Questions 1
Topic – 6.1 Redox processes: electron transfer and changes in oxidation number (oxidation state)
Four equations representing reactions of nitrogen or one of its compounds are given. Which equation represents a disproportionation reaction?
A \(2HNO_3 + CaCO_3 → Ca(NO_3)_2 + CO_2 + H_2O\)
B \(N_2 + 3H_2 → 2NH_3\)
C \(NH_4Cl + NaOH → NH_3 + NaCl + H_2O\)
D \(2NO_2 + H_2O → HNO_3 + HNO_2\)
▶️Answer/Explanation
Ans: D
Questions 2
Topic – 8.2 Effect of temperature on reaction rates and the concept of activation energy
The diagram shows the Boltzmann distribution for one mole of a gas. The gas takes part in a reaction with an activation energy, \(E_a\).
Which statement correctly describes the effect of an increase in temperature?
A Peak P will be higher and fewer molecules will have energy > \(E_a\).
B Peak P will be higher and more molecules will have energy > \(E_a\) .
C Peak P will be lower and fewer molecules will have energy > \(E_a\) .
D Peak P will be lower and more molecules will have energy > \(E_a\) .
▶️Answer/Explanation
Ans: D
Questions 3
Topic – 8.1 Rate of reaction
A student carries out four experiments to investigate the rate of reaction between 3.0 g of calcium carbonate and hydrochloric acid.
\(CaCO_3(s) + 2HCl(aq) → CaCl_2(aq) + CO_2(g) + H_2O(l)\)
experiment 1 \(CaCO_3\) powder + 2.0 \(mol dm^{–3}\) HCl at 35 °C
experiment 2 \(CaCO_3\) powder + 2.0 \(mol dm^{–3}\) HCl at 35 °C
experiment 3 large chips of \(CaCO_3\) + 1.0 \(mol dm^{–3}\) HCl at room temperature
experiment 4 large chips of \(CaCO_3\) + 1.0 \(mol dm^{–3}\) HCl at 35 °C
The student collects the \(CO_2(g)\) and times how long it takes to produce the same volume of gas for each experiment. What could be the correct times for the four experiments?
▶️Answer/Explanation
Ans: B
Questions 4
Topic – 7.1 Chemical equilibria: reversible reactions, dynamic equilibrium
The table shows the partial pressures in an equilibrium mixture formed by the Haber process.
What is the numerical value of the equilibrium constant, \(K_p\), for this reaction?
A \(4.46 × 10^{–9}\)
B \(4.76 × 10^{–5}\)
C \(7.14 × 10^{–5}\)
D \(2.24 × 10^8\)
▶️Answer/Explanation
Ans: A
Questions 5
Topic – 7.1 Chemical equilibria: reversible reactions, dynamic equilibrium
A reversible reaction is shown.
\(2NOCl(g) ⇌ 2NO(g) + Cl_2(g)\) \(∆H = +77.0 kJ mol^{–1}\)
Which change in conditions will move the position of equilibrium to the right and increase the value of the equilibrium constant?
A a decrease in pressure
B a decrease in temperature
C an increase in pressure
D an increase in temperature
▶️Answer/Explanation
Ans: D
Questions 6
Topic – 2.3 Formulas
The ore psilomelane may be considered to have the general formula \(Ba(Mn^{x+})(Mn^{y+})_8O_{16}(OH)_4\). In this general formula, x+ and y+ are the two different oxidation states of manganese in psilomelane. What could be the values of x and y?
▶️Answer/Explanation
Ans: A
Questions 7
Topic – 6.1 Redox processes: electron transfer and changes in oxidation number (oxidation state)
Silicon reacts with a mixture of calcium oxide and magnesium oxide at 1200°C.
\(2MgO + 2CaO + Si → 2Mg + Ca_2SiO_4\)
Which statement about this reaction is correct?
A Calcium is reduced and silicon is neither oxidised nor reduced.
B Magnesium is reduced and calcium is neither oxidised nor reduced.
C Magnesium is reduced and silicon is neither oxidised nor reduced.
D Silicon is reduced and calcium is neither oxidised nor reduced.
▶️Answer/Explanation
Ans: B
Questions 8
Topic – 3.4 Covalent bonding and coordinate (dative covalent) bonding
In which species is there a lone pair of electrons?
