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IBChemistry: HLDPPractice Paper QuestionsSet BPractice Paper 1

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First teaching 2014

Last exams 2024

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Practice Paper 1 (DP IB Chemistry: HL)

Practice Paper Questions

1
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Excess dilute hydrochloric acid is added separately to equal masses of the four metals, calcium, zinc, magnesium and strontium. Which metal will give off the largest volume of hydrogen gas in the reaction?

  • calcium

  • zinc

  • magnesium

  • strontium

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2
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The glass containers X and Y are connected by a closed valve.1-2-h-q11-ib-chemistry-mcqs

X contains pure CO2 gas at 25 °C and a pressure of 1 × 105 Pa. Container Y has been evacuated prior to the experiment and has a volume three times bigger than container X.

During the experiment, the valve is opened, and the temperature of the whole apparatus is raised to 160 °C.

What is the final pressure in the system?

  • fraction numerator 1 space cross times space 10 to the power of 5 space cross times space 160 over denominator 4 space cross times space 25 end fraction

  • fraction numerator 4 space cross times space 10 to the power of 5 space cross times space 433 over denominator 3 space cross times space 298 end fraction

  • fraction numerator 1 space cross times space 10 to the power of 5 space cross times space 433 over denominator 3 space cross times space 298 end fraction

  • fraction numerator 1 space cross times space 10 to the power of 5 space cross times space 433 over denominator 4 space cross times space 298 end fraction

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3
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The diagram below shows the skeletal formula of phenazine.1-1-m-q9-ib-chemistry-mcqsWhat is the empirical formula of phenazine?

  • C6H6N

  • C12H8N2

  • C6H4N

  • C12H12N2

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4
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The mass spectrum of element X is shown below.

2-1-m-q9-mcqs-ib-chemistry
Which of the following statements is correct?

  • X has a relative atomic mass between 70 and 71

  • The three isotopes of X are separated after being converted to anions

  • The most abundant isotope of X contains 71 neutrons

  • The isotope of X with mass 72 will be deflected the most

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5
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Successive ionisation energies for an element, Y, are shown in the table below.

Electrons removed

1st

2nd

3rd

4th

5th
Ionisation energy / kJ mol-1

736

1450

7740

10500

13600

What is the most likely formula for the ion of Y?

  • Y+

  • Y2+

  • Y3+

  • Y4+

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6
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A spectral line that would be found in the visible spectrum of the hydrogen emission spectrum would be

  • n1 → n2

  • n2 → n3

  • n3 → n2

  • n3 → n∞

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7
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Use a periodic table to deduce the correct information about the element tin, Sn (Z = 50)

  Number of occupied
main energy levels		 Number of electrons in the
highest main energy level

A

4

4

B

4

14

C

5

4

D

5

14

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    8
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    Which complex is likely to be colourless?

    • [Zn(H2O)6]Cl2

    • [NH4]2[Fe(H2O)6][SO4]2

    • K3[Co(CN)6]

    • [Ni(NH3)6][BF4]2

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    9
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    Which type of bonding can be described as ‘the electrostatic attraction between positive nuclei and electrons and occurs by the sharing of electrons’? 

    • Hydrogen bonding

    • Ionic bonding 

    • Metallic bonding 

    • Covalent bonding 

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    10
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    Which of the following are properties of transition metals?

    1. They have variable oxidation states
    2. They can behave as catalysts
    3. They can have magnetic properties

    • I and II only

    • I and III only

    • II and III only

    • I, II and III

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    11
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    Which is a characteristic property of sodium oxide?

    • It turns moist litmus paper blue

    • It turns moist litmus paper red

    • When it dissolves in distilled water it forms a solution with pH less than 7

    • It reacts with magnesium metal

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    12
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    Sulfur forms the compound S4N4 with nitrogen, the structure is shown below.q10_4-2_ib_sl_hard_mcq

      Which of the following statements about S4N4 is correct?

    • The sulfur atom marked x has two lone pairs

    • The sulfur atom marked y has two lone pairs

    • Each N atom has two lone pairs 

    • The N-S-N bond angle will be larger than S=N=S bond angle 

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    13
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    Which combination describes the PH4+ ion?

