of freezing point.

   ΔTb = i·Kb·m (Kb = molal elevation/ebullioscopic constant); ΔTf = i·Kf·m (Kf = molal depression/cryoscopic constant).

5. State the formula for osmotic pressure of a dilute solution.

   π = i·C·R·T, where C is molar concentration, R the gas constant, and T the absolute temperature. (π = (n/V)RT)

6. What is Henry's law and its mathematical expression?

   The partial pressure of a gas above a solution is proportional to its mole fraction in solution: p = KH·x, where KH is Henry's constant. KH increases with temperature (gas solubility decreases).

7. Distinguish positive and negative deviations from Raoult's law in terms of A–B interactions.

   Positive deviation: A–B interactions weaker than A–A/B–B; ΔH > 0, ΔV > 0 (e.g. ethanol+acetone). Negative deviation: A–B interactions stronger; ΔH < 0, ΔV < 0 (e.g. chloroform+acetone).

8. What are colligative properties? Name the four.

   Properties depending on the number of solute particles, not their nature: (1) relative lowering of vapour pressure, (2) elevation of boiling point, (3) depression of freezing point, (4) osmotic pressure.

9. Write the Nernst equation for an electrode/cell at 298 K (using log).

   Ecell = E°cell − (0.0591/n)·log Q, where n = number of electrons transferred and Q = reaction quotient.

10. Relate standard cell potential to Gibbs free energy and to the equilibrium constant.

    ΔG° = −nFE°cell; and E°cell = (0.0591/n)·log Kc at 298 K (so ΔG° = −RT ln K).

11. Define molar conductivity and how it varies with dilution.

    Molar conductivity Λm = κ·1000/C (S cm² mol⁻¹). It increases on dilution for both strong and weak electrolytes (more so for weak electrolytes).

12. State Kohlrausch's law of independent migration of ions.

    The limiting molar conductivity of an electrolyte is the sum of individual contributions of its cation and anion: Λ°m = ν₊λ°₊ + ν₋λ°₋.

13. State Faraday's first law of electrolysis and the value of the Faraday constant.

    Mass deposited is proportional to charge passed: m = (E·I·t)/F (E = equivalent weight). One Faraday = 96500 C = charge on one mole of electrons.

14. What are the electrode reactions and use of a hydrogen–oxygen fuel cell?

    Anode: H₂ + 2OH⁻ → 2H₂O + 2e⁻; Cathode: O₂ + 2H₂O + 4e⁻ → 4OH⁻. Overall: 2H₂ + O₂ → 2H₂O. It converts chemical energy directly to electrical energy.

15. Write the cell reactions of a lead storage battery during discharge.

    Anode: Pb + SO₄²⁻ → PbSO₄ + 2e⁻; Cathode: PbO₂ + SO₄²⁻ + 4H⁺ + 2e⁻ → PbSO₄ + 2H₂O. Electrolyte is H₂SO₄.

16. Define corrosion and give the electrochemical basis of rusting of iron.

    Corrosion is the slow oxidation of metal by environment. In rusting, Fe is oxidized (anode: Fe→Fe²⁺+2e⁻), O₂+H₂O reduced (cathode), and Fe²⁺ is further oxidized to hydrated Fe₂O₃·xH₂O (rust).

17. Write the integrated rate law and half-life of a first-order reaction.

    k = (2.303/t)·log([A]₀/[A]); t₁/₂ = 0.693/k (independent of initial concentration).

18. For a zero-order reaction, give the rate expression, integrated form, and half-life.

    Rate = k (constant); [A] = [A]₀ − kt; t₁/₂ = [A]₀/2k.

19. Define order and molecularity of a reaction and one key difference.

    Order = sum of powers of concentration terms in the experimental rate law (can be zero/fractional). Molecularity = number of species in an elementary step (always a whole number ≥1). Order is experimental; molecularity is theoretical.

20. State the Arrhenius equation and the meaning of each term.

    k = A·e^(−Ea/RT), where A = pre-exponential (frequency) factor, Ea = activation energy, R = gas constant, T = absolute temperature.

21. How does a catalyst increase reaction rate according to collision/activation theory?

    A catalyst provides an alternative reaction path with lower activation energy, so a larger fraction of molecules can react; it does not change ΔH or the equilibrium position.

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