6.3. Reversible reactions and equilibrium
A subsection of Chemistry, 5070, through 6. Chemical reactions
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Iron is a transition element. State two physical properties of iron that are typical of a transition element. 1. 2. Name an industrial process that uses iron as a catalyst. Iron(sulfate thermally decomposes to form iron(oxide, sulfur dioxide and sulfur trioxide. 2FeSO4Fe2O3+ SO2+ SO3Explain how the equation shows that this reaction involves oxidation. A sample of 6.08 g of FeSO4 is heated until all the sample has thermally decomposed. Calculate the volume of sulfur dioxide formed, SO2, in dm3, measured at room temperature and pressure. volume of sulfur dioxide dm3 Iron(oxide reacts with dilute sulfuric acid to make iron(sulfate, Fe2(SO4)3. Construct the equation for this reaction. Describe a chemical test that can be used to distinguish between aqueous solutions of iron(sulfate and iron(sulfate. chemical test result with iron(sulfate result with iron(sulfate
5070_s20_qp_21
THEORY
2020
Paper 2, Variant 1
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Sulfur dioxide is a colourless gas which can be found in air. State one environmental problem caused by the presence of sulfur dioxide in air. When heated in air iron pyrite, FeS2, reacts with oxygen. Sulfur dioxide and iron(oxide, Fe2O3, are the products of this reaction. Construct the equation for this reaction. Give one use for sulfur dioxide. Liquid sulfur dioxide is stored in cylinders. When the cylinder is opened the liquid quickly changes into a gas. Use the kinetic particle theory to describe the changes in movement and arrangement of the particles when liquid sulfur dioxide becomes a gas. Sulfur dioxide has a low melting point. Suggest, in terms of structure and bonding, why sulfur dioxide has a low melting point. Describe the chemical test for sulfur dioxide. test observation
5070_s20_qp_22
THEORY
2020
Paper 2, Variant 2
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Iron pyrite, FeS2, is an ore of iron. When heated in air, FeS2 produces both iron(oxide and sulfur dioxide. Balance the equation shown. ………. FeS2 + ………. O2 ………. Fe2O3 + ……… SO2 Describe one environmental problem caused by sulfur dioxide in the air. Describe how sulfur dioxide is converted into sulfuric acid in the contact process. State one other use of sulfur dioxide. Iron(oxide, coke, limestone and hot air are heated together in a blast furnace to make molten iron. Describe the function in the blast furnace of: coke limestone hot air.
5070_s21_qp_21
THEORY
2021
Paper 2, Variant 1
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Sulfur dioxide and oxides of nitrogen are pollutants found in air. State one environmental problem caused by the presence of sulfur dioxide in the air. Coal-fired power stations produce sulfur dioxide as a pollutant. The sulfur dioxide produced is prevented from entering the air by a process called flue gas desulfurisation, FGD. Name the compound used in FGD that reacts with the sulfur dioxide. Coal-fired power stations also produce oxides of nitrogen such as NO. NO is produced when nitrogen, N2, reacts with oxygen. Construct the equation for this reaction. Draw a dot-and-cross diagram to show the bonding in a molecule of nitrogen. Only include the outer shell electrons. Explain why the rate of reaction between nitrogen and oxygen increases as the temperature increases. Nitrogen dioxide, NO2, reacts with water to form a mixture of dilute nitric acid, HNO3, and dilute nitrous acid, HNO2. 2NO2 + H2O HNO2 + HNO3 Nitrogen dioxide reacts with aqueous sodium hydroxide to form two different salts and water. Construct the equation for this reaction. Nitric acid is a strong acid. Nitrous acid is a weak acid. Describe the difference between a weak acid and a strong acid.
5070_s21_qp_22
THEORY
2021
Paper 2, Variant 2
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