Question 1

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Question 2

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Question 3

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Question 4

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Question 5

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Question 6

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Question 7

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Which of the following statements describes first ionisation energy?

The energy required to remove one mole of electrons from one mole of gaseous atoms
The energy required to remove the outermost electron from each atom in one mole of gaseous atoms
The energy required to remove the outermost electron from each atom in one mole of atoms
The energy required to produce one mole of ions from one mole of gaseous atoms

Question 8

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The electronegativity of four elements are given below

N = 3.0 H = 2.1 F = 4.0 P = 2.1

What is the correct order of polarity for the following compounds

PH₃ < PF₃ < NF₃ < NH₃
PH₃ < PF₃ < NH₃ < NF₃
NF₃< NH₃ < PH₃ < PF₃
PH₃ < NH₃ < NF₃< PF₃

Question 9

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Which of the species shown below does not have resonance structures?

C₆H₆
CO₃^2-
C₂H₄
O₃

Question 10

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What is the strongest type of intermolecular force exhibited in the amino acid molecule serine?

Otne2dIl_q3_4-3_ib_sl_medium_mcq

London dispersion forces
Permanent dipole permanent dipole forces
Hydrogen bonding
Covalent bonding

Question 11

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Which of the following molecules will have the highest boiling point?

CH₃CH₂CHO
CH₃CH₂CH₂NH₂
CH₃CH₂OCH₃
CH₃CH₂CH₂F

Question 12

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An experiment was carried out to determine the approximate value for the molar enthalpy change of neutralisation.

75 cm³ of 3.00 mol dm^–3 hydrochloric acid was placed in a polystyrene beaker of negligible heat capacity. Its temperature was recorded, and then 75 cm³ of
3.00 mol dm⁻³potassium hydroxide at the same temperature was quickly added, and the solution stirred.

The temperature rose by 14 °C. The resulting solution may be considered to have a specific heat capacity of 4.18 J g^-1K^-1.

Which calculation below is correct?

$- \frac{(75 \times 4.18 \times 14)}{(6.0 \times 0.150)}$ J mol^-1
$- \frac{(150 \times 4.18 \times 14)}{(3.0 \times 0.075)}$ J mol^-1
$- \frac{(150 \times 4.18 \times 14)}{(3.0 \times 75.0)}$ J mol^-1
$- \frac{(75 \times 4.18 \times 287)}{(6.0 \times 0.150)}$ J mol^-1

Question 13

Marks: 1

The equations below show the formation of sulfur oxides from sulfur and oxygen.

S(s) + O₂(g) → SO₂(g) $∆ H_{f}^{⦵}$ = –297 kJ mol^–1

S(s) + 1½O₂(g) →SO₃(g) $∆ H_{f}^{⦵}$ = –395 kJ mol^–1

What is the enthalpy change of reaction, $∆ H^{⦵}$ ,of 2SO₂(g) + O₂(g) → 2SO₃(g) in kJ mol^–1?

(794 − 594)
(296 + 395)
(− 395 + 297)
(−790 + 594)

Question 14

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The reaction pathway for a reversible reaction is shown below: q1_5-3_ib_sl_easy_mcq

Which statement is correct?

The activation energy of the reverse reaction is +90 kJ mol^–1
The activation energy of the forward reaction is +20 kJ mol^–1
The activation of the reverse reaction is +20 kJ mol^–1
The enthalpy change of forwards reaction is - 70 kJ mol^–1

Question 15

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The diagram shows the skeletal formula of cyclobutane.
q3_5-3_mcq_hard_ib-chemistry-sl

The enthalpy change of formation of cyclobutane is +75.1 kJ mol^–1, and the enthalpy change of atomisation of graphite is +712 kJ mol^–1.

The bond enthalpy of C–H is 414 kJ mol^–1 and of H–H is 436 kJ mol^–1.

What is the average bond enthalpy of the C–C bond in cyclobutane?

$712 - 436 + 2 (414) + \frac{75.1}{4}$
$712 + 436 - 414 - \frac{75.1}{4}$
$712 + 436 - 2 (414) - \frac{75.1}{4}$
$712 + 436 - 2 (414) - 75.1$

Question 16

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Question 17

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Question 18

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Question 19

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Question 20

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What role does each species play in the equilibrium below according to Brønsted-Lowry theory?

CH₃COOH + HCl ⇌ CH₃COOH₂⁺ + Cl^-

	CH₃COOH	HCl	CH₃COOH₂⁺	Cl^-
A	acid	base	base	acid
B	acid	base	acid	base
C	base	acid	base	acid
D	base	acid	acid	base

Question 21

Marks: 1

Four 1.0 M solutions of HCl, NH₃, NaOH and CH₃COOH have been mislabelled, but a student has a pH meter to test the pH of the solutions. Arrange the solutions in order of increasing pH:

HCl (aq) < NH₃ (aq) < NaOH (aq) < CH₃COOH (aq)
CH₃COOH (aq) < HCl (aq) < NH₃ (aq) < NaOH (aq)
HCl (aq) < CH₃COOH (aq) < NH₃ (aq) < NaOH (aq)
NaOH (aq) < NH₃ (aq) < CH₃COOH (aq) < HCl (aq)

Question 22

Marks: 1

The pH of clean rain water is around 5.5. Which substance is responsible for this?

Methane
Carbon dioxide
Nitrogen oxides
Sulfur dioxide

Question 23

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Question 24

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Question 25

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Question 26

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Question 27

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Question 28

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Question 29

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Question 30

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DP IB Chemistry: SL

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