9701_s18_qp_13 - revisedeck

9701_s18_qp_13

A paper of Chemistry, 9701

Questions:

40

Year:

2018

Paper:

1

Variant:

3

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1

Why is the boiling point of ammonia, NH3, higher than the boiling point of phosphine, PH3?

3. Chemical bonding → 3.6. Intermolecular forces, electronegativity and bond properties

11. Group 17 → 11.2. The chemical properties of the halogen elements and the hydrogen halides

3. Chemical bonding → 3.4. Covalent bonding and coordinate (dative covalent) bonding

Open

2

Neutrons are passed through an electric field. The mass of one neutron relative to 12 1 the mass of a 12C atom and any deflection in the electric field is recorded. Which row is correct?

1. Atomic structure → 1.1. Particles in the atom and atomic radius

Open

3

The table refers to the electron distribution in the second shell of an atom with eight protons. Which row is correct for this atom?

1. Atomic structure → 1.3. Electrons, energy levels and atomic orbitals

Open

4

Which statement describes the bond between carbon and hydrogen in an ethene molecule?

3. Chemical bonding → 3.4. Covalent bonding and coordinate (dative covalent) bonding

Open

5

Aspirin, C9H8O4, Mr = 180.0, can be made by a reaction between 2-hydroxybenzoic acid, C7H6O3, Mr = 138.0, and ethanoic anhydride, C4H6O3, Mr = 102.0. The balanced equation for the reaction is shown...

2. Atoms, molecules and stoichiometry → 2.4. Reacting masses and volumes (of solutions and gases)

18. Carboxylic acids and derivatives → 18.2. Esters

17. Carbonyl compounds → 17.1. Aldehydes and ketones

Open

6

Which diagram correctly describes the behaviour of a fixed mass of an ideal gas?

4. States of matter → 4.1. The gaseous state: ideal and real gases and \( pV = nRT \)

Open

7

Anhydrous copper(chloride, CuCl 2, combines with water to form CuCl 2.2H2O. The standard enthalpy changes of formation for this reaction are shown...

5. Chemical energetics → 5.1. Enthalpy change, \(\Delta H\)

Open

8

Xenon hexafluoride, XeF6, reacts with water. XeF6 + 3H2O → XeO3 + 6HF Which statement is correct?

11. Group 17 → 11.2. The chemical properties of the halogen elements and the hydrogen halides

11. Group 17 → 11.3. Some reactions of the halide ions

Open

9

Hydrogen is produced industrially from methane as shown...

14. Hydrocarbons → 14.1. Alkanes

3. Chemical bonding → 3.6. Intermolecular forces, electronegativity and bond properties

11. Group 17 → 11.2. The chemical properties of the halogen elements and the hydrogen halides

Open

10

The chemical equilibrium shown...

7. Equilibria → 7.1. Chemical equilibria: reversible reactions, dynamic equilibrium

Open

11

The enzyme maltase speeds up the reaction between maltose and water. maltase maltose + water glucose Maltase shows specificity. Which statement describes the specificity of maltase?

Open

12

Which description of the bonding and acid / base nature of aluminium oxide is correct?

4. States of matter → 4.2. Bonding and structure

9. The Periodic Table: chemical periodicity → 9.2. Periodicity of chemical properties of the elements in Period 3

3. Chemical bonding → 3.2. Ionic bonding

Open

13

X and Y are elements of the third period. X and Y are individually heated in excess chlorine. Each product is purified and then separately added to water, producing two solutions. Both solutions have a pH of less than 5. What could be X and Y?

9. The Periodic Table: chemical periodicity → 9.2. Periodicity of chemical properties of the elements in Period 3

Open

14

An ore contains magnesium carbonate and barium carbonate. A sample of the ore is dissolved in nitric acid. How could this solution be processed into a magnesium compound and a separate barium compound?

10. Group 2 → 10.1. Similarities and trends in the properties of the Group 2 metals, magnesium to barium, and their compounds

Open

15

When calcium and calcium hydride, CaH2, react separately with water, they each produce a white solid and a colourless gas. The white solid is the same compound in each reaction. Which statement is correct?

