AQA A-Level Chemistry Paper 1, 2017
Every question from AQA A-Level Chemistry Paper 1, 2017: 11 questions, 105 marks, each with its mark scheme and topic.
- Question 1 8 marks
Calculate the enthalpy of lattice formation of silver iodide from given enthalpy-change data and answer related definition, explanation and a test for iodide ions.
Physical Chemistry · Inorganic Chemistry · 3.1.4 Energetics · 3.1.8 Thermodynamics · 3.2.6 Reactions of Ions in Aqueous Solution
- Question 2 9 marks
Calculate the concentration of ethanoic acid in a buffer from Ka and pH, and calculate the pH of a different buffer after a given amount of NaOH is added.
Physical Chemistry · 3.1.12 Acids and Bases
- Question 3 9 marks
Use Kw at 10°C to choose the correct expression for Kw, calculate the pH of pure water and of a 0.0131 mol dm^-3 Ca(OH)2 solution at 10°C, explain why pure water at 10°C is not alkaline, and predict/justify whether a saturated Mg(OH)2 solution (from 0.0131 mol added) has a larger, smaller or same pH as the Ca(OH)2 solution.
Physical Chemistry · 3.1.12 Acids and Bases · 3.1.2 Amount of Substance
- Question 4 8 marks
Calculate the relative atomic mass of titanium from isotope abundances, give the electron-impact ionisation equation and the m/z value of the ion that reaches the detector first, calculate the mass of one 49Ti atom, and calculate the time of flight of the 47Ti+ ion in a TOF mass spectrometer.
Physical Chemistry · Organic Chemistry · 3.1.1 Atomic Structure · 3.1.2 Amount of Substance · 3.3.6 Organic Analysis
- Question 5 6 marks
Calculate the Gibbs free-energy change for the given reaction at 989°C using the provided ΔH° and entropy data and state whether the reaction is feasible.
Physical Chemistry · 3.1.4 Energetics · 3.1.8 Thermodynamics
- Question 6 13 marks
Questions about Period 3 elements and their oxides: write equations for P4 + O2, SO3 + KOH and MgO + H3PO4; describe a test to distinguish sodium oxide and the phosphorus oxide product; state crystal structures of SiO2 and SO3; explain why SiO2 has a higher melting point than SO3; draw the undissociated acid from SO2 + H2O.
Physical Chemistry · Inorganic Chemistry · 3.1.3 Bonding · 3.1.12 Acids and Bases · 3.2.1 Periodicity · 3.2.4 Properties of Period 3 Elements and Their Oxides
- Question 7 9 marks
Multi-part question on the coordination chemistry of [Cu(H2O)6]Cl2: O–H bonding, why Cl− are not ligands, reaction with excess NH3 (ionic equation and colour), identity of blue-green carbonate precipitate, reagent and equation giving yellow-green solution ([CuCl4]2−), and why [CuCl2]− solutions cannot be analysed by colorimetry referring to electron configuration.
Inorganic Chemistry · Physical Chemistry · 3.2.5 Transition Metals · 3.2.6 Reactions of Ions in Aqueous Solution · 3.1.3 Bonding · 3.1.1 Atomic Structure
- Question 8 6 marks
Describe simple test-tube tests to distinguish aqueous KNO3 from K2SO4 and aqueous MgCl2 from AlCl3.
Inorganic Chemistry · Required Practicals · 3.2.6 Reactions of Ions in Aqueous Solution · Required Practical 4: Carry out simple test-tube reactions to identify Cations and Anions
- Question 9 14 marks
Use graphs to deduce optimum temperature and pressure for the industrial methane + steam equilibrium, then calculate equilibrium amounts of CO and H2 given formation of methanol and determine Kp (with units) for CO + 2H2 ⇌ CH3OH at 600 K.
Physical Chemistry · 3.1.6 Chemical Equilibria, Le Chatelier's Principle and Kc · 3.1.10 Equilibrium Constant Kp · 3.1.2 Amount of Substance · 3.1.5 Kinetics
- Question 10 9 marks
Use the standard electrode potentials table to deduce oxidation states of N in NO3- and NO, state the weakest reducing agent in the table, write the conventional cell representation for a cell with EMF +0.43 V, and identify an acid that will oxidise copper, give a balanced equation and calculate the EMF for that reaction.
Physical Chemistry · Inorganic Chemistry · 3.1.11 Electrode Potentials · 3.1.7 Oxidation, Reduction and Redox Equations · 3.1.12 Acids and Bases
- Question 11 14 marks
Calculate the percentage by mass of sodium ethanedioate in the white solid from two titrations, and answer related short questions on the ligand substitution reaction with Fe(III), the structure and isomerism of the iron–ethanedioate complex, and why ethanedioate in foods is not poisonous.
Physical Chemistry · Inorganic Chemistry · 3.1.2 Amount of Substance · 3.1.4 Energetics · 3.1.7 Oxidation, Reduction and Redox Equations · 3.2.5 Transition Metals · 3.2.6 Reactions of Ions in Aqueous Solution · 3.3.1 Introduction to Organic Chemistry