Which metal is less reactive than copper? [mr-1]Which metal is more reactive than magnesium? [mr-2]Which metal is more reactive than hydrogen but less reactive than carbon? [mr-3]Which metal is less reactive than sodium but cannot be extracted using carbon? [mr-4]
Which is formed when a metal reacts with cold water? [mr-5]Which is a compound formed when a metal reacts with an acid? [mr-6]Which is formed when a metal reacts with either water or an acid? [mr-7]
Which is formed when a heated metal reacts with steam? [mr-8] Information is given below on the reactivity of four metals Wa, Xb, Yc and Zd (NOT their real chemical symbols) ... Information is given below on the reactivity of four metals Wa, Xb, Yc and Zd (NOT their real chemical symbols) ... Information is given below on the reactivity of four metals Wa, Xb, Yc and Zd (NOT their real chemical symbols) ... Information is given below on the reactivity of four metals Wa, Xb, Yc and Zd (NOT their real chemical symbols) ...From the four elements listed, which is a metal which is most likely to be found in the ground as the metal itself? [mr-13]From the four elements listed, which is a non-metal with no metallic character at all? [mr-14]From the four elements listed, which is a metal that displaces hydrogen from acids but not from cold water? [mr-15]From the four elements listed, which is a metal that cannot be extracted by displacement with carbon? [mr-16]Which is formed by the reaction of heated magnesium with steam? [mr-17]Which is formed by the reaction of magnesium with cold water? [mr-18]Which is formed by the reaction of magnesium with hydrochloric acid? [mr-19]Which is formed by the reaction of magnesium with sulphuric acid? [mr-20]Which of A to D is less reactive than copper? [mr-21]Which is more reactive than magnesium? [mr-22]Which is more reactive than hydrogen but less reactive than carbon? [mr-23]Which is less reactive than sodium but cannot be extracted from its ore using carbon? [mr-24]Which is found in rocks as the metal itself? [mr-25]Which is a non-metal with a little metallic character? [mr-26]Which is a metal that displaces hydrogen from dilute acids but not from cold water? [mr-27]Which cannot be extracted from its ore with carbon? [mr-28]
Which of these in contact with iron will cause rusting? [mr-29] A steel pier in the sea rusts. The rust consists of? [mr-30] Which of these metals can be used in the 'sacrificial corrosion' method for protecting steel structures from rusting? [mr-31] Which of these metals can be used in the 'sacrificial corrosion' method for protecting steel structures from rusting? [mr-32] Which of these reactions is possible? [mr-33]Which of these reactions is possible? [mr-34]Which of these reactions is possible? [mr-35]Which of these reactions is possible? [mr-36]Which of these reactions is possible? [mr-37]Which of these reactions is possible? [mr-38]Which of these reactions is possible? [mr-39]Which of these reactions is possible? [mr-40] Rust readily forms if an iron object is surrounded by? [mr-45] Which of the following cannot be predicted about metal X, given its position in the reactivity series of metals? [mr-46] Which will displace iron from iron oxide? [mr-47] Road tankers carrying acid use steel tanks lined with glass. The glass is used because? [mr-48] Corrosion occurs when a metal is attacked by? [mr-49] When scrap iron is added to blue copper sulphate solution, a pinky-brown deposit is formed and a pale green solution is left above it. The pinky-brown deposit is? [mr-50] When scrap iron is added to blue copper sulphate solution, a pinky-brown deposit is formed and a pale green solution is left above it. The pale green solution is of? [mr-51] When iron becomes coated in rust, the chemical process is an example of? [mr-52]
The effect of connecting other metals to an iron nail was investigated. From the observations you can deduce? [mr-57]The effect of connecting other metals to an iron nail was investigated. From the observations you can deduce? [mr-58]The effect of connecting other metals to an iron nail was investigated. From the observations you can deduce? [mr-59]The effect of connecting other metals to an iron nail was investigated. From the observations you can deduce? [mr-60]
Aluminium window frames do not corrode away because the aluminium is? [mr-63] Rust protection from galvanising steel car bodies is done by coating the metal in? [mr-64] The rusting of iron is described as an oxidation because the iron atoms? [mr-65]Which reacts with water to form hydrogen? [mr-66]
