SASS Chem P1 Revision

Page 1 ST ANDREW’S SECONDARY SCHOOL NAME CLASS CHEMISTRY 6092/01 Paper 1 REVISION PACKAGE + MULTIPLE CHOICE QUESTIONS 1 2 3 4 © UCLES 2010 9791/01/M/J/10 9 The diagram represents the energy changes for some reactions. ∆H = –130 kJ mol–1 ∆H = –25 kJ mol–1 ∆H = +80 kJ mol–1 W Y X Z What are the natures of the conversions W → Y, Y → X and Z → W? W → Y Y → X Z → W A exothermic endothermic endothermic B exothermic exothermic endothermic C endothermic exothermic exothermic D endothermic endothermic exothermic 10 The diagram shows the energy profile for a reaction both with and without a catalyst present. What is the activation energy of the uncatalysed reverse reaction? energy reactants progress of reaction A B C D products 11 T h e m e t a l n i o b i u m , N b , h a s a r e l a t i v e a t o m i c m a s s o f 9 2 . 9 a n d i s u s e d i n v a r i o u s s t a i n l e s s s t e e l alloys. It is made by reducing niobium chloride with sodium. In this reaction, 54.08 g of niobium chloride produces 18.58 g of niobium. What is the formula of the niobium chloride used? A NbCl 2 B NbCl 3 C NbCl 4 D NbCl 5 4 4 © UCLES 2010 9791/01/M/J/10 9 The diagram represents the energy changes for some reactions. ∆H = –130 kJ mol–1 ∆H = –25 kJ mol–1 ∆H = +80 kJ mol–1 W Y X Z What are the natures of the conversions W → Y, Y → X and Z → W? W → Y Y → X Z → W A exothermic endothermic endothermic B exothermic exothermic endothermic C endothermic exothermic exothermic D endothermic endothermic exothermic 10 The diagram shows the energy profile for a reaction both with and without a catalyst present. What is the activation energy of the uncatalysed reverse reaction? energy reactants progress of reaction A B C D products 11 T h e m e t a l n i o b i u m , N b , h a s a r e l a t i v e a t o m i c m a s s o f 9 2 . 9 a n d i s u s e d i n v a r i o u s s t a i n l e s s s t e e l alloys. It is made by reducing niobium chloride with sodium. In this reaction, 54.08 g of niobium chloride produces 18.58 g of niobium. What is the formula of the niobium chloride used? A NbCl 2 B NbCl 3 C NbCl 4 D NbCl 5 4 12 © UCLES 2010 9791/01/M/J/10 33 1 2 . 5 cm3 of 0.0500 mol dm–3 sodium hydroxide is added to 25.0 cm3 of 0.100 mol dm–3 hydrochloric acid. Which concentration of hydrochloric acid remains in the reaction mixture? A 0 . 0 0 1 9 mol dm–3 B 0.0333 mol dm–3 C 0.0500 mol dm–3 D 0.0750 mol dm–3 34 Which mixture of gaseous oxygen and nitrogen would occupy 0.12 dm3 at room temperature and pressure? A 0 . 0 3 2 g O2 and 0.084 g N2 B 0 . 0 9 6 g O2 and 0.028 g N2 C 0 . 0 9 6 g O2 and 0.056 g N2 D 0.096 g O2 and 0.084 g N2 35 The mass spectrum of CH2F2 would not contain a peak at which m / z value? A 14 B 19 C 38 D 52 36 In the absence of reference spectra, infra-red spectroscopy can most easily be used to distinguish between A 1-chloropropane and 1-bromopropane. B cis but-2-ene and trans but-2-ene. C ethanol and ethanal. D propan-2-ol and propan-1-ol. 12

Page 2 4 5 6 7 8 9 6 © UCLES 2010 9791/01/M/J/10 14 Four compounds of period 3 elements are listed. Na2O SiC l 4 SO 2 N a C l Water is added to each of the four compounds. Pairs of the resulting solutions are mixed together. From which pair of solutions is it possible to get a solution with a pH of 7? A N a Cl and Na2O B N a Cl and SO2 C Na2O and SiCl 4 D SiCl 4 and SO2 15 In Group 2, what are the trends in charge density of the metal cations and thermal stability of the metal carbonates as the atomic number of the metal increases? charge density thermal stability A decreases decreases B decreases increases C increases decreases D increases increases 16 The diagram shows bond energies in halogen molecules. 