9701_s15_qp_22
A paper of Chemistry, 9701
Questions:
4
Year:
2015
Paper:
2
Variant:
2
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1
Chemists recognise that atoms are made of three types of particle. Complete the following table with their names and properties. name of particle relative mass relative charge +1 1/1836 Most elements exist naturally as a mixture of isotopes, each with their own relative isotopic mass. The mass spectrum of an element reveals the abundances of these isotopes, which can be used to calculate the relative atomic mass of the element. Magnesium has three stable isotopes. Information about two of these isotopes is given. isotope relative isotopic mass percentage abundance 24Mg 24.0 79.0 26Mg 26.0 11.0 Defi ne the term relative isotopic mass. The relative atomic mass of magnesium is 24.3. Calculate the percentage abundance and hence the relative isotopic mass of the third isotope of magnesium. Give your answer to three signifi cant fi gures percentage abundance = isotopic mass = Magnesium can be produced by electrolysis of magnesium chloride in a molten mixture of salts. Give equations for the anode and cathode reactions during the electrolysis of molten magnesium chloride, MgCl 2. anode cathode The electrolysis is carried out under an atmosphere of hydrogen chloride gas to convert any magnesium oxide impurity into magnesium chloride. An investigation of the reaction between magnesium oxide and hydrogen chloride gas showed that an intermediate product was formed with the composition by mass Mg, 31.65%; O, 20.84%; H, 1.31% and Cl, 46.20%. Calculate the empirical formula of this intermediate compound. empirical formula The acid/base behaviour of the oxides in the third period varies across the period. Describe this behaviour and explain it with reference to the structure and bonding of sodium oxide, Na2O, aluminium oxide, Al 2O3, and sulfur trioxide, SO3. Write equations for reactions of these three oxides with hydrochloric acid and/or sodium hydroxide as appropriate.
10. Group 2  →  10.1. Similarities and trends in the properties of the Group 2 metals, magnesium to barium, and their compounds
2. Atoms, molecules and stoichiometry  →  2.1. Relative masses of atoms and molecules
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2
Sulfuric acid is an important chemical with a variety of uses. It is manufactured by the Contact process, the fi rst stage of which involves the conversion of sulfur or a sulfi de ore, such as galena, PbS, into sulfur dioxide, SO2. Write an equation for the reaction between galena and oxygen to form sulfur dioxide and lead(oxide. Identify the oxidation number changes that take place during this reaction. The second stage of the Contact process involves the production of sulfur trioxide, SO3, from sulfur dioxide. 2SO2+ O22SO3∆H = –197 kJ mol–1 State the temperature usually chosen for this conversion and explain this in terms of reaction rates and Le Chatelier’s principle. temperature explanation State and explain the pressure conditions that would give the best rate and best yield of sulfur trioxide. Explain why these conditions are not actually used. In the third stage of the process the sulfur trioxide is dissolved in 98% sulfuric acid followed by carefully controlled addition of water. Explain why the sulfur trioxide is not dissolved directly in water to produce sulfuric acid. Write equations for the reaction of sulfur trioxide with sulfuric acid and for the subsequent reaction with water. Explain why sulfur dioxide is used as an additive in some foods and wines. The sulfur dioxide content of wine is most commonly measured by the Ripper Method which involves titration with iodine in the presence of starch as an indicator. SO2+ I2+ 2H2O→ 2I –+ SO4 2–+ 4H+A 50.0 cm3 sample of wine required 12.35 cm3 of 0.010 mol dm–3 I2for complete reaction with the SO2. How many moles of SO2 are present in 50.0 cm3 of wine? moles of SO2 in 50.0 cm3 = How many moles of SO2 are present in 1 dm3 of wine? moles of SO2 in 1 dm3 = How many milligrams, mg, of SO2 are present in 1 dm3 of wine? Give your answer to three signifi cant fi gures. (1 g = 1000 mg) mass of SO2 in 1 dm3 = mg
12. Nitrogen and sulfur  →  12.1. Nitrogen and sulfur
11. Group 17  →  11.4. The reactions of chlorine
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Ethane reacts with chlorine to form chloroethane. C2H6+ Cl 2→ C2H5Cl + HCl Use bond energies from the Data Booklet to calculate the enthalpy change for this reaction. Include a sign in your answer. enthalpy change = kJ mol–1 State the conditions needed for this reaction to occur. Use a series of equations to describe the mechanism of this reaction including the names of each stage and an indication of how butane can be produced as a minor by-product. Chloroethane can be converted back into ethane by a two-stage process via an intermediate compound, X. C2H5Cl C2H6 X reaction 1 reaction 2 Give the name of X. Suggest the reagent and conditions needed for reaction 1. Suggest the reagent and conditions needed for reaction 2.
5. Chemical energetics  →  5.1. Enthalpy change, \(\Delta H\)
14. Hydrocarbons  →  14.1. Alkanes
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There are seven structural isomers with the molecular formula C5H10O that are carbonyl compounds. Four of these are aldehydes. These four aldehydes, A, B, C and D, have the following properties. ● Aldehyde A has a straight chain while B, C and D are branched. ● Aldehyde B is the only one of the four isomers with a chiral centre and it exists as a pair of optical isomers. ● Aldehyde C has two methyl groups in its structure but D has three. Give the structure of each of the four isomers. A B C D Draw the three-dimensional structures of the two optical isomers of B. Describe a chemical test that would allow you to distinguish between any of the four isomers A to D and any of the other three structural isomers of C5H10O, that are carbonyl compounds. In your answer you should describe any necessary reagents and conditions as well as explaining what you would see in each case. Describe a test that would give the same result with all seven carbonyl isomers of C5H10O.
13. An introduction to AS Level organic chemistry  →  13.4. Isomerism: structural isomerism and stereoisomerism
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