Copper can be used for roofing domes on buildings because it? [mr-67]Salt water speeds up the corrosion of metals because it contains ions from salts like sodium chloride. Aluminium can be used for the upper structures of ships because the aluminium? [mr-68]In which reaction is a metal oxidised? [mr-69]In which reaction is a solid non-metal oxidised? [mr-70]In which reaction is a gaseous non-metal oxidised? [mr-71]In which reaction is a metal oxide reduced? [mr-72] Four chemical changes are shown below as part, or full, word equations. Which can be described as an oxidation only? [mr-73] Four chemical changes are shown below as part, or full, word equations. Which can be described as a reduction only? [mr-74] Four chemical changes are shown below as part, or full, word equations. Which can be described as an oxidation and reduction (redox)? [mr-75] Four chemical changes are shown below as part, or full, word equations. Which can be described as an oxidation and reduction (redox)? [mr-76] Given the following four observations of the reactions of four metals ... Given the following five observations of the reactions of four metals with hydrogen (H), carbon (C) and other metal oxides ... Underground pipes made of steel (alloy of iron) can be protected from rusting if you attach metal blocks made of a? [mr-88] Stainless steel is made by alloying iron, nickel and ? [mr-89] Roofs of buildings made of copper weather to give a compound ? in colour. [mr-90]
Roofs of buildings made of iron weather to give a compound ? in colour. [mr-91]When copper is heated in air, the oxide compound formed is ? in colour. [mr-92]When magnesium burns in air, the oxide compound formed is ? in colour. [mr-93] Given the following three observations of the reactions of four metals ... Given the following ionic redox equation for the displacement of copper from copper(II) sulphate using zinc metal ... Given the following ionic redox equation for the displacement of copper from copper(II) sulphate using zinc metal ... Given the following ionic redox equation for the displacement of copper from copper(II) sulphate using zinc metal ... Given the following ionic redox equation for the displacement of copper from copper(II) sulphate using zinc metal ...
A simple battery cell can be made by connecting two metal strips dipped into a conducting solution of ions to form a complete circuit. The copper-zinc cell gives a voltage of 1.10 V. What voltage would be produced by a magnesium-iron cell? [mr-53]A simple battery cell can be made by connecting two metal strips dipped into a conducting solution of ions to form a complete circuit. The copper-zinc cell gives a voltage of 1.10 V. What voltage would be produced by a zinc-silver cell? [mr-54]A simple battery cell can be made by connecting two metal strips dipped into a conducting solution of ions to form a complete circuit. The copper-zinc cell gives a voltage of 1.10 V. Which combination of metals will give a voltage of 0.79 V? [mr-55]A simple battery cell can be made by connecting two metal strips dipped into a conducting solution of ions to form a complete circuit. The copper-zinc cell gives a voltage of 1.10 V. Which combination of metals will give a voltage of 0.95 V? [mr-56] Given the following equation: Mg(s) + ? ==> MgCl2(aq) + H2(g) Given the following equation: Ca(s) + 2H2O(l) ==> ? + H2(g) Given the following equation: Zn(s) + H2SO4(aq) ==> ? + H2(g) Given the following equation: Mg(s) + ? ==> MgO(s) H2(g) Given the following equation: Zn(s) + ? ==> ZnSO4(aq) + Fe(s) Given the following equation: ? + 3Zn(s) ==> 2Fe(s) + 3ZnSO4(aq) Given the following equation: 2Al(s) + 3CuO(s) ==> ? + 3Cu(s) Given the following equation: 2K(s) + 2H2O(l) ==> ? + H2(g) The rusting of iron is described as an oxidation because the iron atoms? [mr-85] Which of the following is a definition of oxidation? [mr-95] Which of the following is a definition of reduction? [mr-96] Which of the following is a definition of reduction? [mr-97]
Galvanising, means 'coating with zinc', and is used to protect iron and steel objects from corrosion. The object can be dipped in a bath of molten zinc! but it is now mainly done by electrolysis. At the positive electrode? [mr-98] Galvanising, means 'coating with zinc', and is used to protect iron and steel objects from corrosion. The object can be dipped in a bath of molten zinc! but it is now mainly done by electrolysis. At the negative electrode? [mr-99] Galvanising, means 'coating with zinc', and is used to protect iron and steel objects from corrosion. The object can be dipped in a bath of molten zinc! but it is now mainly done by electrolysis. The process at the positive electrode is described as a ...?... reaction. [mr-100] Galvanising, means 'coating with zinc', and is used to protect iron and steel objects from corrosion. The object can be dipped in a bath of molten zinc! but it is now mainly done by electrolysis. The process at the negative electrode is described as ...?... reaction. [mr-101] Galvanising, means 'coating with zinc', and is used to protect iron and steel objects from corrosion. The object can be dipped in a bath of molten zinc! but it is now mainly done by electrolysis. The overall process is described as ...?... reaction. [mr-102]