300 250 200 150 100 50 0 bond energy / kJ mol–1 period 2 3 4 5 F2 Br2 I2 Cl2 Why does the value for fluorine not follow the trend shown by chlorine, bromine and iodine? A Fluorine is more electronegative than the other halogens. B Lone electron pairs in fluorine repel more strongly than those in the other halogens. C The bonds in fluorine are more polar than those in the other halogens. D The bonds in fluorine have some π-character. 6 12 © UCLES 2010 9791/01/M/J/10 33 1 2 . 5 cm3 of 0.0500 mol dm–3 sodium hydroxide is added to 25.0 cm3 of 0.100 mol dm–3 hydrochloric acid. Which concentration of hydrochloric acid remains in the reaction mixture? A 0 . 0 0 1 9 mol dm–3 B 0.0333 mol dm–3 C 0.0500 mol dm–3 D 0.0750 mol dm–3 34 Which mixture of gaseous oxygen and nitrogen would occupy 0.12 dm3 at room temperature and pressure? A 0 . 0 3 2 g O2 and 0.084 g N2 B 0 . 0 9 6 g O2 and 0.028 g N2 C 0 . 0 9 6 g O2 and 0.056 g N2 D 0.096 g O2 and 0.084 g N2 35 The mass spectrum of CH2F2 would not contain a peak at which m / z value? A 14 B 19 C 38 D 52 36 In the absence of reference spectra, infra-red spectroscopy can most easily be used to distinguish between A 1-chloropropane and 1-bromopropane. B cis but-2-ene and trans but-2-ene. C ethanol and ethanal. D propan-2-ol and propan-1-ol. 12 2 © UCLES 2011 9791/01/M/J/11 1 The table shows the successive ionisation energies for an element Q. 1 s t 2 n d 3 r d 4 t h ionisation energy / kJ mol–1 4 1 8 3 0 7 0 4 6 0 0 5 8 6 0 What is the likely formula of the oxide of Q? A QO B Q3O2 C Q2O D Q2O3 2 How many neutrons are present in 0.13 g of 13C? [L = the Avogadro constant] A 0.06 L B 0.07 L C 0.13 L D 0 . 9 1 L 3 Phosphorus sulfide, P4S3, is used in small amounts in the tips of matches. On striking a match this compound burns to produce an oxide of phosphorus in the +5 oxidation state and an oxide of sulfur in the +4 oxidation state. How many moles of oxygen gas are needed to burn one mole of P4S3 in this way? A 6 B 7 . 5 C 8 D 1 6 4 F o u r e l e m e n t s , W , X , Y a n d Z , a r e i n t h e p o tassium to krypton period with consecutive atomic numbers. The table shows the number of unpaired electrons in each atom in its ground state. element W X Y Z unpaired electrons 2 1 0 1 In which group of the Periodic Table is element W? A 4 B 10 C 14 D 16 5 When the N2 + ion is formed from N2 a σ bonding electron is removed. Which statement is correct? A The bond order decreases so N2 + has a stronger, shorter bond than N2. B The bond order decreases so N2 + has a weaker, longer bond than N2. C The bond order increases so N2 + has a stronger, shorter bond than N2. D The bond order increases so N2 + has a weaker, longer bond than N2. 18 2 © UCLES 2011 9791/01/M/J/11 1 The table shows the successive ionisation energies for an element Q. 1 s t 2 n d 3 r d 4 t h ionisation energy / kJ mol–1 4 1 8 3 0 7 0 4 6 0 0 5 8 6 0 What is the likely formula of the oxide of Q? A QO B Q3O2 C Q2O D Q2O3 2 How many neutrons are present in 0.13 g of 13C? [L = the Avogadro constant] A 0.06 L B 0.07 L C 0.13 L D 0 . 9 1 L 3 Phosphorus sulfide, P4S3, is used in small amounts in the tips of matches. On striking a match this compound burns to produce an oxide of phosphorus in the +5 oxidation state and an oxide of sulfur in the +4 oxidation state. How many moles of oxygen gas are needed to burn one mole of P4S3 in this way? A 6 B 7 . 5 C 8 D 1 6 4 F o u r e l e m e n t s , W , X , Y a n d Z , a r e i n t h e p o tassium to krypton period with consecutive atomic numbers. The table shows the number of unpaired electrons in each atom in its ground state. element W X Y Z unpaired electrons 2 1 0 1 In which group of the Periodic Table is element W? A 4 B 10 C 14 D 16 5 When the N2 + ion is formed from N2 a σ bonding electron is removed. Which state