A \(CH_3\)
B \(CH_3^+\)
C\(CH_3^-\)
D \(CH_4\)
▶️Answer/Explanation
Ans: C
Questions 9
Topic – 4.1 The gaseous state: ideal and real gases and pV = nRT
Under which conditions will nitrogen behave most like an ideal gas?
▶️Answer/Explanation
Ans: B
Questions 10
Topic – 5.1 Enthalpy change, ΔH
The equation for a chemical reaction is shown. All substances are in their standard states.
\(XeF_6 + 3H_2O → XeO_3 + 6HF\)
Which statement describes the standard enthalpy change of reaction for this reaction?
A the enthalpy change when a total of one mole of products is produced
B the enthalpy change when a total of one mole of reactants is reacted
C the enthalpy change when one mole of water reacts
D the enthalpy change when six moles of hydrogen fluoride are produced
▶️Answer/Explanation
Ans: D
Questions 11
Topic – 2.1 Relative masses of atoms and molecules
Molten aluminium chloride has a simple molecular structure. Each molecule consists of two aluminium atoms and six chlorine atoms. Which statement is correct?
A All the chlorine atoms in 1 g of molten aluminium chloride have the same mass.
B One mole of molten aluminium chloride contains \(6.02 × 10^{23}\) aluminium atoms.
C One mole of molten aluminium chloride contains \(3.61 × 10^{24}\) chlorine atoms.
D The empirical formula of molten aluminium chloride is Al₂Cl₆.
▶️Answer/Explanation
Ans: C
Questions 12
Topic – 2.1 Relative masses of atoms and molecules
Which atom contains four times as many neutrons as the \(_3^7 Li\) atom?
A \(_{20}^{40} Ca\)
B \(_{12}^{24} Mg\)
C \(_{15}^{31} P\)
D \(_{14}^{28} Si\)
▶️Answer/Explanation
Ans: C
Questions 13
Topic – 1.4 Ionisation energy
Which statement about the first ionisation energies of magnesium and neon is correct?
A Magnesium has the greater numerical value and both are endothermic.
B Magnesium has the greater numerical value and both are exothermic.
C Neon has the greater numerical value and both are endothermic.
D Neon has the greater numerical value and both are exothermic.
▶️Answer/Explanation
Ans: C
Questions 14
Topic – 2.1 Relative masses of atoms and molecules
In a sample of pure water, what is the maximum number of hydrogen bonds that one molecule of water can be involved in?
A 1
B 2
C 3
D 4
▶️Answer/Explanation
Ans: D
Questions 15
Topic – 2.1 Relative masses of atoms and molecules
Hydrated cobalt(II) sulfate loses water when heated to give anhydrous cobalt(II) sulfate. All the water of crystallisation is lost to the atmosphere as steam. When 3.10 g of hydrated cobalt(II) sulfate, \(CoSO_4•xH_2O\), is heated to constant mass the loss in mass is 1.39 g. What is the value of x, to the nearest whole number?
A 4
B 6
C 7
D 11
▶️Answer/Explanation
Ans: C
Questions 16
Topic – 1.2 Isotopes
The table shows bond energies for some diatomic molecules. Deuterium, D, is an isotope of hydrogen. Which statements are correct?
1 Diatomic molecules have exact values for their bond energies, which are always positive.
2 The trend in Group 7 bond energies can be explained by the variation in instantaneous dipole–induced dipole (id–id) forces.
3 A value for the enthalpy change for the reaction between deuterium and chlorine can be calculated using these data alone.
A 1 only
B 1 and 2 only
C 1 and 3 only
D 2 and 3 only
▶️Answer/Explanation
Ans: A
Questions 17
Topic – 2.2 The mole and the Avogadro constant
Two procedures are described.
1 Sulfur is burned in an excess of oxygen and then NO is added to the product mixture.
2 Sulfur is burned in an excess of oxygen and then NO₂ is added to the product mixture.
Which procedures will produce some sulfur trioxide, SO₃?
A both 1 and 2
B 1 only
C 2 only
D neither 1 nor 2
▶️Answer/Explanation
Ans: A
Questions 18
Topic – 2.1 Relative masses of atoms and molecules
Powder P is a mixture containing two of AgCl , AgBr or AgI. P is shaken with dilute aqueous ammonia. A yellow solid, Q, remains. The mixture is filtered and Q is washed and dried. The filtrate is collected and treated with aqueous nitric acid to produce a white precipitate, R, which is filtered off, washed and dried. Q and R are warmed separately with concentrated sulfuric acid, H₂SO₄. Which observations are made?