Galvanising means coating an iron (Fe) or steel object with a layer of zinc (Zn) to protect it from corrosion. Steel cans can also be coated with tin (Sn), also to protect it from corrosion, including fruit juices in 'tin' cans. When the zinc coating is scratched through to the iron underneath, the iron still does not corrode intially. However, if the tin surface is scratched through to the iron, the iron corrodes even faster compared to when there was no coating at. This means? [mr-103]Galvanising means coating an iron (Fe) or steel object with a layer of zinc (Zn) to protect it from corrosion. Steel cans can also be coated with tin (Sn), also to protect it from corrosion, including fruit juices in 'tin' cans. When the zinc coating is scratched through to the iron underneath, the iron still does not corrode intially. However, if the tin surface is scratched through to the iron, the iron corrodes even faster compared to when there was no coating at. This means? [mr-104]Galvanising means coating an iron (Fe) or steel object with a layer of zinc (Zn) to protect it from corrosion. Steel cans can also be coated with tin (Sn), also to protect it from corrosion, including fruit juices in 'tin' cans. When the zinc coating is scratched through to the iron underneath, the iron still does not corrode intially. However, if the tin surface is scratched through to the iron, the iron corrodes even faster compared to when there was no coating at. This means? [mr-105]Galvanising means coating an iron (Fe) or steel object with a layer of zinc (Zn) to protect it from corrosion. Steel cans can also be coated with tin (Sn), also to protect it from corrosion, including fruit juices in 'tin' cans. When the zinc coating is scratched through to the iron underneath, the iron still does not corrode intially. However, if the tin surface is scratched through to the iron, the iron corrodes even faster compared to when there was no coating at. This means? [mr-106]Galvanising means coating an iron (Fe) or steel object with a layer of zinc (Zn) to protect it from corrosion. Steel cans can also be coated with tin (Sn), also to protect it from corrosion, including fruit juices in 'tin' cans. When the zinc coating is scratched through to the iron underneath, the iron still does not corrode intially. However, if the tin surface is scratched through to the iron, the iron corrodes even faster compared to when there was no coating at. This means? [mr-107]A simple battery cell can be made by connecting two metal strips dipped into a conducting solution of ions to form a complete circuit. Some of the first 'batteries' were made from dipping strips of zinc and copper into their salt solutions, but even a solution of acid works too. The electrode potential (V) is a measure of how easily a metal loses electrons. The more negative the potential the more easily the metal atoms lose electrons. The potential difference of the cell (p.d. in Volts) is the difference between the two electrode potentials of the two metals (shown in the table compared to hydrogen). What voltage does this cell produce if copper and zinc electrodes are used? [mr-108]A simple battery cell can be made by connecting two metal strips dipped into a conducting solution of ions to form a complete circuit. Some of the first 'batteries' were made from dipping strips of zinc and copper into their salt solutions, but even a solution of acid works too. The electrode potential (V) is a measure of how easily a metal loses electrons. The more negative the potential the more easily the metal atoms lose electrons. The potential difference of the cell (p.d. in Volts) is the difference between the two electrode potentials of the two metals (shown in the table compared to hydrogen). Which two metals will give a cell voltage of 1.25V? [mr-109]A simple battery cell can be made by connecting two metal strips dipped into a conducting solution of ions to form a complete circuit. Some of the first 