     

    Molecular geometry

    Central atom hybridisation

    A

    Tetrahedral

    sp3

    B

    Square planar

    sp3

    C

    Tetrahedral

    sp2

    D

    Square planar

    sp2

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      14
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      Which enthalpy changes correctly describe the following reactions? 

      Reaction 1: HNO3 (aq) + NH3 (aq) → NH4NO3 (aq)

      Reaction 2: CuCO3 (s) → CuO (s) + CO2 (g)

      Reaction 3: S (s) + O2 (g) → SO2 (g)

       

      ΔHӨc

      ΔHӨf

      ΔHӨneut

      ΔHӨr

      A

      2

      2

      1

      3

      B

      3

      2

      1

      2

      C

      3

      3

      1

      2

      D

      2

      3

      1

      3

       

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        15
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        Bond energy calculations show the enthalpy of combustion for propene to be -1572.0 kJ mol-1.

        Compound

        C3H6 (g)

        CO2 (g)

        H2O (l)

        H2O (g)

        ΔHӨf / kJ mol-1

        +20.0

        -393.5

        -285.8

        -241.8

          

        Using the enthalpy of formation data, which calculation correctly shows the percentage error between propene’s enthalpy of combustion values obtained from bond energy calculations and Hess’s Law calculations, assuming the bond energy calculation value is correct?

        • begin mathsize 14px style fraction numerator negative 1572.0 over denominator left parenthesis left parenthesis 3 space cross times space minus 393.5 right parenthesis space plus space left parenthesis 3 space cross times space minus 241.8 right parenthesis space minus space left parenthesis 20 right parenthesis right parenthesis space minus space 1572.0 end fraction x space 100 end style

        • begin mathsize 14px style fraction numerator left parenthesis 3 space cross times space minus 393.5 right parenthesis space plus space left parenthesis 3 space cross times space minus 241.8 right parenthesis space minus space left parenthesis 20 right parenthesis over denominator negative 1572.0 end fraction x space 100 end style

        • begin mathsize 14px style fraction numerator left parenthesis 3 space cross times space minus 393.5 right parenthesis space plus space left parenthesis 3 space cross times space minus 241.8 right parenthesis space plus space left parenthesis 20 right parenthesis over denominator negative 1572.0 end fraction cross times 100 end style

        • begin mathsize 14px style fraction numerator left parenthesis left parenthesis 3 space cross times space minus 393.5 right parenthesis space plus space left parenthesis 3 space cross times space minus 241.8 right parenthesis space minus space left parenthesis 20 right parenthesis right parenthesis space minus space left parenthesis negative 1572.0 right parenthesis over denominator negative 1572.0 end fraction cross times space 100 end style

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        16
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        The ΔGϴf values for the following substances are shown.

        Substance

        ΔGϴf (kJ mol-1)

        NH3 (g)

        -16.4

        O2 (g)

        0

        H2O (g)

        -228.6

        NO (g)

        87.6

         

        Which of the following is the correct calculation to determine ΔGϴ? 

        4NH3 (g) + 5O2 (g) ⇌ 6H2O (g) + 4NO (g)

        • (-228.6 + 87.6) + (-16.4)

        • (-16.4 x 4) - [(-228.6 x 6) + (87.6 x 4)]

        • [-228.6 + (87.6 x 4)] - (-16.4 x 4)

        • [(-228.6 x 6) + (87.6 x 4)] - (-16.4 x 4)

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        17
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        Which statements are correct for ionic compounds?

        1. Solubility in water depends on the relative magnitude of the lattice energy compared to the hydration energy
        2. Melting points of ionic compounds increase as the size of the cation increases
        3. The enthalpy of solution for calcium chloride is represented by CaCl2 (s) → CaCl2 (aq)

        • I and II only

        • I and III only

        • II and III only

        • I, II and III

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        18
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        A student performs to reactions and measures the rate of product formation.

        Reaction 1: 1.5g of solid calcium carbonate is added to 100 cm3 of 0.5 M hydrochloric acid

        Reaction 2: 100 cm3 of distilled water is then added to 100 cm3 of 0.5 M hydrochloric acid then 1.5g of solid calcium carbonate is added

        The rate of reaction 1 was faster than the rate of reaction 2.