▶️Answer/Explanation
Ans: B
Questions 19
Topic – 9.1 Periodicity of physical properties of the elements in Period 3
Two Period 3 elements, X and Y, burn separately in oxygen to form solid oxides. The oxide of X is insoluble in water. The oxide of Y dissolves in water to form a solution which dissolves the oxide of X. What could X and Y be?
▶️Answer/Explanation
Ans: A
Questions 20
Topic – 3.1 Electronegativity and bonding
Which row describes the structure and bonding of SiO₂ and SiCl₄?
▶️Answer/Explanation
Ans: B
Questions 21
Topic – 2.4 Reacting masses and volumes (of solutions and gases)
A sample containing 0.010 mol of anhydrous calcium nitrate is heated strongly until it fully decomposes. All the gas produced is collected and its volume measured at room conditions. What is the volume of gas produced?
A \(120 cm^3\)
B \(600 cm^3\)
C \(720 cm^3\)
D \(840 cm^3\)
▶️Answer/Explanation
Ans: B
Questions 22
Topic – 9.1 Periodicity of physical properties of the elements in Period 3
V and Z are both elements in Period 3 of the Periodic Table. Each element forms one stable ion that does not contain another element. The atomic radius of each element and the ionic radius of the ion described above is shown.
Which statement is correct?
A Ions of V and Z have the same number of full electron shells.
B Ions of Z are positively charged.
C Z has a greater electronegativity than V.
D V has more outer electrons than Z
▶️Answer/Explanation
Ans: C
Questions 23
Topic – 10.1 Similarities and trends in the properties of the Group 2 metals, magnesium to barium, and their compounds
In Group 2 of the Periodic Table, the properties of the elements and their compounds show regular change down the group. Which property shows a decrease from magnesium to barium?
A the decomposition temperature of the carbonates
B the decomposition temperature of the nitrates
C the solubility of the hydroxides
D the solubility of the sulfates
▶️Answer/Explanation
Ans: D
Questions 24
Topic – 10.1 Similarities and trends in the properties of the Group 2 metals, magnesium to barium, and their compounds
Four properties of beryllium, Be, or a beryllium compound are listed. Which property is different from the property of magnesium or the equivalent magnesium compound?
A Be reacts with \(O_2\) when heated in air; Mg does not.
B Be reacts with aqueous H₂SO₄ to form a metal sulfate and H₂; Mg does not.
C Be(NO₃)₂ decomposes on heating to form a metal oxide, NO₂, and O₂; Mg(NO₃)₂ does not.
D BeCl₂ reacts with water to form fumes of HCl ; MgCl₂ does not.
▶️Answer/Explanation
Ans: D
Questions 25
Topic – 29.4 Isomerism: optical
Which two formulae correctly represent a pair of structural isomers?
A CH₃CH(CH₃)COOH and (CH₃)₂CHCOOH
B CH₃CH(COOH)CH₃ and (CH₃)₂CHCOOH
C CH₃CHCOOH and CH₃CH₂CH₂COOH
D CH₃CH₂CH₂COOH and (CH₃)₂CHCOOH
▶️Answer/Explanation
Ans: D
Questions 26
Topic – 2.4 Reacting masses and volumes (of solutions and gases)
Which reagents and conditions would result in the formation of butanenitrile, \(CH_3CH_2CH_2CN\)?
A 1-bromobutane heated under pressure with ammonia in ethanol
B 1-bromopropane heated with potassium cyanide in ethanol
C propanal heated with hydrogen cyanide in the presence of potassium cyanide
D propanone heated with hydrogen cyanide in the presence of potassium cyanide
▶️Answer/Explanation
Ans: B
Questions 27
Topic – 29.4 Isomerism: optical
Compound X, \(C_7H_{13}Br\), reacts with hot alcoholic NaOH to produce two compounds, Y and Z. On reaction with \(Br_2\), Y gives a product, C₇H₁₂Br₂, which exists as a mixture of four optical isomers. On reaction with Br₂, Z gives a product, C₇H₁₂Br₂, which is non-chiral. What could X be?
▶️Answer/Explanation
Ans: A
Questions 28
Topic – 2.3 Formulas
When illudin S is heated under reflux with an excess of acidified potassium dichromate(VI), compound M is formed.
What is the molecular formula of compound M?