'batteries' were made from dipping strips of zinc and copper into their salt solutions, but even a solution of acid works too. The electrode potential (V) is a measure of how easily a metal loses electrons. The more negative the potential the more easily the metal atoms lose electrons. The potential difference of the cell (p.d. in Volts) is the difference between the two electrode potentials of the two metals (shown in the table compared to hydrogen). Which two metals will give a cell voltage of 0.65V? [mr-110]A simple battery cell can be made by connecting two metal strips dipped into a conducting solution of ions to form a complete circuit. Some of the first 'batteries' were made from dipping strips of zinc and copper into their salt solutions, but even a solution of acid works too. The electrode potential (V) is a measure of how easily a metal loses electrons. The more negative the potential the more easily the metal atoms lose electrons. The potential difference of the cell (p.d. in Volts) is the difference between the two electrode potentials of the two metals (shown in the table compared to hydrogen). Which statement is TRUE if copper and zinc metal electrodes are used? [mr-111]A simple battery cell can be made by connecting two metal strips dipped into a conducting solution of ions to form a complete circuit. Some of the first 'batteries' were made from dipping strips of zinc and copper into their salt solutions, but even a solution of acid works too. The electrode potential (V) is a measure of how easily a metal loses electrons. The more negative the potential the more easily the metal atoms lose electrons. The potential difference of the cell (p.d. in Volts) is the difference between the two electrode potentials of the two metals (shown in the table compared to hydrogen). Which statement is TRUE if copper and zinc metal electrodes are used? [mr-112]
The diagram shows the results of some sacrificial rust protection experiments. When silver is connected to iron, electrons transfer from iron to silver. This causes? [mr-113]The diagram shows the results of some sacrificial rust protection experiments. When zinc is connected to iron, electrons transfer from zinc to iron. This causes? [mr-114] If an iron sheet is dipped into a silver nitrate solution it becomes coated in grey layer of silver. The overall reaction is an example of? [mr-115] If an iron sheet is dipped into a copper sulphate solution it becomes coated in pink-brown deposit of copper. This formation of the copper is an example of? [mr-116]
Which of (1) - (5) represents where a blast of hot air is blown in? [me-1]Which of (1) - (5) represents where molten iron is tapped off? [me-2]Which of (1) - (5) represents where slag is removed? [me-3]Which of (1) - (5) represents where waste gases are removed? [me-4]Which of (1) - (5) represents where limestone is added? [me-5]Which of (1) - (5) represents where coke (carbon) is added? [me-6]
Why is limestone added to the blast furnace? [me-7]Iron is reduced in a blast furnace. This means? [me-8]Which reaction is causes the high temperature in a blast furnace? [me-9] In which reaction does an oxidation and a reduction produce the same product? [me-10]Which reaction represents the iron ore reduction in a blast furnace? [me-11]Which reaction removes solid acidic impurities from the iron produced in a blast furnace? [me-12]Which of these blast furnace reactions is the most exothermic? [me-13]Which reaction produces the molecule that reduces the iron ore to iron? [me-14]In which of these blast furnace reactions does one gas molecule get oxidised to another gas molecule? [me-15]Which of these blast furnace reactions forms the 'slag'? [me-16] | [me-17] The reactions in the blast furnace to produce iron are summarised by equations (1) to (4). The symbol equations may NOT be numerically balanced. ... (1) C + O2 ==> CO2 ... (2) CO2 + C ==> CO ... (3) Fe2O3 + CO ==> Fe + CO2 ... (4) CaCO3 + SiO2 ==> CaSiO3 + CO2 Which statement is TRUE? |
| [me-18] The reactions in the blast furnace to produce iron are summarised by equations (1) to (4). The symbol equations may NOT be numerically balanced. ... (1) C + O2 ==> CO2 ... (2) CO2 + C ==> CO ... (3) Fe2O3 + CO ==> Fe + CO2 ... (4) CaCO3 + SiO2 ==> CaSiO3 + CO2 Which statement is TRUE? |
| [me-19] The reactions in the blast furnace to produce iron are summarised by equations (1) to (4). The symbol equations may NOT be numerically balanced. ... (1) C + O2 ==> CO2 ... (2) CO2 + C ==> CO ... (3) Fe2O3 + CO ==> Fe + CO2 ... (4) CaCO3 + SiO2 ==> CaSiO3 + CO2 Which statement is TRUE? |
