0620_s16_qp_32
A paper of Chemistry, 0620
Questions:
8
Year:
2016
Paper:
3
Variant:
2
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1
The structures of some substances containing phosphorus are shown. P H H H A C B D E PH4 + I– PH4 + I– PH4 + I– Na+ Na+ Na+ P3– Na+ Na+ Na+ P3– Na+ Na+ Na+ P3– PH4 + I– I– PH4 + I– PH4 + P P P P O O O O O O P P P P Answer the following questions about these substances. Which two of these substances are ionic? and Which one of these substances is an element? Explain your answer. Determine the simplest formula for substance D. 1 12 Phosphorus has one naturally occurring isotope. Determine the number of neutrons present in one atom of the isotope P. How many electrons are there in the outer shell of one phosphorus atom? Determine the total number of electrons present in a phosphorus molecule, P4. What type of oxide is phosphorus(oxide? Explain your answer. [Turn over 1 12
2. Atoms, elements and compounds  →  2.2. Atomic structure and the Periodic Table
8. The Periodic Table  →  8.1. Arrangement of elements
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The table describes the ease of reduction of some metal oxides with carbon. ease of reduction on heating metal oxide moderate heating at 200°C needed lead oxide high temperature at 750°C needed nickel oxide very high temperatures above 1700°C needed titanium oxide very high temperature at 900°C needed zinc oxide Put the metals in order of their reactivity. Put the least reactive metal first. least reactive most reactive Aluminium is extracted by the electrolysis of molten aluminium oxide. Predict the products of this electrolysis at the positive electrode , negative electrode When iron reacts with dilute hydrochloric acid, an aqueous solution containing iron(ions is formed. Describe a test for iron(ions. test result Iron rusts very easily. Complete the following sentence. Iron rusts in the presence of and . 1 12 Describe one method of rust prevention and explain how it works. [Turn over 1 12
9. Metals  →  9.6. Extraction of metals
9. Metals  →  9.5. Corrosion of metals
4. Electrochemistry  →  4.1. Electrolysis
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Sulfur dioxide reacts with excess oxygen to form sulfur trioxide. 2SO3⇌ O2+ 2SO2What is the meaning of the symbol ⇌? The energy level diagram for the reaction is shown. energy 2SO2+ O22SO3Is this reaction exothermic or endothermic? Give a reason for your answer. 1 12 The graph shows how the percentage yield of sulfur trioxide changes with temperature when the pressure is kept constant. temperature / °C % yield of sulfur trioxide Describe how the percentage yield of sulfur trioxide changes with temperature. Determine the percentage yield of sulfur trioxide when the temperature is 500ºC. Describe a test for sulfur dioxide. test result Give one use of sulfur dioxide. [Turn over 1 12 Sulfur dioxide reacts with magnesium. 2Mg + SO2 →2MgO + S Which substance is reduced in this reaction? Explain your answer. Sulfur dioxide reacts with water to form sulfurous acid, H2SO3. Sulfurous acid reacts with hydrogen sulfide to form water and sulfur. Complete the chemical equation for this reaction. H2SO3 + 2H2S → H2O + 3S 1 12
6. Chemical reactions  →  6.3. Reversible reactions and equilibrium
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Alkanes, alkenes and alcohols are three different homologous series of organic compounds. What is meant by the term homologous series? The structures of some alkanes, alkenes and alcohols are shown below. C H F H H H C H O H H H C H G H H H C H H C H O H H H C H H C H H C H H H H C C H H H I J K C C H C C H H H H H H H Which two of these compounds, F, G, H, I, J and K, are saturated hydrocarbons? Explain your answer. Which one of these compounds is the main constituent of natural gas? Which two of these compounds are alkenes? and Why are two compounds, I and K, not hydrocarbons? [Turn over 1 12 The table gives some information about four alcohols. boiling point /ºC density in g/cm3 molecular formula alcohol 0.793 CH4O methanol 0.789 C2H6O 0.804 C3H8O propanol 0.810 C4H10O butanol Give the name of the alcohol with the formula C2H6O. A student predicts that the density of the alcohols increases as the number of carbon atoms increases. Does the data in the table support this prediction? Explain your answer. Suggest a value for the boiling point of methanol. 1 12 The alcohol with the formula C2H6O burns in a limited supply of air to form carbon monoxide and water. Complete the chemical equation for this reaction. C2H6O + 2O2 → CO + H2O State an adverse effect of carbon monoxide on health. [Turn over 1 12
