OCR A-Level Chemistry Periodic table, elements and physical chemistry (01), June 2018
Every question from OCR A-Level Chemistry Periodic table, elements and physical chemistry (01), June 2018 (H432): 21 questions, 100 marks, each with its mark scheme and topic.
- Question 1 1 mark
Calculate the percentage of 11B atoms in a boron sample given its relative atomic mass and constituent isotopes.
Module 2: Foundations in chemistry · 2.1 Atoms and reactions
- Question 2 1 mark
Determine the oxidation numbers of iodine and antimony in the ionic compound [ICl2]+[SbCl6]- given that the oxidation number of chlorine is -1.
Module 2: Foundations in chemistry · 2.1 Atoms and reactions
- Question 3 1 mark
Calculate the number of hydrogen atoms in 0.125 mol of C2H5OH
Module 2: Foundations in chemistry · 2.1 Atoms and reactions
- Question 4 1 mark
Calculate the concentration of nitric acid in mol dm⁻³ required to neutralise a given volume and concentration of barium hydroxide solution.
Module 2: Foundations in chemistry · Practical Activity Groups · PAG 2: Acid-base titration · 2.1 Atoms and reactions
- Question 5 1 mark
Identify the statement that best explains why nitrogen has a larger first ionisation energy than oxygen.
Module 2: Foundations in chemistry · Module 3: Periodic table and energy · 3.1 The periodic table · 2.2 Electrons, bonding and structure
- Question 6 1 mark
Deduce the formula of an ionic compound formed between an element in Group 2 and an element in Group 15.
Module 2: Foundations in chemistry · Module 3: Periodic table and energy · 3.1 The periodic table · 2.1 Atoms and reactions
- Question 7 1 mark
Identify which statement about ammonium carbonate is not correct from a choice of four options.
Module 3: Periodic table and energy · Practical Activity Groups · PAG 4: Qualitative analysis of ions · 3.1 The periodic table
- Question 8 1 mark
Identify the correct rate-concentration graph for a reaction that is first order with respect to reactant X.
Module 5: Physical chemistry and transition elements · 5.1 Rates, equilibrium and pH
- Question 9 1 mark
Calculate the partial pressure of SO3 given the equilibrium moles of SO2, O2, and SO3 and the total pressure.
Module 5: Physical chemistry and transition elements · 5.1 Rates, equilibrium and pH
- Question 10 1 mark
Calculate the pH of a buffer solution prepared by mixing propanoic acid and sodium propanoate solutions of given volumes and concentrations, given the acid dissociation constant Ka.
Module 5: Physical chemistry and transition elements · 5.1 Rates, equilibrium and pH
- Question 11 1 mark
Calculate the standard entropy change for the formation of methanol from carbon monoxide and hydrogen using standard entropy data.
Module 5: Physical chemistry and transition elements · 5.2 Energy
- Question 12 1 mark
Identify the overall cell reaction equation for a hydrogen-oxygen fuel cell in alkaline solution given two half-equations with their standard electrode potentials.
Module 5: Physical chemistry and transition elements · 5.2 Energy
- Question 13 1 mark
Identify which of the given enthalpy changes (bond enthalpy of C-H, second electron affinity of oxygen, and standard enthalpy change of formation of magnesium) are endothermic.
Module 3: Periodic table and energy · Module 5: Physical chemistry and transition elements · 3.2 Physical chemistry · 5.2 Energy
- Question 14 1 mark
Identify which statements explain why reaction rates increase as temperature increases using Maxwell-Boltzmann distribution concepts.
Module 3: Periodic table and energy · 3.2 Physical chemistry
- Question 15 1 mark
Identify the correct statements regarding the stereochemistry, bond angles, and isomerism of the platinum complex Pt(NH3)2Cl2.
Module 5: Physical chemistry and transition elements · 5.3 Transition elements
- Question 16 15 marks
Calculate enthalpy changes of hydration, complete an enthalpy cycle, explain hydration and bond enthalpies, and calculate a bond enthalpy using average bond values.
Module 3: Periodic table and energy · Module 5: Physical chemistry and transition elements · 3.2 Physical chemistry · 5.2 Energy
- Question 17 11 marks
Determine the rate constant, reaction mechanism, activation energy, and pre-exponential factor from experimental initial rates and an Arrhenius plot for the reaction between iron(III) and iodide ions.
Module 5: Physical chemistry and transition elements · 5.1 Rates, equilibrium and pH
- Question 18 10 marks
Write an expression for Kc, calculate the amount of NO2 at equilibrium given Kc and moles, predict enthalpy change from Kp at different temperatures, and explain the effect of pressure change on equilibrium position in terms of Kp.
Module 5: Physical chemistry and transition elements · 5.1 Rates, equilibrium and pH
- Question 19 11 marks
Calculate the pKa of ethanoic acid and percentage dissociation from pH, find the percentage purity of a sodium hydroxide drain cleaner from titration data, and draw the dot-and-cross diagram of a carbonate ion.
Module 5: Physical chemistry and transition elements · Module 2: Foundations in chemistry · Module 4: Core organic chemistry · 5.1 Rates, equilibrium and pH · 2.2 Electrons, bonding and structure · 4.2 Alcohols, haloalkanes and analysis
- Question 20 20 marks
Analyze halogen boiling points, complete an enthalpy profile diagram for hydrogen iodide decomposition, determine the molecular formula of a chlorine oxide using gas laws, and calculate the formula of a Group 1 iodate(V) using titration data.
Module 2: Foundations in chemistry · Module 3: Periodic table and energy · Module 5: Physical chemistry and transition elements · Practical Activity Groups · PAG 2: Acid-base titration · 3.1 The periodic table · 3.2 Physical chemistry · 2.1 Atoms and reactions
- Question 21 18 marks
Complete electron configurations, determine standard cell potentials and explain redox reactions, equilibria, and copper chemistry involving transition elements.
Module 2: Foundations in chemistry · Module 5: Physical chemistry and transition elements · Practical Activity Groups · 2.2 Electrons, bonding and structure · 5.2 Energy · 5.3 Transition elements · PAG 8: Electrochemical cells