5070_s22_qp_21
A paper of Chemistry, 5070
Questions:
9
Year:
2022
Paper:
2
Variant:
1
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1
Choose from the following compounds to answer the questions. NH4Cl BaSO4 KI K2SO3 Mg(NO3)2 NaOCOCH3 Na2CO3 Na3PO4 ZnSO4 Each compound may be used once, more than once or not at all. State which compound: reacts with dilute nitric acid to form a gas that turns limewater milky reacts with warm aqueous sodium hydroxide to form a gas that turns damp red litmus paper blue reacts with dilute hydrochloric acid to give a gas that decolourises acidified potassium manganate(is prepared using a precipitation reaction contains an anion with a charge of –3 is used to test for an oxidising agent.
12. Experimental techniques and chemical analysis  →  12.5. Identification of ions and gases
6. Chemical reactions  →  6.4. Redox
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2
The table shows some information about elements in Group V. element electronic configuration melting point / °C boiling point / °C nitrogen 2, 5 –210 –196 phosphorus arsenic 2, 8, 18, 5 antimony 2, 8, 18, 18, 5 bismuth 2, 8, 18, 32, 18, 5 State the electronic configuration for phosphorus. Explain why it is easier to predict the boiling point of bismuth than to predict its melting point. Use information from the table to explain why antimony is a liquid at 1000 °C. Nitrogen exists as a diatomic molecule, N2. Draw the dot-and-cross diagram to show the bonding in N2. Show only the outer shell electrons. Explain, in terms of structure and bonding, why nitrogen has a low melting point. Bismuth is a metal. Predict two physical properties of bismuth. Calculate the volume, in dm3, of 19.2 g of nitrogen at room temperature and pressure. Give your answer to two significant figures. volume dm3
8. The Periodic Table  →  8.1. Arrangement of elements
2. Atoms, elements and compounds  →  2.2. Atomic structure and the Periodic Table
10. Chemistry of the environment  →  10.1. Water
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3
The diagram shows some reactions of butanol. gas A and liquid B organic liquid D liquid B and gas C liquid B and organic liquid E complete combustion acidified potassium manganate(heat with ethanoic acid incomplete combustion H C H H H C H H C H H C H C OH A, B and C are different compounds. Identify by name A, B and C. A B C Name and draw the structure of D. name structure Name and draw the structure of E. name structure
11. Organic chemistry  →  11.2. Naming organic compounds
5. Chemical energetics  →  5.1. Exothermic and endothermic reactions
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4
The table shows information about some particles. particle proton number nucleon number 17Cl 17Cl – 19K 19K+ State the number of neutrons in 35 17Cl. State the number of electrons in 35 17Cl –. 19K is the full symbol for one isotope of potassium. Suggest the full symbol for one other isotope of potassium. Describe how a potassium ion, K+, is formed from a potassium atom, K. Potassium chloride is an ionic compound. Potassium chloride has a high melting point and a high boiling point. Explain why potassium chloride has a high melting point. Predict two other physical properties of potassium chloride.
2. Atoms, elements and compounds  →  2.2. Atomic structure and the Periodic Table
2. Atoms, elements and compounds  →  2.3. Isotopes
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5
Iron reacts with steam and with dilute sulfuric acid. The reaction between iron and steam is reversible. The forward reaction is exothermic. 3Fe+ 4H2OFe3O4+ 4H2An equilibrium mixture is formed when the reversible reaction happens in a closed system. Predict what happens to the amount of hydrogen in the equilibrium mixture if the temperature is increased and the pressure remains constant. Explain your answer. prediction explanation Predict what happens to the amount of hydrogen in the equilibrium mixture if the pressure is increased and the temperature remains constant. Explain your answer. prediction explanation Iron reacts with dilute sulfuric acid to make aqueous iron(sulfate, FeSO4. Construct the ionic equation, with state symbols, for this reaction. Describe a chemical test to confirm that iron(sulfate is formed instead of iron(sulfate. The aqueous iron(sulfate formed is crystallised to make hydrated iron(sulfate, FeSO4•7H2O. Calculate the relative formula mass of hydrated iron(sulfate. relative formula mass = A student uses 2.80 g of iron to make 12.5 g of hydrated iron(sulfate crystals. This is a 90% yield. Calculate the mass of hydrated iron(sulfate crystals made from 2.80 g of iron if the yield is 100%. mass = g Aqueous iron(sulfate is electrolysed using graphite electrodes. Predict the products of this electrolysis. product at cathode product at anode Iron is extracted from iron ore in a blast furnace. Describe the essential reactions involved in the extraction of iron.