| [me-20] The reactions in the blast furnace to produce iron are summarised by equations (1) to (4). The symbol equations may NOT be numerically balanced. ... (1) C + O2 ==> CO2 ... (2) CO2 + C ==> CO ... (3) Fe2O3 + CO ==> Fe + CO2 ... (4) CaCO3 + SiO2 ==> CaSiO3 + CO2 Which statement is TRUE? |
| [me-21] The reactions in the blast furnace to produce iron are summarised by equations (1) to (4). The symbol equations may NOT be numerically balanced. ... (1) C + O2 ==> CO2 ... (2) CO2 + C ==> CO ... (3) Fe2O3 + CO ==> Fe + CO2 ... (4) CaCO3 + SiO2 ==> CaSiO3 + CO2 Which statement is TRUE? |
In the reactions in a blast furnace what happens to most of the carbon monoxide? [me-22]Oxidation of a substance can be defined as? [me-23]Reduction of a substance can be defined as? [me-24]
To produce aluminium, electricity is passed through? [me-31]To produce aluminium by electrolysis the the ore must be molten so that? [me-32]During the electrolysis of molten aluminium oxide ore, the aluminium ions move? [me-33]During the electrolysis of molten aluminium oxide ore, the oxide ions move? [me-34]In the extraction of aluminium by electrolysis of molten aluminium oxide ore, the ore is dissolved in cryolite to? [me-35]In the extraction of aluminium by electrolysis of its ore, the positive electrodes have to be regularly replaced because? [me-36] In the extraction of aluminium by the electrolysis of molten aluminium oxide ore, the aluminium forms? [me-37]In the extraction of aluminium by the electrolysis of molten aluminium oxide ore, oxygen forms? [me-38]The name of a common ore from which iron can be extracted is called? [me-39]The name of a common ore from which aluminium can be extracted is called? [me-40]The name of the substance used to lower the melting point of aluminium oxide ore in the electrolytic extraction of aluminium is called? [me-41]In the electrolysis of aluminium oxide to extract aluminium, the electrodes are made of? [me-42]
After the initial chemical extraction of copper from a copper ore, the copper is purified by? [me-51]After the initial chemical extraction of copper from a copper ore, the copper is purified by electrolysis. The negative electrode is made of? [me-52]After the initial chemical extraction of copper from a copper ore, the copper is purified by electrolysis. The positive electrode is made of? [me-53]After the initial chemical extraction of copper from a copper ore, the copper is purified by electrolysis. The electrolyte solution contains dissolved? [me-54]Which contains the iron oxide in the blast furnace extraction of iron? [me-63]Which is oxidised in the blast furnace extraction of iron? [me-64]Which removes impurities from iron in the blast furnace extraction of iron? [me-65]Which is NOT a raw material in the blast furnace extraction of iron? [me-66]
Which metals is obtained from bauxite ore? [me-67] Which metals is obtained from haematite ore? [me-68] Which metals is purified by electrolysis? [me-69] Which metals is most likely to be found as the element and not as an oxide or sulphide compound? [me-70] Which statement is TRUE? [me-71] Which statement is TRUE? [me-72] A mineral from which a metal can be extracted, is called? [me-73] Which is the reason why aluminium was first extracted commercially by electrolysis in the 19th century but metals like iron had been extracted for thousands of years? [me-74] Which metal is added to aluminium to make a stronger alloy? [me-77] Which metal is added to steel to give it good anti-corrosion properties? [me-78]
Which metal is found as the free element in the Earth's crust? [me-79]
| Stages in the extraction of iron in a blast furnace are described below after iron ore, coke and limestone have been added at the top, but not in the correct order. (1) carbon dioxide reacts with coke (carbon) to form carbon monoxide (2) limestone combines with acid impurities (3) hot air is blown into the furnace (4) carbon monoxide reacts with iron oxide to make iron (5) coke (carbon) burns to form carbon dioxide Which is the correct order of sequence for (1) to (5)? [me-86] |