11. Group 17 → 11.2. The chemical properties of the halogen elements and the hydrogen halides

11. Group 17 → 11.4. The reactions of chlorine

Open

16

When concentrated sulfuric acid is added to solid sodium chloride, HCl is formed but not Cl 2. When concentrated sulfuric acid is added to solid sodium iodide, I2 is formed. Which statement explains these observations?

11. Group 17 → 11.3. Some reactions of the halide ions

11. Group 17 → 11.4. The reactions of chlorine

Open

17

Silver chloride and silver iodide form equilibria when added to water. AgClAg++ Cl –Kc = K1 AgIAg++ I–Kc = K2 Each equilibrium position lies well to the left. Silver iodide will not dissolve in aqueous ammonia. Silver chloride will dissolve in aqueous ammonia. Another equilibrium is formed. Ag++ 2NH3Ag(NH3)2 +Kc = K3 The position of this equilibrium lies to the right. What is the order of magnitude for these three equilibrium constants?

7. Equilibria → 7.1. Chemical equilibria: reversible reactions, dynamic equilibrium

11. Group 17 → 11.3. Some reactions of the halide ions

Open

18

Elements and their compounds are important as catalysts. In which process is a compound used, rather than an element?

14. Hydrocarbons → 14.2. Alkenes

14. Hydrocarbons → 14.1. Alkanes

Open

19

The gaseous products of heating a mixture of Ca(OH)2 and NH4Cl are passed through solid CaO. This absorbs water vapour and a gas, W, is collected. A sample of W is oxidised by Cl 2to produce two gases, X and Y. X is an element. Y is acidic. Y reacts with W to produce Z. What are X and Z?

11. Group 17 → 11.4. The reactions of chlorine

2. Atoms, molecules and stoichiometry → 2.4. Reacting masses and volumes (of solutions and gases)

Open

20

Molecule G is shown...

13. An introduction to AS Level organic chemistry → 13.4. Isomerism: structural isomerism and stereoisomerism

1. Atomic structure → 1.3. Electrons, energy levels and atomic orbitals

Open

21

Sibirene, C15H24, is reacted with an excess of HBr. The major product is X. X excess HBrsibirene What is the skeletal formula of X?

13. An introduction to AS Level organic chemistry → 13.1. Formulas, functional groups and the naming of organic compounds

14. Hydrocarbons → 14.2. Alkenes

Open

22

Which statement is not correct?

2. Atoms, molecules and stoichiometry → 2.3. Formulas

4. States of matter → 4.1. The gaseous state: ideal and real gases and \( pV = nRT \)

Open

23

The presence of a halogen in an organic compound may be detected by warming the organic compound with aqueous silver nitrate. Which compound would be the quickest to produce a precipitate?

15. Halogen compounds → 15.1. Halogenoalkanes

11. Group 17 → 11.2. The chemical properties of the halogen elements and the hydrogen halides

Open

24

Halogenoalkanes react with NaOHeither by an SN1 mechanism or by an SN2 mechanism. The mechanism followed by the reaction depends on the structure of the halogenoalkane. This question is about the reaction of 3-bromo-3-ethylpentane, (C2H5)3CBr. Which statement is correct?

15. Halogen compounds → 15.1. Halogenoalkanes

Open

25

Which compound is a secondary alcohol that can be dehydrated to form an alkene with Mr = 70?

16. Hydroxy compounds → 16.1. Alcohols

14. Hydrocarbons → 14.2. Alkenes

Open

26

When 0.0075 mol of alcohol X are completely burnt in excess oxygen and the gases produced are passed through an excess of limewater (calcium hydroxide solution), 3.0 g of calcium carbonate are produced. When X is warmed with acidified potassium dichromate(there is a colour change from orange to green. What could be the identity of X?

16. Hydroxy compounds → 16.1. Alcohols

2. Atoms, molecules and stoichiometry → 2.4. Reacting masses and volumes (of solutions and gases)

Open

27

Considering only structural isomers, what is the number of alcohols of each type with the formula C5H12O?

16. Hydroxy compounds → 16.1. Alcohols

13. An introduction to AS Level organic chemistry → 13.4. Isomerism: structural isomerism and stereoisomerism

Open

28

A student carried out a two-stage synthesis in which CH3CH2CH2Br was converted into CH3CH2CH2CO2H. Which compound could have been formed by the first stage of this synthesis?

