0620_s16_qp_42
A paper of Chemistry, 0620
Questions:
6
Year:
2016
Paper:
4
Variant:
2
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1
For each of the following, give the name of an element from Period 2 (lithium to neon), which matches the description. Elements may be used once, more than once or not at all. an element which is gaseous at room temperature and pressure an element which forms an oxide that is a reactant in photosynthesis an element that is a product of photosynthesis an element that makes up approximately 78% by volume of the air an element which has atoms with a full outer shell of electrons an element which exists as both diamond and graphite an element that reacts vigorously with cold water a soft metallic element which is stored in oil Give the formula of a compound that contains only boron and oxygen, only lithium and nitrogen.
2. Atoms, elements and compounds  →  2.2. Atomic structure and the Periodic Table
3. Stoichiometry  →  3.1. Formulae
8. The Periodic Table  →  8.4. Transition elements
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3
Gallium is a metallic element in Group III. It has similar properties to aluminium. Describe the structure and bonding in a metallic element. You should include a labelled diagram in your answer. Explain why metallic elements such as gallium are good conductors of electricity. Give the formula of gallium(chloride, gallium(sulfate. Gallium(oxide, Ga2O3, is amphoteric. Write the chemical equation for the reaction between gallium(oxide and dilute nitric acid to form a salt and water only. The reaction between gallium(oxide and sodium hydroxide solution forms only water and a salt containing the negative ion Ga2O4 2–. Write the chemical equation for this reaction. Alloys of gallium and other elements are often more useful than the metallic element itself. Suggest two reasons why alloys of gallium are more useful than the metallic element.
2. Atoms, elements and compounds  →  2.7. Metallic bonding
2. Atoms, elements and compounds  →  2.4. Ions and ionic bonds
9. Metals  →  9.1. Properties of metals
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4
Hydrogen can be manufactured from methane by steam reforming. CH4+ H2OCO+ 3H2The reaction is carried out using a nickel catalyst at temperatures between 700 °C and 1100 °C and using a pressure of one atmosphere. The forward reaction is endothermic. What is meant by the term catalyst? Suggest two reasons why a temperature lower than 700 °C is not used. Suggest one advantage of using a pressure greater than one atmosphere. Suggest one disadvantage of using a pressure greater than one atmosphere. Hydrogen can also be manufactured by electrolysis. The electrolyte is concentrated aqueous sodium chloride. The electrodes are inert. The products of electrolysis are hydrogen, chlorine and sodium hydroxide. Define the term electrolysis. Name a substance that can be used as the inert electrodes. Write an ionic half-equation for the reaction in which hydrogen is produced. Where is hydrogen produced in the electrolytic cell? Describe a test for chlorine. test result The electrolysis of concentrated aqueous sodium chloride can be represented by the following word equation. sodium chloride + water → sodium hydroxide + hydrogen + chlorine Construct a chemical equation to represent this reaction. Do not include state symbols. State one use of chlorine, sodium hydroxide, hydrogen.
4. Electrochemistry  →  4.1. Electrolysis
6. Chemical reactions  →  6.3. Reversible reactions and equilibrium
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5
Hydrocarbons are compounds which contain hydrogen and carbon only. • 10 cm3 of a gaseous hydrocarbon, CxHy, are burned in 100 cm3 of oxygen, which is an excess of oxygen. • After cooling to room temperature and pressure, there is 25 cm3 of unreacted oxygen, 50 cm3 of carbon dioxide and some liquid water. All volumes are measured under the same conditions of temperature and pressure. What is meant by an excess of oxygen? What was the volume of oxygen that reacted with the hydrocarbon? Complete the table below to express the smallest whole number ratio of volume of hydrocarbon reacted : volume of oxygen reacted : volume of carbon dioxide produced volume of hydrocarbon reacted volume of oxygen reacted volume of carbon dioxide produced smallest whole number ratio of volumes Use your answer to to find the mole ratio in the equation below. Complete the equation and deduce the formula of the hydrocarbon. CxHy+ O2→ CO2+ H2Oformula of hydrocarbon = Cracking is used to convert long chain alkanes into shorter chain alkanes and alkenes. Alkenes are unsaturated compounds. Decane, C10H22, can be cracked to give propene and one other product. Complete the chemical equation. C10H22 → C3H6 + What is meant by the term unsaturated? Describe a test to show that propene is an unsaturated compound. test result Propene can be polymerised. The only product is polypropene. The equation for the polymerisation is: n C H CH3 C H H nC3H6 Name the type of polymerisation that occurs. Deduce the maximum mass of polypropene that could be produced from 1 kg of propene. kg Give the empirical formula of propene, polypropene.
11. Organic chemistry  →  11.5. Alkenes
1. States of matter  →  1.1. Solids, liquids and gases
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6
Zinc is extracted from an ore called zinc blende, which consists mainly of zinc sulfide, ZnS. The zinc sulfide in the ore is first converted into zinc oxide. Describe how zinc oxide is made from zinc sulfide. Write a chemical equation for the reaction in . Zinc oxide is converted into zinc. Zinc oxide and coke are fed into a furnace. Hot air is blown into the bottom of the furnace. Zinc has a melting point of 420 °C and a boiling point of 907 °C. The temperature inside the furnace is over 1000 °C. Explain how zinc oxide is converted into zinc. Your answer should include details of how the heat is produced and equations for all the reactions you describe. Explain why the zinc produced inside the furnace is a gas. State the name of the physical change for conversion of gaseous zinc into molten zinc. Rusting of steel can be prevented by coating the steel with a layer of zinc. Explain, in terms of electron transfer, why steel does not rust even if the layer of zinc is scratched so that the steel is exposed to air and water. When a sample of steel is added to dilute hydrochloric acid, an aqueous solution of iron(chloride, FeCl 2, is formed. When a sample of rust is added to dilute hydrochloric acid, an aqueous solution of iron(chloride, FeCl 3, is formed. Aqueous sodium hydroxide is added to the solutions of iron(chloride and iron(chloride. Complete the table below, showing the observations you would expect to make. iron(chloride solution iron(chloride solution aqueous sodium hydroxide Solutions of iron(chloride and iron(chloride were added to solutions of potassiumiodide and acidifiedpotassiummanganate(. The results are shown in the table. iron(chloride solution iron(chloride solution potassium iodide solution no change solution turns from colourless to brown acidified potassium manganate(solution solution turns from purple to colourless no change What types of substance cause potassium iodide solution to turn from colourless to brown? What types of substance cause acidified potassium manganate(solution to turn from purple to colourless? Which ion in iron(chloride solution causes potassium iodide solution to turn from colourless to brown? Which ion in iron(chloride solution causes acidified potassium manganate(solution to turn from purple to colourless?
9. Metals  →  9.4. Reactivity series
9. Metals  →  9.6. Extraction of metals
9. Metals  →  9.5. Corrosion of metals
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