        Which of the following 3 hypotheses correctly describes the difference in the rate?

        1

        Adding water reduces the frequency of collisions between reactant molecules.

        2

        Adding water reduces the proportion of effective collisions between reactant molecules.

        3

        Adding water reduces the proportion of reactant molecules possessing the activation energy.

        • 1 only

        • 1 and 2 only

        • 3 only

        • 1, 2 and 3

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        19
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        The stoichiometry of a catalysed reaction is shown by the equation below.

        R (g) + S (g)  ⇌ T (g) + U (g)

        Two experiments were carried out in which the amount of product T was measured against time. The results are shown in the diagram below.

        q9-6-1-hard

        Which changes in the conditions from experiment 1 to experiment 2 might explain the results shown?

        1

        product U was continuously removed from the equilibrium mixture

        2

        a different catalyst was used

        3

        less of reactant R was used

        • 1 only

        • 1 and 3 only

        • 2 and 3 only

        • 1, 2 and 3

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        20
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        A student experimentally determined the rate expression for the reaction between iodine and propanone to be: 

        Rate = k [H+] [C3H6O] 

        Which graph is consistent with this information?

        q2_16-1_-medium-rate-expression--reaction-mechanism_ib_hl

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          21
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          The following information was obtained for the rate constant, k, for a reaction at 25 OC

          A

          Ea

          R

          2.57 × 109 s–1

          96.2 kJ mol–1

          8.31 J K–1 mol–1

          Which expression correctly represents how to calculate the rate constant, k?

          • k = (2.57 x 109) x e(-96.2 / 8.31×25)

          • k = (2.57 x 109) x e(-96.2 / 8.31×298)

          • k = (2.57 x 109) x e(-96200 / 8.31×25)

          • k = (2.57 x 109) x e(-96200 / 8.31×298)

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          22
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          Consider the following reversible reaction:

          3O2 (g) ⇌ 2O3 (g) 

          What is the value of Kc when the equilibrium concentrations are [O2] = 4.0 mol dm-3 and [O3] = 4.0 mol dm-3 ?

          • 0.25

          • 4

          • 16

          • 64

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          23
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          Which of the following equations is used when calculating the temperature, in Kelvin, at which a reaction becomes feasible if ΔHΘ = x and ΔSΘ = y.

          • T = begin mathsize 14px style x over y end style

          • T = x y

          • T = x + y

          • T = begin mathsize 14px style italic y over italic x end style

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          24
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          In the Brønsted–Lowry theory of acids and bases, the difference between a conjugate acid and its conjugate base is the presence of which of the following?

          • a positive charge

          • a pair of electrons

          • a proton

          • a hydrogen atom

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          25
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          How many different types of ions can be found in acid rain, assuming it contains a mixture of sulfuric, sulfurous, nitric and nitrous acids?

          • 4

          • 5

          • 6

          • 7

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          26
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          Which of the following statements are correct for a titration between 0.10 mol dm-3 propanoic acid and 0.10 mol dm-3 potassium hydroxide? 

          • The equivalence point will be at pH 7

          • The salt formed will hydrolyse to form an acidic salt 

          • The salt formed will be CH3COOK

          • At half equivalence point [CH3CH2COOH (aq)] = [CH3CH2COO- (aq)]

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          27
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          Which of the following statements is correct? 

          • As temperature increases, the pH value of pure water decreases

          • As temperature decreases, the pH value of pure water decreases

          • The pH of water is unaffected by temperature 

          • Pure water is not neutral 

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          28
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          Below is a diagram of a voltaic cell. When the cell is running, what is happening in the salt bridge?

          9-1-mcq-q10-ib-chemistry

          • K+ ions flow to the zinc half-cell and NO3− ions flow to the copper half-cell

          • K+ ions flow to the copper half-cell and NO3− ions flow to the zinc half-cell

          • K+ and NO3− ions flow to the copper half-cell

          • K+ and NO3− ions flow to the zinc half-cell

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          29
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          Which of the following reactions could take place at the positive electrode (cathode) in a voltaic cell? 

