Download AQA A-level CHEMISTRY Paper 1 QUESTION PAPER 2024: Inorganic and Physical Chemistry and more Exams Chemistry in PDF only on Docsity!
*Jun24 7405101 *
IB/M/Jun24/G4006/E9 7405/
For Examiner’s Use
Question Mark 1 2 3 4 5 6 7 8 9
TOTAL
Monday 10 June 2024 Morning Time allowed: 2 hours
Materials
For this paper you must have:
- the Periodic Table/Data Booklet, provided as an insert (enclosed)
- a ruler with millimetre measurements
- a scientific calculator, which you are expected to use where appropriate.
Instructions
- Use black ink or black ball-point pen.
- Fill in the boxes at the top of this page.
- Answer all questions.
- You must answer the questions in the spaces provided. Do not write outside the box around each page or on blank pages.
- If you need extra space for your answer(s), use the lined pages at the end of this book. Write the question number against your answer(s).
- All working must be shown.
- Do all rough work in this book. Cross through any work you do not want to be marked.
Information
- The marks for questions are shown in brackets.
- The maximum mark for this paper is 105.
Please write clearly in block capitals.
Centre number Candidate number
Surname
Forename(s)
Candidate signature I declare this is my own work.
A-level
CHEMISTRY
Paper 1 Inorganic and Physical Chemistry
Do not write outside the Answer all questions in the spaces provided.^ box
(^0 1) This question is about atomic structure.
(^0 1). 1 In 1897 JJ Thomson discovered the electron. He suggested that atoms were positively charged spheres with electrons embedded within them.
Figure 1 represents an atom using Thomson’s model.
Figure 1
Suggest the identity of this atom.
Give two differences between the modern model of an atom and the Thomson model of an atom. [ 3 marks]
Identity
Difference 1
Difference 2
Do not write outside the 0 1. (^4) In the TOF mass spectrometer an ion of an isotope of tellurium, with mass number y ,^ box travels along a 1.25 m flight tube with a kinetic energy of 1.88 x 10 –12^ J
The ion takes 3.00 x 10–7^ s to reach the detector.
KE =
1 2 mv
2
KE = kinetic energy / J m = mass / kg v = speed / m s–
Calculate the mass, in g, of 1 mole of these tellurium ions.
Use your answer to suggest the mass number y of the tellurium isotope.
The Avogadro constant, L = 6.022 × 10^23 mol– [ 5 marks]
Mass g
Mass number y
Turn over ►
Do not write outside the 0 1. (^5) Tellurium has several other isotopes.^ box Two of these isotopes are 126 Te and 124 Te A different sample of tellurium is analysed using a TOF mass spectrometer.
Which statement about kinetic energy ( KE ) is correct? [1 mark] Tick () one box.
The KE of 126 Te+^ is greater than the KE of 124 Te+
The KE of 126 Te+^ is the same as the KE of 124 Te+
The KE of 126 Te+^ is less than the KE of 124 Te+
Turn over for the next question
Turn over ►
Do not write outside the (^0 2) This question is about an experiment to determine the solubility of strontium hydroxide^ box in water at 20 °C
Strontium hydroxide is slightly soluble in water. Strontium hydroxide solution reacts in a similar way to calcium hydroxide solution.
- Some solid strontium hydroxide is added to approximately 1 dm 3 of distilled water in a stoppered flask.
- The mixture is kept at 20 °C. Every day, the mixture is checked. If no solid is present in the flask, more solid strontium hydroxide is added.
- On the day when no more solid needs to be added, the flask is opened and the mixture is filtered into another flask and stoppered.
- A 25.0 cm 3 sample of the filtrate is transferred to a conical flask with a pipette and a few drops of indicator added.
- This sample is titrated with 0.100 mol dm –3^ hydrochloric acid.
- The titration is repeated several times with further samples of the filtrate. The results are shown in Table 1 on page 8.
(^0 2). 1 Suggest why the solution is kept until no more solid needs to be added. [1 mark]
0 2. (^2) Suggest why it is important to remove the undissolved strontium hydroxide before the titration. [1 mark]
(^0 2). 3 After the filtration, the solution is stored in a stoppered flask.
Suggest a reason for stoppering the flask. [1 mark]
Question 2 continues on the next page
Do not write outside the 0 2. (^4) The diagrams in Figure 2 show the part of a pipette with the graduation line.^ box
Which diagram identifies the pipette that is correctly filled? [1 mark] Tick () one box.
Figure 2
A B C
0 2. (^5) Solubility can be quoted as ‘g of solute per 100 cm 3 of solution’.
Table 1 shows the results of the titrations between strontium hydroxide and hydrochloric acid. These can be used to determine the solubility of strontium hydroxide.