11. Organic chemistry  →  11.1. Formulae, functional groups and terminology
11. Organic chemistry  →  11.5. Alkenes
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Chlorine, bromine and iodine are halogens. The melting point of bromine is –7ºC. The boiling point of bromine is +59ºC. Deduce the state of bromine at +6ºC. Explain your answer. Complete the word equation for the reaction of chlorine with potassium iodide. chlorine + potassium iodide → + Suggest why iodine does not react with aqueous potassium bromide. The structure of the dye Lithol fast yellow is shown. C C C C O O C C Cl Cl H H N H H H C H H N H N H O O N C C C C C C H Complete the table and calculate the relative molecular mass of Lithol fast yellow. atomic mass number of atoms type of atom 13 × 12 = 156 carbon 10 × 1 = 10 hydrogen 4 × 14 = 56 nitrogen oxygen chlorine relative molecular mass = 1 12 Chromatography is used to separate a mixture of dyes. Draw a cross on the diagram to show where the mixture of dyes is placed at the start of the chromatography. solvent Suggest a suitable solvent that could be used. Describe what you would observe as the experiment proceeds. [Turn over 1 12
8. The Periodic Table  →  8.3. Group VII properties
11. Organic chemistry  →  11.4. Alkanes
11. Organic chemistry  →  11.5. Alkenes
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Sodium is a metal in Group I of the Periodic Table. Describe some physical and chemical properties of sodium. In your answer include • any observations about the reactions of sodium, • at least one word equation. The presence of sodium in compounds can be confirmed using a flame test. Describe how a flame test is carried out and give the result of the test for sodium. test result Aqueous sodium hydroxide is strongly alkaline. Which one of the following values is the pH of a strongly alkaline solution? Put a ring around the correct answer. pH 13 D pH 7 C pH 2 B pH 1 A Describe how you could use litmus to show that aqueous sodium hydroxide is alkaline. 1 12 Sodium sulfite, Na2SO3, reacts with hydrochloric acid. Na2SO3+ 2HCl→2NaCl+ SO2+ H2OExplain why this reaction could have an adverse effect on health if not carried out in a fume cupboard. [Turn over 1 12
7. Acids, bases and salts  →  7.1. The characteristic properties of acids and bases
12. Experimental techniques and chemical analysis  →  12.5. Identification of ions and gases
9. Metals  →  9.4. Reactivity series
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When magnesium reacts with hydrochloric acid, the products are aqueous magnesium chloride and hydrogen. Mg+ 2HCl→MgCl2+ H2A student used the apparatus shown to follow the progress of this reaction. dilute hydrochloric acid magnesium Complete the diagram by putting the correct labels in the boxes. The student conducted two experiments using the same mass of magnesium in each experiment and two different concentrations of hydrochloric acid. The hydrochloric acid was in excess. All other conditions were kept constant. The student measured the volume of hydrogen produced over a period of time. The graph shows the results. time / s volume of hydrogen / cm3 0.5 mol / dm3 HCl 1.0 mol / dm3 HCl 1 12 Which concentration of hydrochloric acid gave the faster initial rate of reaction? Use the graph to explain your answer. Draw a curve on the graph on page 16 to show how the volume of hydrogen would change if a third experiment was carried out using 1.5mol/dm3 hydrochloric acid and the same mass of magnesium. Give one use of hydrogen. Explosions have occasionally been reported where tiny particles of metal dust escape into the air. Explain why metal dust can form an explosive mixture with air. [Turn over 1 12
9. Metals  →  9.4. Reactivity series
6. Chemical reactions  →  6.2. Rate of reaction
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Solder is an alloy of lead and tin. What is the meaning of the term alloy? State the name of another alloy. A student heated a piece of solder carefully. The diagram shows what happens to the solder. at the start after 2 minutes solder solder iron plate Use the kinetic particle theory to describe and explain what happens to the solder as it changes state. When heated above 1744°C, lead forms a vapour. Describe a general property of a vapour which is not shown by a solid. 1 12
1. States of matter  →  1.1. Solids, liquids and gases
9. Metals  →  9.3. Alloys and their properties
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