9701_s21_qp_11 - revisedeck

9701_s21_qp_11

A paper of Chemistry, 9701

Questions:

40

Year:

2021

Paper:

1

Variant:

1

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1

Which contains the largest number of hydrogen atoms?

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

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

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2

In which pair of species do both species have only one unpaired p electron?

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

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3

Phosphorus forms two chlorides. Phosphorus(chloride, PCl 3, is a covalent liquid. Phosphorus(chloride is an ionic solid. One of the ions present is [PCl 4]+. What is the shape of the PCl 3 molecule and the [PCl 4]+ ion?

13. An introduction to AS Level organic chemistry → 13.3. Shapes of organic molecules; σ and π bonds

3. Chemical bonding → 3.5. Shapes of molecules

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4

is the standard enthalpy of formation of methane. is the standard enthalpy of combustion of carbon. is the standard enthalpy of combustion of hydrogen. CH4+ 2O2CO2+ 2H2OWhich expression is equivalent to ?

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

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5

The diagram shows the Boltzmann distribution for the same gas at two different temperatures, T1 and T2. y x T1 T2 What is plotted on the y-axis and which line represents the higher temperature?

8. Reaction kinetics → 8.2. Effect of temperature on reaction rates and the concept of activation energy

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

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6

What is the minimum mass of oxygen required to ensure the complete combustion of 12 dm3 of propane measured under room conditions?

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

14. Hydrocarbons → 14.1. Alkanes

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

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7

Why is the first ionisation energy of oxygen less than that of nitrogen?

1. Atomic structure → 1.4. Ionisation energy

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8

Which gas would behave most like an ideal gas under room conditions?

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

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9

When hydrogen iodide is reacted with concentrated sulfuric acid, several reactions occur, including: 8HI + H2SO4  H2S + 4H2O + 4I2 Which row gives the change in oxidation number of iodine and of sulfur in this reaction?

6. Electrochemistry → 6.1. Redox processes: electron transfer and changes in oxidation number (oxidation state)

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10

The diagram represents the Haber process for the manufacture of ammonia from nitrogen and hydrogen. heat exchanger condenser catalytic converter N2 + H2 NH3 What is the purpose of the heat exchanger?

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

17. Carbonyl compounds → 17.1. Aldehydes and ketones

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

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11

Which statement about catalysts is correct?

8. Reaction kinetics → 8.3. Homogeneous and heterogeneous catalysts

8. Reaction kinetics → 8.2. Effect of temperature on reaction rates and the concept of activation energy

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

Open

12

Element X is in Period 3. Element X forms a solid oxide Y. Y reacts with hot concentrated hydrochloric acid. Y reacts with hot aqueous sodium hydroxide to form a compound in which X is part of an anion. How many p electrons does one atom of X have in its outer shell?

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

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

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13

The gaseous products of heating a mixture of Ca(OH)2 and NH4Cl are passed through solid CaO. A single gaseous product, W, is collected. A sample of W reacts with 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?

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

11. Group 17 → 11.4. The reactions of chlorine

18. Carboxylic acids and derivatives → 18.1. Carboxylic acids

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14

Q is a mixture of a Group 2 oxide and a Group 2 sulfate. Q contains equal amounts of the two compounds. Q is shaken with water and the resulting mixture filtered; a solid residue is obtained. There is no reaction when the solid residue is shaken with HCl . Shaking the filtrate with H2SO4produces a white precipitate. What could be Q?

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

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

11. Group 17 → 11.4. The reactions of chlorine

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15

Which substance will not be a product of the thermal decomposition of hydrated magnesium nitrate?

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

12. Nitrogen and sulfur → 12.1. Nitrogen and sulfur

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16

A 5 cm3 sample of 0.05 mol dm–3 sodium chloride is mixed with a 5 cm3 sample of 0.05 mol dm–3 potassium iodide. 10 cm3 of acidified 0.05 mol dm–3 silver nitrate is then added, followed by concentrated ammonia solution. What is seen after the addition of an excess of concentrated ammonia solution?

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

12. Nitrogen and sulfur → 12.1. Nitrogen and sulfur

16. Hydroxy compounds → 16.1. Alcohols

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17

The volatility of the Group 17 elements, chlorine, bromine and iodine, decreases down the group. What is responsible for this trend?

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

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

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18

Acid rain is a dilute solution of sulfuric acid. Which pollutant also contributes to the formation of acid rain?

12. Nitrogen and sulfur → 12.1. Nitrogen and sulfur

7. Equilibria → 7.2. Brønsted–Lowry theory of acids and bases

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19

R is an oxide of Period 3 element T. 5.00 g of R contains 2.50 g of T. What is T?

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

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20

Bromoethane reacts with cyanide ions, producing propanenitrile. Which statement about the SN2 mechanism of this reaction is correct?