A \(C_{15}H_{16}O_4\)
B \(C_{15}H_{16}O_5\)
C \(C_{15}H_{18}O_4\)
D \(C_{15}H_{18}O_5\)
▶️Answer/Explanation
Ans: B
Questions 29
Topic – 13.1 Formulas, functional groups and the naming of organic compounds
Cyclohexene, C₆H₁₀, is a hydrocarbon with a six-membered ring of carbon atoms. It has several structural isomers that are straight-chain alkenes. The number of double bonds in each of these molecules is P. What is the shape of the cyclohexene molecule and what is the value of P?
▶️Answer/Explanation
Ans: D
Questions 30
Topic – 14.1 Alkanes
Exhaust gases from an internal combustion engine are made less harmful by passing them through a catalytic converter. A number of reactions take place in the catalytic converter. Two such reactions are described in the table. Which row is correct?
▶️Answer/Explanation
Ans: A
Questions 31
Topic – 21.1 Organic synthesis
Which compound reacts most rapidly with aqueous silver nitrate by an \(S_N1\) mechanism?
A 1-chloromethylpropane
B 2-chloromethylpropane
C 1-iodomethylpropane
D 2-iodomethylpropane
▶️Answer/Explanation
Ans: D
Questions 32
Topic – 21.1 Organic synthesis
Tartaric acid, HOOCCH(OH)CH(OH)COOH, is found in many plants. A sample of tartaric acid reacts with an excess of LiAlH₄ to form the organic product J. What happens when NaOH(aq) is added to separate samples of tartaric acid and J?
A Both tartaric acid and J react.
B Only tartaric acid reacts.
C Only J reacts.
D Neither tartaric acid nor J react.
▶️Answer/Explanation
Ans: B
Questions 33
Topic – 21.1 Organic synthesis
Citric acid can be converted into tricarballylic acid in two stages. An intermediate, Q, is formed.
Which reagents are needed for each stage?
▶️Answer/Explanation
Ans: A
Questions 34
Topic – 21.1 Organic synthesis
Structural and stereoisomerism should be considered when answering this question. P has molecular formula \(C_5H_{10}O\). P produces an orange precipitate with 2,4-dinitrophenylhydrazine (2,4-DNPH reagent). How many isomeric structures does P have?
A 5
B 6
C 7
D 8
▶️Answer/Explanation
Ans: D
Questions 35
Topic – 2.3 Formulas
Two isomeric alcohols, W and X, have molecular formula \(C_4H_9OH\). W is oxidised to carbonyl compound Y which gives a red precipitate with Fehling’s solution. X is oxidised to carbonyl compound Z which does not give a red precipitate with Fehling’s solution. Which of W and X gives a yellow precipitate with alkaline I₂ (aq)?
A insufficient data is given to answer this question
B W only
C X only
D neither W nor X
▶️Answer/Explanation
Ans: C
Questions 36
Topic – 18.2 Esters
The ester ethyl butanoate can be hydrolysed using an excess of dilute sodium hydroxide solution. Which substance is a product of this reaction?
A CH₃CH₂CH₂CO₂Na
B CH₃CO₂Na
C CH₃CH₂ONa
D H₂O
▶️Answer/Explanation
Ans: A
Questions 37
Topic – 4.1 The gaseous state: ideal and real gases and pV = nRT
An aqueous solution contains 4.00 g of a carboxylic acid, Q. When this solution reacts with an excess of magnesium, 380 cm³ of gas is produced, measured at s.t.p. What is the relative formula mass of Q?
A 59
B 118
C 126
D 236
▶️Answer/Explanation
Ans: B
Questions 38
Topic – 22.1 Infrared spectroscopy
The infrared spectrum of an organic compound is shown.
Which compound could give this spectrum?
A \(CH_3CH_2CO_2H\)
B \(CH_3CH(OH)CH_3\)
C \(CH_3COCH_3\)
D \(CH_3COCH_2OH\)
▶️Answer/Explanation
Ans: C
Questions 39
Topic – 21.1 Organic synthesis
Cyclohexa-1,4-diene is treated with a solution of bromine in tetrachloromethane in the dark.
Which product is formed? 
▶️Answer/Explanation
Ans: B
Questions 40
Topic – 21.1 Organic synthesis
2-methylbut-2-ene is reacted with hot, concentrated, acidified potassium manganate(VII) solution. What are the products of this reaction?
A ethanal and propanone
B ethanoic acid and propanone
C ethanoic acid and propan-2-ol
D ethanol and propan-2-ol
▶️Answer/Explanation
Ans: B