OCR A-Level Chemistry Periodic table, elements and physical chemistry (01), June 2022
Every question from OCR A-Level Chemistry Periodic table, elements and physical chemistry (01), June 2022 (H432): 22 questions, 100 marks, each with its mark scheme and topic.
- Question 1 1 mark
Identify the remaining silver halide precipitates after adding silver nitrate followed by excess dilute ammonia to a mixture of chloride, bromide, and iodide ions.
Module 3: Periodic table and energy · Practical Activity Groups · 3.1 The periodic table · PAG 4: Qualitative analysis of ions
- Question 2 1 mark
Identify the correct equation for the reaction of 20 cm3 of nitrogen gas with 10 cm3 of oxygen gas to form 20 cm3 of a gaseous product.
Module 2: Foundations in chemistry · 2.1 Atoms and reactions
- Question 3 1 mark
Identify element X given the mass of element X and the mass of its oxide X2O3 formed by reaction with oxygen
Module 2: Foundations in chemistry · 2.1 Atoms and reactions
- Question 4 1 mark
Calculate the concentration of hydrogen peroxide in a disinfectant using titration data and a balanced redox equation, choosing from multiple-choice options A to D.
Module 2: Foundations in chemistry · Practical Activity Groups · 2.1 Atoms and reactions · PAG 2: Acid-base titration
- Question 5 1 mark
Determine the formula of a substance given the mass of 4 molecules.
Module 2: Foundations in chemistry · 2.1 Atoms and reactions
- Question 6 1 mark
Determine the number of Fe2+ and Fe3+ ions in one formula unit of Prussian blue, C18Fe7N18.
Module 2: Foundations in chemistry · 2.1 Atoms and reactions
- Question 7 1 mark
Calculate the enthalpy change for the combustion of methane using the provided bond enthalpies.
Module 3: Periodic table and energy · 3.2 Physical chemistry
- Question 8 1 mark
Calculate the rate constant for a first-order reaction given its half-life is 80 seconds.
Module 5: Physical chemistry and transition elements · 5.1 Rates, equilibrium and pH
- Question 9 1 mark
Identify the equation that represents the standard enthalpy change of atomisation of bromine.
Module 3: Periodic table and energy · Module 5: Physical chemistry and transition elements · 3.2 Physical chemistry · 5.2 Energy
- Question 10 1 mark
Determine the signs of enthalpy change (ΔH) and entropy change (ΔS) for the condensation of ammonia gas.
Module 5: Physical chemistry and transition elements · 5.2 Energy
- Question 11 1 mark
Deduce the colour change when aqueous sodium hydroxide is added to an indicator solution that is already yellow, given the equilibrium HA(aq) <=> A-(aq) + H+(aq) where HA is blue and A- is yellow
Module 5: Physical chemistry and transition elements · 5.1 Rates, equilibrium and pH
- Question 12 1 mark
Identify the Brønsted-Lowry acids in the equilibrium mixture of ammonia and water.
Module 5: Physical chemistry and transition elements · 5.1 Rates, equilibrium and pH
- Question 13 1 mark
Determine the standard electrode potential for the redox system Cr2+(aq) + 2e– = Cr(s) using given standard electrode potentials for chromium species.
Module 5: Physical chemistry and transition elements · 5.2 Energy
- Question 14 1 mark
Identify which given chemical reactions form a product with non-polar molecules from a multiple-choice list.
Module 2: Foundations in chemistry · 2.2 Electrons, bonding and structure
- Question 15 1 mark
Identify which of the given transition metal ions contain one or more unpaired electrons.
Module 5: Physical chemistry and transition elements · 5.3 Transition elements
- Question 16 10 marks
Explain the effect of temperature on the rate of reaction using a Boltzmann distribution, determine the orders, rate equation, rate constant and units from experimental data, and suggest a two-step mechanism for a reaction.
Module 5: Physical chemistry and transition elements · 5.1 Rates, equilibrium and pH
- Question 17 14 marks
Calculate maximum temperature change, standard enthalpy of formation, standard entropy change, enthalpy change, and feasibility of reactions involving energy changes, enthalpy, and entropy.
Module 3: Periodic table and energy · Module 5: Physical chemistry and transition elements · 3.2 Physical chemistry · 5.2 Energy
- Question 18 9 marks
Complete the first ionisation energy graph for elements He to Ne, estimate the energy required to form one Li+ ion from one Li atom in standard form to two significant figures, and explain trends in first ionisation energies across periods based on nuclear charge, shielding, and sub-shells.
Module 2: Foundations in chemistry · Module 3: Periodic table and energy · 3.1 The periodic table · 2.1 Atoms and reactions · 2.2 Electrons, bonding and structure
- Question 19 14 marks
Calculate the mass of succinic acid in a health supplement tablet using titration data, and calculate the pH and explain the action of a glycolic acid-potassium hydroxide buffer solution.
Module 2: Foundations in chemistry · Module 5: Physical chemistry and transition elements · Practical Activity Groups · PAG 2: Acid-base titration · 5.1 Rates, equilibrium and pH · 2.1 Atoms and reactions
- Question 20 8 marks
Calculate the equilibrium constant Kc for the Haber process and explain the compromise conditions, and determine the effect of temperature and pressure on iron oxide reduction equilibria
Module 5: Physical chemistry and transition elements · 5.1 Rates, equilibrium and pH
- Question 21 14 marks
Analyze Group 2 reactions and compounds involving magnesium, barium oxide, and calcium minerals through observations, half-equations, calculations of mass, ionic equations, and reaction equations.
Module 3: Periodic table and energy · Module 2: Foundations in chemistry · Module 5: Physical chemistry and transition elements · 3.1 The periodic table · 2.1 Atoms and reactions · 5.1 Rates, equilibrium and pH
- Question 22 16 marks
Determine the formulae, structures, ionic equations, and explanations related to transition metal complexes of iron and copper, including isomerism, redox potentials, and stoichiometry.
Module 5: Physical chemistry and transition elements · Module 3: Periodic table and energy · 5.3 Transition elements · 3.1 The periodic table