          1.   Cu2+ (aq) to Cu (s)
          2.   Br2 (g) to Br- (aq)
          3.   Co3+ (aq) to Co2+(aq)

          • I and II only

          • I and III only

          • II and III only

          • I, II and III

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          30
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          Consider these standard electrode potentials.

          Fe2+ (aq) + 2e- rightwards harpoon over leftwards harpoonFe (s) EΘ = -0.45 V

          Cu2+ (aq) + 2e- rightwards harpoon over leftwards harpoonCu (s) EΘ = +0.15 V

          Which is the correct working to determine EΘcell?

          • EΘcell = 0.15 - (-0.45)

          • EΘcell = 0.15 + (-0.45)

          • EΘcell = (-0.45) - 0.15

          • EΘcell = 0.15 x (-0.45)

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          31
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          What types of isomerism can the following molecule show?

          10-1-h-q9-mcqs-ib-chemistry

          I.
          Branch-chain
          II.
          Positional 
          III.
          Functional group

          • I and II only

          • I and III only

          • II and III only

          • I, II and III

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          32
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          Which factors affect the rate of nucleophilic substitution in halogenoalkanes?

          1. The nature of the attacking nucleophile
          2. The structure of the halogenoalkane
          3. The identity of the halogen

          •  I and II only

          •  I and III only

          • II and III only

          • I, II and III

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          33
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          Compound Q has the formula CH3CH2CO2CH3

          What is the name of compound Q and how does its boiling point compare with that of butanoic acid?

           

          name of Q

          boiling point compared to butanoic acid

          A

          B

          C

          D

          methyl propanoate

          propyl methanoate

          methyl propanoate

          propyl methanoate

          lower

          lower

          higher

          higher

           

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            34
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            An alkene, X, undergoes electrophilic addition with hydrogen bromide to form a halogenoalkane, Y, as the minor product. 

            The halogenoalkane, Y , can react with sodium hydroxide in aqueous conditions to form butan-1-ol. 

            What is the correct identity of the alkene, X? 

            • 2-methylpropene

            • But-1-ene

            • But-2-ene 

            • Pent-1-ene

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            35
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            In the presence of an H+ catalyst, compound X reacts with ethanoic acid to produce the compound below.

            10-2-m-q8-ib-chemistry-mcqs

            What is the molecular formula of compound X?

            • C4H8O 

            • C4H8O2

            • C2H6O2

            • C2H6O3

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            36
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            What is this molecule called?
            q2_20-3_ib_hl_medium_mcq

            • Z-2-bromo-1-chloro-2-fluoroethene

            • E-2-bromo-1-chloro-2-fluoroethene

            • Z-1-bromo-2-chloro-1-fluoroethene

            • E-1-bromo-2-chloro-1-fluoroethene

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            37
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            The synthesis of 2-propyl propanoate can be carried out in two steps:

                                                           I                                

                                     CH3COCH3   →  CH3CH(OH)CH3

                                                           II   

                              CH3CH(OH)CH3  → C2H5COOCH(CH3)2 

            What are the reagents needed in I and II?

             

            I

            II

            A

            potassium dichromate(VI)

            sulfuric acid, propanoic acid

            B

            sodium borohydride

            sulfuric acid, propanoic acid

            C

            sodium borohydride

            sulfuric acid, ethanoic acid

            D

            potassium dichromate(VI)

            sulfuric acid, ethanoic acid

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              38
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              Which molecule has an index of hydrogen deficiency (IHD) = 1?

              • C6H10

              • C2Br2

              • C4H9N

              • C3H8O

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              39
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              The 1H NMR spectrum of CH3CHCl2 shows two signals.

              What is the correct assignment of splitting patterns for these signals?

                CH3 group CH group
              A doublet quartet
              B quartet doublet
              C singlet singlet
              D triplet singlet

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                40
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                Which row correctly describes the splitting pattern observed on the 1H NMR spectrum for each labelled hydrogen?


                q2_21-1_spectroscopic-identification-of-organic-compounds_medium_ib_hl

                • One doublet and four triplets

                • One triplet, one quartet and one singlet

                • One triplet, one doublet and three singlets

                • One triplet, one quartet and three singlets

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