17. Carbonyl compounds → 17.1. Aldehydes and ketones

15. Halogen compounds → 15.1. Halogenoalkanes

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21

Which compound would produce two different carboxylic acids when treated with hot, concentrated, acidified manganate(ions?

18. Carboxylic acids and derivatives → 18.1. Carboxylic acids

17. Carbonyl compounds → 17.1. Aldehydes and ketones

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22

Which compound could show both cis-trans isomerism and optical isomerism?

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

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23

Limonene is a hydrocarbon found in the rind of citrus fruits. limonene What is the molecular formula of limonene?

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

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24

The compound cetyl palmitate, C15H31CO2C16H33, is a waxy solid. Cetyl palmitate is heated under reflux with an excess of aqueous sodium hydroxide. Which products will be formed?

18. Carboxylic acids and derivatives → 18.1. Carboxylic acids

11. Group 17 → 11.4. The reactions of chlorine

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25

When an organic compound is oxidised, any oxygen atom gained by the organic molecule is considered to be from a water molecule also producing 2H+ + 2e–. Any hydrogen atom lost may be considered to be lost as H+ + e–. These changes can be represented by the following two equations. H2O  [O] + 2H+ + 2e– [H]  H+ + e– Compound X is oxidised by heating under reflux with hot, acidified potassium dichromate(for one hour. The half-equation for the reduction reaction is shown...

17. Carbonyl compounds → 17.1. Aldehydes and ketones

13. An introduction to AS Level organic chemistry → 13.2. Characteristic organic reactions

11. Group 17 → 11.4. The reactions of chlorine

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26

Compound X has the empirical formula C2H4O. Its infra-red spectrum is shown...

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

2. Atoms, molecules and stoichiometry → 2.3. Formulas

Open

27

How many moles of hydrogen, H2, are evolved when an excess of sodium metal is added to one mole of citric acid?

7. Equilibria → 7.2. Brønsted–Lowry theory of acids and bases

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

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

Open

28

Which statement is correct for the reaction of carbonyl compounds with HCN?

17. Carbonyl compounds → 17.1. Aldehydes and ketones

15. Halogen compounds → 15.1. Halogenoalkanes

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29

The table describes four reactions of propene. Which row is correct?

14. Hydrocarbons → 14.2. Alkenes

14. Hydrocarbons → 14.1. Alkanes

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30

Butanoic acid is prepared from 1-bromopropane. This synthesis requires a sequence of two reactions. Which compound is prepared in the first stage of the synthesis?

21. Organic synthesis → 21.1. Organic synthesis

15. Halogen compounds → 15.1. Halogenoalkanes

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31

Ethanol combines with ethanoic acid to form ethyl ethanoate according to the following reaction. C2H5OH(+ CH3CO2H(CH3CO2C2H5(+ H2O(∆H o = –6 kJ mol–1 9.2 g ethanol, 12 g ethanoic acid and 8.8 g ethyl ethanoate are mixed and allowed to stand at 298 K, until equilibrium is reached. (Mr: C2H5OH, 46; CH3CO2H, 60; CH3CO2C2H5, 88) The resulting equilibrium mixture is found to contain 4.8 g ethanoic acid. The experiment is repeated at 323 K. Which statements are correct?

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

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32

The diagram shows an incomplete energy profile diagram for a reaction. reactants products enthalpy progress of reaction Which reactions could this diagram refer to?

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

8. Reaction kinetics → 8.3. Homogeneous and heterogeneous catalysts

Open

33

A gaseous hydrocarbon has a density of 2.42 g dm–3 under room conditions. What could be the skeletal formula of 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 → 2.3. Formulas

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34

Which molecules contain at least one bond angle of 120?

13. An introduction to AS Level organic chemistry → 13.3. Shapes of organic molecules; σ and π bonds

3. Chemical bonding → 3.5. Shapes of molecules

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35

Which statements are correct going across Period 3 from sodium to chlorine?

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

3. Chemical bonding → 3.1. Electronegativity and bonding

1. Atomic structure → 1.4. Ionisation energy

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36

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

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37

Which statements are correct?

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

14. Hydrocarbons → 14.1. Alkanes

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

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38

Which pairs of compounds may be distinguished by testing with alkaline aqueous iodine?

17. Carbonyl compounds → 17.1. Aldehydes and ketones

16. Hydroxy compounds → 16.1. Alcohols

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39

Which reactions have a coloured organic product?

17. Carbonyl compounds → 17.1. Aldehydes and ketones

16. Hydroxy compounds → 16.1. Alcohols

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40

Propanoic acid is reacted with an excess of lithium aluminium hydride. The organic product of this reaction is reacted with ethanoic acid in the presence of concentrated sulfuric acid, forming product X. What are major commercial uses of X?

18. Carboxylic acids and derivatives → 18.1. Carboxylic acids

16. Hydroxy compounds → 16.1. Alcohols

17. Carbonyl compounds → 17.1. Aldehydes and ketones

Open