CHAPTER 13
Quiz yourself by thinking what should be in
each of the black spaces below before clicking
on it to display the answer.
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| When limestone is heated it forms lime (calcium oxide) and carbon dioxide. CaCO3(s) → CaO(s) + CO2(g) Name three statements? | 1 Carbon dioxide is a greenhouse gas which may contribute to climate change.
2 Slaked lime is used to neutralise industrial waste.
3 This reaction is an example of thermal decomposition
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| Lime (calcium oxide) is used to treat waste water from a factory. Which substance is removed by the lime? | Sulfuric acid
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| Which process is used to make lime (calcium oxide) from limestone (calcium carbonate)? | Thermal decomposition
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| Why is lime added to the soil before planting the vegetable? | The lime is an indicator
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| In which process is carbon dioxide not formed? | Heating lime
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| Which process does not produce carbon dioxide? | The treatment of acidic soil with lime
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| Carbon dioxide is produced when dilute hydrochloric acid reacts with......... | Copper(II) carbonate
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| Quicklime, which is calcium oxide, is made by heating limestone in a furnace. CaCO3(s) CaO(s) + CO2(g) The reaction does not come to equilibrium. Suggest why the conversion to calcium oxide is complete. | Carbon dioxide escapes
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| Calcium hydroxide, slaked lime, is made from calcium oxide. Write an equation for this reaction | CaO + H2O € Ca(OH)2
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| Explain in 3 points the chemistry of desulfurization of flue gases. | Flue gas contains sulfur dioxide;
Sulfur dioxide is acidic;
Calcium carbonate reacts with sulfur dioxide;
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| Give one other use of calcium carbonate | Making of steel or iron
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| Explain in two terms of collisions between reacting particles each of the following. The reaction rate would be slower if 20.0 g of larger lumps of calcium carbonate and 40 cm3 of hydrochloric acid, concentration 2.0 mol / dm3, were used | Smaller surface area
Lower collision rate
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| Explain in three terms of collisions between reacting particles each of the following. The reaction rate would be faster if the experiment was carried out at a higher temperature | Molecules have more energy
Collide more frequently
More molecules have enough energy to react
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| Lead has a metallic structure which is a lattice of lead ions surrounded by a ‘sea’ of mobile electrons. This structure is held together by attractive forces called a metallic bond. Explain why there are attractive forces in a metallic structure. | Attractive force between positive ions and negative electrons
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| Explain why a metal, such as lead, is malleable. | Layers of lead ions
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| Soda lime is a mixture of sodium hydroxide and calcium oxide. Why do these two substances react with carbon dioxide? | Carbon dioxide is acidic
Sodium hydroxide and calcium oxide are bases
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| Name two substances formed when soda lime reacts with carbon dioxide | Calcium carbonate
Sodium carbonate
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| Calcium carbonate is an important raw material. Name six rocks which is made up of calcium carbonate | Limestone
Marble
Chalk
Coral
Calcite
Aragonite
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| When calcium carbonate is heated strongly, it decomposes. CaCO3 → CaO + CO2 Calculate the relative formula mass of: CaCO3 | 100
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| 7.00 kg of calcium oxide was formed. What mass of calcium carbonate was heated? | 7.00kg is 1/8 of 56
1/8 of 100kg is 12.5kg
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| Calcium carbonate is used to control soil acidity. Why is it important to control soil acidity? Name 3 points. | Plants prefer soil pH about 7
Plants do not grow (well) in acidic soils
Plants grow better To increase crop yields
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| Both calcium carbonate, insoluble in water, and calcium oxide, slightly soluble, are used to increase soil pH. Suggest three advantages of using calcium carbonate. | With calcium carbonate, pH cannot go above 7
It is not washed away by the rain
Remains longer in the soil It is not absorbed by the plant
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| Give two uses of calcium carbonate other than for making calcium oxide and controlling soil pH. | Making steel
Making iron
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| Name three waste gases that leave the blast furnace | Carbon dioxide;
Carbon monoxide;
Nitrogen;
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| Describe how the malleability of iron changes as the percentage of carbon changes. | As the percentage of carbon increases, so the malleability decreases;
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| Iron obtained from the blast furnace contains high levels of carbon. Explain how the amount of carbon in the iron can be decreased | Oxygen (gas) blown in;
Carbon dioxide formed
C + O2 → CO2
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| Iron from the Blast Furnace is impure. It contains 5% of impurities, mainly carbon, sulfur, silicon and phosphorus, which been removed when iron is converted to steel. Explain in 5 how the addition of oxygen and calcium oxide removes these impurities. | Forming an oxide in elements
Gaseous oxides in carbon dioxide
Acidic oxides in Silcon
Equation mark - S + O2 € SO2;
Word equation mark - calcium oxide + phosphorus(III / V) oxide € calcium phosphate;
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| Mild steel is the most common form of steel. Mild steel contains a maximum of 0.3% of carbon. High carbon steel contains 2% of carbon. It is less malleable and much harder than mild steel. Give three uses of mild steel | Machinery;
Chains;
Pylons;
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| Suggest a use of high carbon steel | Knives;
Drills;
Railway tracks;
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| Explain why metals are malleable | Rows or layers slide over one another
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| Suggest an explanation why high carbon steel is less malleable and harder than mild steel. | Carbon atoms or particles in structure different size (to cations);
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