Why is hot air blown into a blast furnace? [me-87] Which is formed on burning coke in the blast furnace? [me-88] Which removes the oxygen from the iron ore in a blast furnace? [me-89] Which is produced when limestone combines with acidic impurities in the blast furnace extraction of iron? [me-90] Which is added to a blast furnace to produce carbon monoxide and heat energy? [me-91]Haematite iron ore contains mainly? [me-92] Ingots of aluminium from its electrolytic extraction can be stored outside in all weathers. Why do aluminium ingots not corrode away, despite aluminium being quite high in the reactivity series of metals? [me-93] Which pair of elements are non-metals which will displace less reactive metals from their oxide ores? [me-94] Given the equation of the reduction of an iron oxide in a blast furnace: It is possible for an iron oxide ore in a blast furnace to be directly reduced by the coke (carbon) to form iron. It is possible for an iron oxide ore in a blast furnace to be directly reduced by the coke (carbon) to form iron. Iron oxide ore in a blast furnace is mainly reduced by carbon monoxide to form iron. Which is the correct and balanced equation for the formation of carbon monoxide in the blast furnace? [me-29] Given the equation of the reduction of an iron oxide in a blast furnace ... | In the extraction of aluminium by electrolysis of molten aluminium oxide, all the chemical changes occur on the surface of the electrodes. The formula for aluminium oxide is Al2O3. Which is the correct equation to show the change at the negative electrode? [me-43] |
| In the extraction of aluminium by electrolysis of molten aluminium oxide, all the chemical changes occur on the surface of the electrodes. The formula for aluminium oxide is Al2O3. Which is the correct equation to show the change at the positive electrode? [me-44] |
| In the extraction of aluminium by electrolysis of molten aluminium oxide, all the chemical changes occur on the surface of the electrodes. The formula for aluminium oxide is Al2O3. Which word describes the process happening on the surface of the positive electrode? [me-45] |
| In the extraction of aluminium by electrolysis of molten aluminium oxide, all the chemical changes occur on the surface of the electrodes. The formula for aluminium oxide is Al2O3. Which word describes the process happening on the surface of the negative electrode? [me-46] |
| Copper is purified by the electrolysis of copper(II) sulphate solution using copper electrodes. All the chemical changes occur on the surface of the electrodes. The formula for copper(II) sulphate is CuSO4. Which word describes the process happening on the surface of the positive electrode? [me-47] |
| Copper is purified by the electrolysis of copper(II) sulphate solution using copper electrodes. All the chemical changes occur on the surface of the electrodes. The formula for copper(II) sulphate is CuSO4. Which word describes the process happening on the surface of the negative electrode? [me-48] |
| Copper is purified by the electrolysis of copper(II) sulphate solution using copper electrodes. All the chemical changes occur on the surface of the electrodes. The formula for copper(II) sulphate is CuSO4. Which equation correctly describes the process happening on the surface of the positive electrode? [me-49] |
| Copper is purified by the electrolysis of copper(II) sulphate solution using copper electrodes. All the chemical changes occur on the surface of the electrodes. The formula for copper(II) sulphate is CuSO4. Which equation correctly describes the process happening on the surface of the negative electrode? [me-50] |
Which is TRUE about the extraction of aluminium by electrolysis? [me-75]Which is TRUE about the extraction of aluminium by electrolysis? [me-76]The diagram shows how copper is purified by electrolysis. What happens at the negative electrode? [me-95]The diagram shows how copper is purified by electrolysis. What happens at the positive electrode? [me-96]The diagram shows how copper is purified by electrolysis. Which is a suitable salt to use? [me-97]
Electrolysis processes can only be done on solutions or molten materials because? [me-98]In an electrolysis process which word describes the overall chemical change? [me-99]In an electrolysis process which word describes the change at the positive electrode? [me-100]In an electrolysis process which word describes the change at the negative electrode? [me-101]
Sodium and chlorine can be manufactured by passing a direct current through the molten salt sodium chloride. What happens at the negative electrode? [me-102]Sodium and chlorine can be manufactured by passing a direct current through the molten salt sodium chloride. What happens at the positive electrode? [me-103]Sodium and chlorine can be manufactured by passing a direct current through the molten salt sodium chloride. What happens to the sodium ions is an example of? [me-104]Sodium and chlorine can be manufactured by passing a direct current through the molten salt sodium chloride. What happens to the chloride ion is an example of? [me-105]