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FSc Part 1 Chemistry MCQs with answers

Practise FSc Part 1 Chemistry (Part 1) with 300 exam-style MCQs, each with the answer and a short explanation. Every test is marked the moment you finish and shows your score chapter by chapter, so you know what to revise next. It is free and needs no sign-up.

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FSc Part 1 Chemistry MCQs with answers

Practise FSc Part 1 Chemistry (Part 1) with 300 exam-style MCQs, each with the answer and a short explanation. Every test is marked the moment you finish and shows your score chapter by chapter, so you know what to revise next. It is free and needs no sign-up.

300 questions · 11 chapters

What each chapter covers 11 chapters

The questions follow the syllabus chapter by chapter. You can test the whole subject or one chapter at a time.

  1. Basic concepts 30 questionsAtoms, molecules, ions and isotopes, The mole and Avogadro's number, Stoichiometry, limiting reactant and yield
  2. Experimental techniques in chemistry 20 questionsFiltration, crystallisation and sublimation, Solvent extraction and chromatography
  3. Gases 30 questionsGas laws and the ideal gas equation, Dalton's law, Graham's law and kinetic molecular theory, Non-ideal behaviour, liquefaction and plasma
  4. Liquids and solids 32 questionsIntermolecular forces and hydrogen bonding, Evaporation, vapour pressure, boiling point and liquid crystals, Crystalline solids
  5. Atomic structure 30 questionsDiscovery of subatomic particles and Rutherford's model, Planck's theory, Bohr's model and the hydrogen spectrum, Quantum numbers, orbitals and electronic configuration
  6. Chemical bonding 29 questionsPeriodic trends, ionic and covalent bonds, VSEPR theory, valence bond theory and hybridisation, Molecular orbital theory, bond energy and dipole moment
  7. Thermochemistry 20 questionsEnergy, the first law and enthalpy, Standard enthalpy changes, Hess's law and the Born-Haber cycle
  8. Chemical equilibrium 29 questionsLaw of mass action, Kc and Kp, Le Chatelier's principle and industrial applications, Ionic equilibria: pH, buffers and solubility product
  9. Solutions 29 questionsConcentration units, Raoult's law, ideal and non-ideal solutions, Colligative properties, hydration and hydrolysis
  10. Electrochemistry 29 questionsOxidation numbers and balancing redox equations, Electrolysis and electrolytic cells, Galvanic cells, electrode potentials and batteries
  11. Reaction kinetics 22 questionsRate of reaction, order and half-life, Activation energy, factors affecting rate and catalysis
Sample FSc Part 1 Chemistry MCQs with answers 12 questions

12 questions from the test, one or two from each chapter. Try each one, then open the answer.

1. 5.4 g of aluminium is heated with 14.2 g of chlorine. What mass of AlCl3 can form? 2Al + 3Cl2 → 2AlCl3 (AlCl3 = 133.5)

  1. A
    26.7 g
  2. B
    17.8 g
  3. C
    19.6 g
  4. D
    13.35 g
Show answer

Answer: B. Al = 0.2 mol needs 0.3 mol Cl2, but only 0.2 mol Cl2 is present, so Cl2 limits: 0.2 × 2/3 = 0.1333 mol AlCl3 × 133.5 = 17.8 g. 26.7 g assumes Al is limiting.

2. Paper chromatography is classified as

  1. A
    partition chromatography
  2. B
    adsorption chromatography
  3. C
    ion-exchange chromatography
  4. D
    gas chromatography
Show answer

Answer: A. Components are distributed (partitioned) between the water held on the paper and the moving solvent, so it is partition chromatography.

3. 500 cm3 of a gas is at 1 atm and 27 °C. What is its volume at 2 atm and 327 °C?

  1. A
    250 cm3
  2. B
    500 cm3
  3. C
    1000 cm3
  4. D
    3028 cm3
Show answer

Answer: B. V2 = V1 × (P1/P2) × (T2/T1) = 500 × (1/2) × (600/300) = 500 cm3. Doubling pressure halves V, doubling kelvin temperature doubles it.

4. Water boils at about 98 °C at Murree. Why is this lower than 100 °C?

  1. A
    the vapour pressure of water is higher at Murree
  2. B
    the water there is purer
  3. C
    the external atmospheric pressure is lower
  4. D
    the air is colder
Show answer

Answer: C. At high altitude atmospheric pressure is lower, so water's vapour pressure equals it at a lower temperature.

5. In Rutherford's experiment, most α-particles passed straight through the gold foil. What did this show?

  1. A
    the nucleus is negatively charged
  2. B
    most of the atom is empty space
  3. C
    electrons are very heavy
  4. D
    the atom is a solid sphere of positive charge
Show answer

Answer: B. Only a very few α-particles were strongly deflected, so the positive charge and mass are concentrated in a tiny nucleus and the rest is mostly empty.

6. What is the hybridisation of each carbon atom in ethene, C2H4?

  1. A
    sp
  2. B
    sp2
  3. C
    sp3
  4. D
    sp3d
Show answer

Answer: B. Each C forms three σ bonds (trigonal planar, 120°) using sp2 orbitals; the unhybridised p orbitals overlap sideways to form the π bond.

7. Hess's law of constant heat summation follows from the fact that

  1. A
    a catalyst does not change ΔH
  2. B
    mass is conserved in a reaction
  3. C
    all reactions are exothermic
  4. D
    enthalpy is a state function, so ΔH depends only on the initial and final states
Show answer

Answer: D. Whatever route is taken between the same reactants and products, the total enthalpy change is the same, because H is a state function.

8. For H2(g) + I2(g) ⇌ 2HI(g), the equilibrium concentrations are [H2] = 0.10, [I2] = 0.10 and [HI] = 0.70 mol dm−3. What is Kc?

  1. A
    7.0
  2. B
    49
  3. C
    70
  4. D
    0.020
Show answer

Answer: B. Kc = [HI]2 ÷ ([H2][I2]) = 0.49 ÷ 0.010 = 49. Forgetting to square [HI] gives 70.

9. 1.8 g of a non-electrolyte in 100 g of water lowers the freezing point by 0.186 K. Kf = 1.86 K kg mol−1. What is the molar mass of the solute?

  1. A
    18 g mol−1
  2. B
    360 g mol−1
  3. C
    180 g mol−1
  4. D
    1.8 g mol−1
Show answer

Answer: C. M = (Kf × 1000 × w2) ÷ (ΔTf × w1) = (1.86 × 1000 × 1.8) ÷ (0.186 × 100) = 3348 ÷ 18.6 = 180 g mol−1.

10. What is the oxidation number of chromium in K2Cr2O7?

  1. A
    +7
  2. B
    +3
  3. C
    +12
  4. D
    +6
Show answer

Answer: D. 2(+1) + 2x + 7(−2) = 0, so 2x = 12 and x = +6. +12 is the total for both Cr atoms.

11. The rate equation of a reaction is rate = k[A]2[B]. What is the overall order of the reaction?

  1. A
    first
  2. B
    second
  3. C
    third
  4. D
    fourth
Show answer

Answer: C. The overall order is the sum of the powers in the rate equation: 2 + 1 = 3. The order is found by experiment, not from the balanced equation.

12. Which element has the largest number of naturally occurring stable isotopes?

  1. A
    carbon
  2. B
    tin
  3. C
    fluorine
  4. D
    chlorine
Show answer

Answer: B. Tin has ten stable isotopes, the most of any element. Fluorine has only one, and carbon and chlorine have two each.

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The 300 MCQs are our own, written to the syllabus in the style of the exam.

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