9.4. Reactivity series
A subsection of Chemistry, 0620, through 9. Metals
Listing 10 of 452 questions
The table shows some properties of cobalt, copper, magnesium and tin. metal relative heat conduction density in g / cm3 melting point / °C relative strength cobalt 1.00 8.90 55.0 copper 3.85 8.92 32.0 magnesium 1.50 1.74 1.5 tin 0.64 7.28 1.0 Answer the questions using the information shown in the table. Which metal is the best to use for the base of a pan for cooking food? Use information in the table to give reasons for your answer. Which two metals in the table are transition elements? Use information in the table to give reasons for your answer. Which metal in the table is most likely to be used in an alloy for aircraft bodies? Use information in the table to give reasons for your answer. Some observations about the reactions of the four metals with hydrochloric acid are shown in the table. metal observations cobalt Bubbles formed very slowly. copper No bubbles formed. magnesium Many bubbles formed very rapidly. tin A steady stream of bubbles formed. Use the information in the table to put these metals in order of their reactivity with hydrochloric acid. least reactive most reactive Crystals of hydrated cobalt(sulfate, CoSO4.7H2O, can be made by reacting dilute sulfuric acid with insoluble cobalt carbonate. Describe how you could prepare a pure dry sample of cobalt(sulfate crystals from dilute sulfuric acid and cobalt(carbonate. When heated, hydrated cobalt(sulfate forms an anhydrous salt in a reversible reaction. Complete the equation for this reaction by inserting the sign for a reversible reaction in the box. CoSO4.7H2O hydrated cobalt(sulfate pale red CoSO4 anhydrous cobalt(sulfate dark blue + 7H2O Suggest how you could use this reaction to test for the presence of water.
0620_m16_qp_32
THEORY
2016
Paper 3, Variant 2
View
Iron pyrite, FeS2, is known as Fool’s Gold because it is a shiny yellow solid which is similar in appearance to gold. Iron pyrite is an ionic compound. Gold is a metallic element. Iron pyrite, FeS2, contains positive and negative ions. The positive ion is Fe2+. Deduce the formula of the negative ion. A student is provided with a sample of iron pyrite and a sample of gold. Suggest how the student could distinguish between the two substances. Sulfur dioxide is produced on a large scale by heating iron pyrite strongly in air. The iron pyrite reacts with oxygen in the air producing iron(oxide, Fe2O3, and sulfur dioxide. Construct a chemical equation for the reaction between iron pyrite and oxygen. Give one use of sulfur dioxide.
0620_m16_qp_42
THEORY
2016
Paper 4, Variant 2
View
Silver dichromate, Ag2Cr2O7, is a red insoluble salt. Silver dichromate can be made by reacting silver nitrate solution with ammonium dichromate solution. The chemical equation for the reaction is shown. 2AgNO3+ (NH4)2Cr2O72NH4NO3+ Ag2Cr2O7Describe how you could obtain pure dry solid silver dichromate after mixing silver nitrate solution and ammonium dichromate solution. The charge on a silver ion is +1. Deduce the charge on the dichromate ion in Ag2Cr2O7. Write the ionic equation for the formation of silver dichromate in this reaction. State symbols are not required. Dilute aqueous sodium hydroxide was added to the ammonium nitrate solution made in the reaction. The mixture was then warmed and damp Universal Indicator paper was held above the mixture. State and explain what would happen to the Universal Indicator paper. The apparatus shown was set up. solid silver nitrate solid ammonium dichromate plastic trough water S After five minutes, a red solid appeared along the line marked S on the diagram. Explain why a red solid appeared along the line marked S. The experiment was repeated at a higher temperature. What effect, if any, would this have on the time taken for the red solid to appear? Explain your answer. Ammonium dichromate, (NH4)2Cr2O7, undergoes thermal decomposition. The products are chromium(oxide, nitrogen and water. What is meant by thermal decomposition? Write a chemical equation for the thermal decomposition of ammonium dichromate.
0620_m17_qp_42
THEORY
2017
Paper 4, Variant 2
View
Titanium is extracted from an ore called rutile. Rutile is an impure form of titanium(oxide, TiO2. Rutile is mixed with coke and heated in a furnace through which chlorine gas is passed. The product is gaseous titanium(chloride, TiCl 4. TiO2+ 2C+ 2Cl 2TiCl 4+ 2COThe gaseous titanium(chloride produced is condensed into the liquid state. The titanium(chloride is then separated from liquid impurities. Suggest the name of the process by which liquid titanium(chloride could be separated from the liquid impurities. Carbon monoxide, CO, is also produced in the reaction. Why should carbon monoxide not be released into the atmosphere? Calculate the volume of chlorine gas, Cl 2, at room temperature and pressure, that reacts completely with 400 g of TiO2using the following steps. TiO2+ 2Cl 2+ 2CTiCl 4+ 2CO● ● Calculate the relative formula mass, Mr, of TiO2.  Mr of TiO2 = ● ● Calculate the number of moles in 400 g of TiO2.  mol ● ● Determine the number of moles of Cl 2 that react with 400 g of TiO2.  moles of Cl 2 = mol ● ● Calculate the volume of Cl 2 that reacts with 400 g of TiO2.  volume of Cl 2 = dm3  Titanium(chloride, TiCl 4, is heated with an excess of magnesium, in an atmosphere of argon. Balance the chemical equation for the reaction. TiCl 4 + Mg Ti + MgCl 2  Titanium(chloride can be reacted with sodium instead of magnesium. The reaction between titanium(chloride and sodium is similar to the reaction between titanium(chloride and magnesium. Write a chemical equation for the reaction between titanium(chloride and sodium. Suggest why the reaction between titanium(chloride and magnesium is done in an atmosphere of argon and not in air. After titanium(chloride is heated with magnesium, the unreacted magnesium is removed by adding an excess of dilute hydrochloric acid to the mixture. The dilute hydrochloricacid also dissolves the magnesiumchloride. The dilute hydrochloricacid does not react with the titanium or dissolve it. Give two observations and write a chemical equation for the reaction that occurs when dilute hydrochloric acid reacts with magnesium. chemical equation  Name the process that is used to separate the titanium from the mixture after all the magnesium has been removed. Titanium does not react with the dilute hydrochloric acid or dissolve in it. Suggest why titanium does not react with dilute hydrochloric acid. Magnesium cannot be produced by electrolysis of aqueous magnesium chloride using inert electrodes. Name the product formed at the negative electrode during the electrolysis of aqueous magnesium chloride. Suggest how magnesium can be produced from magnesium chloride by electrolysis. 
0620_m19_qp_42
THEORY
2019
Paper 4, Variant 2
View
Water is essential for many industrial processes. State one use of water in industry. What is the pH of pure water? Draw a circle around the correct answer. pH 0 pH 6 pH 7 pH 14 Filtration and chlorination are two of the steps used in water treatment. Describe the purpose of each of these steps. filtration chlorination  The changes of state of water are shown. water ice steam A freezing B boiling Give the names of the changes of state represented by A and B. A B  The table compares the reactions of four metals with both steam and dilute hydrochloricacid. metal reaction with steam at 200 °C observation with dilute hydrochloric acid copper no reaction no bubbles formed magnesium rapid reaction bubbles form rapidly nickel no reaction bubbles form slowly zinc rapid reaction bubbles form slowly Put the four metals in order of their reactivity. Put the least reactive metal first. least reactive most reactive  
0620_m20_qp_32
THEORY
2020
Paper 3, Variant 2
View
Questions Discovered
452