Table 1
Titration Rough 1 2 3
Final burette reading / cm 3 34.40 38.00 41.05 37.
Initial burette reading / cm 3 0.00 5.55 8.05 4.
Titre / cm 3 34.40 32.45 33.00 32.
Give the equation for the reaction between strontium hydroxide and hydrochloric acid.
Use the results in Table 1 to calculate the mean titre.
Use the mean titre to calculate the solubility of strontium hydroxide, in g per 100 cm 3 of solution, at 20 °C [ 6 marks]
Do not write outside the There are no questions printed on this page^ box
DO NOT WRITE ON THIS PAGE
ANSWER IN THE SPACES PROVIDED
Turn over ►
Do not write outside the (^0 3) This question is about aqueous ions of the metal iron.^ box
When an aqueous [Fe(H 2 O) 6 ] 3+^ ion reacts with ethanedioate ions, an iron(III) complex ion X is formed.
The only ligands in X are ethanedioate ions.
0 3. (^1) Draw the structure of X.
Include the charge. [2 marks]
0 3. (^2) The formation of X is an example of the chelate effect.
Explain the meaning of the chelate effect. [ 2 marks]
Question 3 continues on the next page
Turn over ►
Do not write outside the box
Do not write outside the 0 3. (^4) A student adds dilute ammonia solution to a solution containing [Fe(H 2 O) 6 ]2+^ ions.^ box
Give the formula of the precipitate that forms. [1 mark]
0 3. 5 The student adds sodium carbonate solution to a solution containing [Fe(H 2 O) 6 ] 2+^ ions.
State one observation the student would make.
Give an equation for the reaction. [2 marks]
Observation
Equation
(^0 3). 6 A solution containing [Fe(H 2 O) 6 ] 2+^ ions changes to a yellow-brown colour after several hours in contact with air.
The student adds sodium carbonate to the yellow-brown solution.
Give an equation for the reaction with sodium carbonate. [1 mark]
Do not write outside the 0 4. 3 The temperature of the equilibrium mixture formed in Question 04.1 is increased.^ box
How does the amount of H 2 (g) change when the new position of equilibrium is reached? [1 mark] Tick () one box.
The amount decreases.
The amount does not change.
The amount increases.
Ethanol can be made from ethene and steam.
C 2 H 4 (g) + H 2 O(g) ⇌ CH 3 CH 2 OH(g) Δ H = – 45 kJ mol–
Table 2 shows the mole fractions of each of the gases in an equilibrium mixture at 6000 kPa
Table 2
Gas Mole fraction
Ethene 0.
Steam 0.
Ethanol 0.
Turn over ►
Do not write outside the 0 4. (^4) Give an expression for K p for this reaction.^ box
Calculate the value of K p at 6000 kPa
State the units. [ 4 marks]
K p
Units
(^0 4). 5 State the effect, if any, of an increase in volume of the container on the value of K p for this reaction at a constant temperature. [1 mark]
Turn over for the next question
Turn over ►
Do not write outside the 0 5. (^4) Give the equation for the reaction of solid sodium chloride with^ box concentrated sulfuric acid.
State the role of the chloride ions in this reaction. [ 2 marks]
Equation
Role
(^0 5). (^5) Draw the shape of the Cl 3 –^ ion. Include any lone pairs of electrons that influence the shape. [ 1 mark]
0 5. 6 Chlorine forms an ion with the Group 3 element thallium (Tl).
State and explain the bond angle in TlCl 2 + [2 marks]
Bond angle
Explanation
Do not write outside the (^0 6) This question is about vanadium ions.^ box
Table 3 shows some standard electrode potential values.
Table 3
E o^ / V
O 2 (g) + 4 H+^ (aq) + 4 e−^ → 2 H 2 O(l) +1.
VO 2 +^ (aq) + 2 H+^ (aq) + e−^ → VO 2+^ (aq) + H 2 O(l) +1.
VO 2+^ (aq) + 2 H+^ (aq) + e−^ → V3+^ (aq) + H 2 O(l) +0.
V3+^ (aq) + e−^ → V2+^ (aq) –0.
Fe2+^ (aq) + 2 e−^ → Fe(s) –0.
Zn2+^ (aq) + 2 e−^ → Zn(s) –0.
V2+^ (aq) + 2 e−^ → V(s) –1.
Mg 2+^ (aq) + 2 e−^ → Mg(s) –2.
(^0 6). 1 Use the data in Table 3 to explain why Zn reduces an aqueous solution of VO 2 +^ ions to V2+^ ions, but does not reduce it any further. [ 2 marks]
(^0 6). 2 Identify the species in Table 3 that can reduce an aqueous solution of VO 2 +^ to V [ 1 mark]