21. Organic synthesis → 21.1. Organic synthesis

Open

29

An ester X has the structural formula CH3CO2CH(CH3)CH2CH3. X can be prepared by heating an alcohol Y, under reflux, with ethanoic acid and an acid catalyst. What is the correct name for Y?

18. Carboxylic acids and derivatives → 18.2. Esters

16. Hydroxy compounds → 16.1. Alcohols

Open

30

Compound S can be extracted from natural compounds. Reacting S with hot, concentrated KMnO4 produces the organic product, T. Some of the absorptions found in the infra-red spectra of S and T are described. S has no strong absorption between 1670 and 1740 cm–1. T has a strong absorption at 1720 cm–1 but has no strong, broad absorption between 2500 and 3000 cm–1. From this information, what could be the formulae of S and T?

13. An introduction to AS Level organic chemistry → 13.1. Formulas, functional groups and the naming of organic compounds

15. Halogen compounds → 15.1. Halogenoalkanes

Open

31

Complete combustion of a sample of a hydrocarbon gave 0.132 g of carbon dioxide and 0.054 g of water. Which formulae could correctly represent this hydrocarbon?

13. An introduction to AS Level organic chemistry → 13.1. Formulas, functional groups and the naming of organic compounds

2. Atoms, molecules and stoichiometry → 2.4. Reacting masses and volumes (of solutions and gases)

14. Hydrocarbons → 14.1. Alkanes

Open

32

Which statements are correct?

10. Group 2 → 10.1. Similarities and trends in the properties of the Group 2 metals, magnesium to barium, and their compounds

3. Chemical bonding → 3.2. Ionic bonding

Open

33

Ammonia and chlorine react as shown...

11. Group 17 → 11.4. The reactions of chlorine

12. Nitrogen and sulfur → 12.1. Nitrogen and sulfur

11. Group 17 → 11.2. The chemical properties of the halogen elements and the hydrogen halides

Open

34

The diagram shows the reaction pathway for a reversible reaction. extent of reaction energy / kJ mol–1 Which statements are correct?

5. Chemical energetics → 5.1. Enthalpy change, \(\Delta H\)

Open

35

The structure of metals is considered to be positive ions surrounded by delocalised electrons. The melting points of the metals in Period 3 increase with increasing atomic number. Which statements help to explain this trend from sodium to aluminium?

9. The Periodic Table: chemical periodicity → 9.1. Periodicity of physical properties of the elements in Period 3

10. Group 2 → 10.1. Similarities and trends in the properties of the Group 2 metals, magnesium to barium, and their compounds

Open

36

Under room conditions, 600 cm3 of a gas, X, has a mass of 0.700 g. What could X be?

4. States of matter → 4.1. The gaseous state: ideal and real gases and \( pV = nRT \)

2. Atoms, molecules and stoichiometry → 2.4. Reacting masses and volumes (of solutions and gases)

Open

37

Which compounds, on reaction with NaBH4, form a compound with a chiral carbon atom?

15. Halogen compounds → 15.1. Halogenoalkanes

13. An introduction to AS Level organic chemistry → 13.1. Formulas, functional groups and the naming of organic compounds

Open

38

Compound Y is a straight chain molecule with formula CnH2n+1X. X is a halogen. The Mr of Y is 137. The halogen atom is on the second carbon atom in the chain. Which statements are correct?

13. An introduction to AS Level organic chemistry → 13.4. Isomerism: structural isomerism and stereoisomerism

11. Group 17 → 11.1. Physical properties of the Group 17 elements

Open

39

Propanone and hydrogen cyanide react together by the mechanism shown...

17. Carbonyl compounds → 17.1. Aldehydes and ketones

14. Hydrocarbons → 14.2. Alkenes

Open

40

Acrolein is an organic compound with the molecular formula C3H4O. It is used in water treatment and as a herbicide. When acrolein reacts with 2,4-dinitrophenylhydrazine an orange precipitate is obtained. Reaction of acrolein with Tollens’ reagent produces a silver mirror. Which statements are correct?

15. Halogen compounds → 15.1. Halogenoalkanes

11. Group 17 → 11.3. Some reactions of the halide ions

Open