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Higher Chemistry Unit 3: Chemistry in Society Homework 3∙5 1. Which of the following compounds is a raw material in the chemical industry? A B C D Ammonia Calcium carbonate Hexane Nitric acid Answer ______ 2. Which line in the table shows the correct entries for tetrafluoroethene, C2F4? Answer ______ 3. When two atoms form a non-polar covalent bond, the two atoms must have A B C D the same the same the same the same atomic size electronegativity ionisation energy number of outer electrons? Answer ______ 4. 20 cm3 of ammonia gas reacted with an excess of heated copper(II) oxide. 3CuO + 2NH3 3Cu + 3H2O + N2 Assuming all measurements were made at 200°C, what would be the volume of gaseous products? A B C D 10 cm3 20 cm3 30 cm3 40 cm3 Answer ______ Higher Chemistry Homework 3∙5 4 5. 20 cm3 of butane is burned in 150 cm3 of oxygen. C4H10(g) + 6½O2(g) 4CO2(g) + 5H2O(g) What is the total volume of gas present after complete combustion of the butane? A B C D 80 cm3 100 cm3 180 cm3 200 cm3 Answer ______ 6. In which of the following reactions would an increase in pressure cause the equilibrium position to move to the left? Answer ______ 7. If ammonia is added to a solution containing copper(II) ions an equilibrium is set up. If acid is added to this equilibrium system A the intensity of the deep blue colour will increase B the equilibrium position will move to the right C the concentration of Cu2+(aq) ions will increase D the equilibrium position will not be affected. Answer _____ 8. A catalyst is added to a reaction at equilibrium. Which of the following does not apply? A The rate of the forward reaction increases. B The rate of the reverse reaction increases. C The position of the equilibrium remains unchanged. D The position of the equilibrium shifts to the right. Answer ______ Higher Chemistry Homework 3∙5 4 9. Atmospheric oxygen, O2(g), dissolves in the Earth’s oceans forming dissolved oxygen, O2(aq), which is essential for aquatic life. An equilibrium is established. (a) (b) 10. (i) What is meant by a reaction at “equilibrium”? 1 (ii) What would happen to the concentration of dissolved oxygen if the temperature of the Earth’s oceans increased? 1 A sample of oceanic water was found to contain 0∙010 g of dissolved oxygen. Calculate the number of moles of dissolved oxygen in the sample. Which of the following is the best description of a feedstock? A A consumer product such as a textile, plastic or detergent. B A complex chemical that has been synthesised from small molecules. C A mixture of chemicals formed from raw materials. D A chemical from which other chemicals can be extracted or synthesised. Answer ______ 11. 1 1 What volume of oxygen (in litres) would be required for the complete combustion of a gaseous mixture containing 1 litre of carbon monoxide and 3 litres of hydrogen? (All volumes are measured at the same temperature and pressure.) A 1 B 2 C 3 D 4 Answer ______ Higher Chemistry Homework 3∙5 1 12. Chlorine gas can be produced by heating calcium hypochlorite, Ca(OCl)2, in dilute hydrochloric acid. Ca(OCl)2(s) (a) (b) 13. + 2HCl(aq) Ca(OH)2(aq) 2Cl2(g) Calculate the mass of calcium hypochlorite that would be needed to produce 0∙096 litres of chlorine gas. (Take the molar volume of chlorine gas to be 24 litres mol-1.) 2 Calculate the atom economy if chlorine gas is the desired product. 2 What type of bonding and structure is found in a fullerene? A Ionic lattice B Metallic lattice C Covalent molecular D Covalent network Answer ______ 14. + 1 Which of the following compounds has the greatest ionic character? A Caesium fluoride B Caesium iodide C Sodium fluoride D Sodium iodide Answer ______ Higher Chemistry Homework 3∙5 1 15. Diols are compounds widely used in the manufacture of polymers. Ethane-1,2-diol is used to produce plastic food containers. In industry ethane-1,2-diol is produced by reacting glycerol with hydrogen. (a) (b) (c) Excess hydrogen reacts with 27∙6 kg of glycerol to produce 13∙4 kg of ethane-1,2-diol. Calculate the percentage yield of ethane-1,2-diol. 2 Calculate the atom economy for the production of ethane-1,2-diol from glycerol and hydrogen. 2 What type of van der Waal’s force is present in both glycerol and ethane-1,2-diol? 1 Higher Chemistry Homework 3∙5 16. Hydrogen sulfide is a toxic gas with the smell of rotten eggs. (a) Hydrogen sulfide gas can be prepared by the reaction of iron(II) sulfide with excess dilute hydrochloric acid: (i) (ii) (b) Draw a diagram to show an assembled apparatus that could be used to measure the volume of H2S gas produced when a sample of iron(II) sulfide reacts with hydrochloric acid. Your diagram should be labelled and should show the names of any chemical used. 2 Calculate the mass, in g, of iron(II) sulfide required to produce 79 cm3 of hydrogen sulfide gas. (Take the molar volume of hydrogen sulfide to be 24 litres mol-1.) 2 Hydrogen sulfide gas produced from iron(II) sulfide is often contaminated with hydrogen gas and gaseous arsenic compounds. (i) Arsenic(III) sulfide is an orange-yellow powder which is insoluble in water. Below 310°C it can sublime, turning from a solid to a gas. Name the type of bonding and structure is present in arsenic(III) sulfide. Higher Chemistry Homework 3∙5 1 16. (b) (ii) To avoid these contaminants, hydrogen sulfide can be made by reacting aluminium sulfide with water. Hydrogen sulfide and aluminium hydroxide are produced. Write a balanced chemical equation for the production of hydrogen sulfide from aluminium sulfide and water. 17. Iron can be produced by reacting iron(III) oxide with carbon monoxide as shown in the equation. Fe2O3 18. 2 + 3CO 2Fe + 3CO2 (a) Calculate the atom economy for the production of iron in reaction. 2 (b) What is the atom economy of the product of a reaction when there are no by-products? 1 (a) Write a balanced equation for the complete combustion of ethyne, C2H2. 1 (b) If 50 cm3 of ethyne is burned completely in 220 cm3 of oxygen, what will be the volume and composition of the resulting gas mixture? 1 (All volumes are measured under the same conditions of temperature and pressure.) Total Marks 36 Higher Chemistry Homework 3∙5