9. Metals  →  9.6. Extraction of metals
6. Chemical reactions  →  6.3. Reversible reactions and equilibrium
4. Electrochemistry  →  4.1. Electrolysis
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6
Carbon monoxide and nitrogen monoxide are pollutants formed in a car engine. Describe how nitrogen monoxide is formed in a car engine. Carbon monoxide reacts with nitrogen monoxide as shown in the equation. 2CO + 2NO 2CO2 + N2 This reaction is extremely slow at room temperature but is much faster in the presence of a catalyst in a catalytic converter. Explain why this reaction involves both oxidation and reduction. The reaction between carbon monoxide and nitrogen monoxide is exothermic. Explain, using ideas about bond breaking and bond forming, why the reaction is exothermic. Explain, using ideas about particles, why increasing the temperature increases the rate of the reaction between carbon monoxide and nitrogen monoxide. Explain why a catalyst increases the rate of the reaction between carbon monoxide and nitrogen monoxide. Explain, using ideas about particles, why the catalyst in a catalytic converter needs to have a large surface area.
10. Chemistry of the environment  →  10.3. Air quality and climate
6. Chemical reactions  →  6.2. Rate of reaction
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7
Aluminium is an element in Group III of the Periodic Table. Aluminium is used to make containers for food because it does not react with water. State and explain, in terms of its properties, one other large-scale use of aluminium. large-scale use explanation Explain why aluminium does not react with cold water. Describe, with the aid of a labelled diagram, the metallic bonding in solid aluminium. Aluminium is manufactured by the electrolysis of aluminium oxide dissolved in molten cryolite. Write the ionic equations for the reactions at the cathode and at the anode. cathode anode A sample of 2.34 g of aluminium is reacted with 50.0 cm3 of 2.00 mol / dm3 sulfuric acid. 2Al + 3H2SO4Al 2(SO4)3+ 3H2Show by calculation that the aluminium is in excess in this reaction.
9. Metals  →  9.4. Reactivity series
9. Metals  →  9.2. Uses of metals
9. Metals  →  9.6. Extraction of metals
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8
Alkenes are a homologous series of unsaturated hydrocarbons. Name the alkene which has only three carbon atoms in its molecule. Draw the structure of an unbranched and of a branched alkene. Show all of the atoms and all of the bonds in each structure. unbranched alkene branched alkene Describe a chemical test that distinguishes an alkene from an alkane. chemical test result with alkene result with alkane Alkenes are manufactured by the cracking of long chain hydrocarbons. The equation for the cracking of C14H30 is shown. C14H30 2X + C8H18 Give two reasons why the cracking of long chain hydrocarbons is important. Compound X contains 85.7% carbon by mass and 14.3% hydrogen by mass. Calculate, using the percentage composition data, the empirical formula of X. Show your working. State the molecular formula of X. empirical formula molecular formula
11. Organic chemistry  →  11.5. Alkenes
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9
Ammonia, NH3, is used to make nitrogenous fertilisers. Ammonia is manufactured using the reversible reaction between nitrogen and hydrogen. Construct the equation for this reversible reaction. Ammonia is used to make the soluble salt ammonium nitrate, NH4NO3. Name the acid that reacts with ammonia to make ammonium nitrate. Calculate the percentage by mass of nitrogen in ammonium nitrate. percentage by mass = Nitrogenous fertilisers such as ammonium nitrate leach from farmland and cause water pollution problems in rivers and lakes. Name the process caused by this type of water pollution. Explain why this type of water pollution problem is increased when nitrate fertilisers are used instead of other fertilisers. A farmer adds ammonium nitrate, NH4NO3, to soil. The farmer then adds calcium hydroxide, Ca(OH)2, to the same soil. State the purpose of adding calcium hydroxide to soil. Construct the equation for the reaction between ammonium nitrate and calcium hydroxide. Using your equation, explain why the ammonium nitrate fertiliser is less effective after calcium hydroxide is added.
10. Chemistry of the environment  →  10.2. Fertilisers
6. Chemical reactions  →  6.3. Reversible reactions and equilibrium
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