5. 5 dm 3 of carbon monoxide, CO (g), and 2 dm 3 of oxygen, O 2. Turn over

Transcription

1 3 M09/4/CEMI/SPM/ENG/TZ1/XX+ 4 M09/4/CEMI/SPM/ENG/TZ1/XX+ 1. The molar mass of a compound is approximately 56 g mol 1. Which formula is possible for this compound? A. NaNO 3 B. AgO C. MgO D. KO 4. What is the maximum mass, in g, of magnesium oxide that can be obtained from the reaction of oxygen with.4 g of magnesium? A..4 B. 3.0 C. 4.0 D Which compound has the empirical formula with the largest mass? A. C 6 B. C 4 C. C D. C dm 3 of carbon monoxide, CO (g), and dm 3 of oxygen, O (g), at the same temperature and pressure are mixed together. Assuming complete reaction according to the equation given, what is the maximum volume of carbon dioxide, CO (g), in dm 3, that can be formed? A. 3 B. 4 CO( g) O ( g) CO ( g) C What is the coefficient for O (g) when the equation for the combustion of 1 mole of pentane is balanced? D. 7 A. 5 B. 6 C. 8 D. 16 C 5 1(g) _O (g) _CO (g) _O(g) 6. Which statement about solutions is correct? A. When vitamin D dissolves in fat, vitamin D is the solvent and fat is the solute. B. In a solution of NaCl in water, NaCl is the solute and water is the solvent. C. An aqueous solution consists of water dissolved in a solute. D. The concentration of a solution is the amount of solvent dissolved in 1 dm 3 of solution

2 5 M09/4/CEMI/SPM/ENG/TZ1/XX+ 6 M09/4/CEMI/SPM/ENG/TZ1/XX+ 7. ow many protons, neutrons and electrons are present in each atom of 31 P? Protons Neutrons Electrons A B C Which is the best definition of electronegativity? A. Electronegativity is the energy required for a gaseous atom to gain an electron. B. Electronegativity is the attraction of an atom for a bonding pair of electrons. C. Electronegativity is the attraction between the nucleus and the valence electrons of an atom. D. Electronegativity is the ability of an atom to attract electrons from another atom. D What are the correct formulas of the following ions? 8. Which is correct for the following regions of the electromagnetic spectrum? Ammonium ydrogencarbonate Phosphate Ultraviolet (UV) Infrared (IR) A. N 4 CO 3 PO 4 A. high energy short wavelength low energy low frequency B. N 3 CO 3 PO 4 3 B. high energy low frequency low energy long wavelength C. N 4 CO 3 PO 4 C. high frequency short wavelength high energy long wavelength D. high frequency long wavelength low frequency low energy D. N 4 CO 3 PO An element is in group 4 and period 3 of the periodic table. ow many electrons are in the highest occupied energy level of an atom of this element? A. 3 B. 4 C What happens when magnesium metal reacts with chlorine gas? A. Each magnesium atom loses two electrons and each chlorine atom gains two electrons. B. Each magnesium atom gains one electron and each chlorine atom loses one electron. C. Each magnesium atom loses two electrons and each chlorine atom gains one electron. D. Each magnesium atom gains one electron and each chlorine atom loses two electrons. D Which is the best description of ionic bonding? A. The electrostatic attraction between positively charged nuclei and an electron pair B. The electrostatic attraction between positive ions and delocalized negative ions C. The electrostatic attraction between positive ions and delocalized electrons D. The electrostatic attraction between oppositely charged ions

3 7 M09/4/CEMI/SPM/ENG/TZ1/XX+ 8 M09/4/CEMI/SPM/ENG/TZ1/XX+ 14. Which is the best description of the bonding present in silicon dioxide, SiO? A. Each silicon atom forms four single covalent bonds to oxygen atoms. B. Each silicon atom forms two double covalent bonds to oxygen atoms. C. Each silicon atom forms two single covalent bonds to oxygen atoms. D. Each silicon atom forms four double covalent bonds to oxygen atoms. 15. When some solid barium hydroxide and solid ammonium thiosulfate were reacted together, the temperature of the surroundings was observed to decrease from 15 ºC to 4 ºC. What can be deduced from this observation? A. The reaction is exothermic and ë is negative. B. The reaction is exothermic and ë is positive. C. The reaction is endothermic and ë is negative. D. The reaction is endothermic and ë is positive. 16. Which process represents the C Cl bond enthalpy in tetrachloromethane? A. CCl ( g) C( g) + Clg ( ) 4 4 B. CCl ( g) CCl ( g) + Clg ( ) 4 3 C. CCl () l C( g) + Clg ( ) 4 4 D. CCl () l C() s + Cl ( g) Some water is heated using the heat produced by the combustion of magnesium metal. Which values are needed to calculate the enthalpy change of reaction? I. The mass of magnesium II. III. The mass of the water The change in temperature of the water 18. What is the best definition of rate of reaction? A. The time it takes to use up all the reactants B. The rate at which all the reactants are used up C. The time it takes for one of the reactants to be used up D. The increase in concentration of a product per unit time 19. Which factors can affect reaction rate? I. The state of the reactants II. III. The frequency of the collisions between particles The average kinetic energy of the particles

4 9 M09/4/CEMI/SPM/ENG/TZ1/XX+ 10 M09/4/CEMI/SPM/ENG/TZ1/XX+ 0. Equal masses of powdered calcium carbonate were added to separate solutions of hydrochloric acid. The calcium carbonate was in excess. The volume of carbon dioxide produced was measured at regular intervals. Which curves best represent the evolution of carbon dioxide against time for the acid solutions shown in the table below. Volume of CO (g) / cm 3 I. For equal volumes of 1.0 mol dm 3 solutions of hydrochloric acid, Cl (aq), and methanoic acid, COO (aq), which statements are correct? I. Cl dissociates more than COO II. III. Cl is a better electrical conductor than COO Cl will neutralize more NaO than COO II IV III Time / s 5 cm 3 of mol dm 3 Cl 50 cm 3 of 1 mol dm 3 Cl 5 cm 3 of 1 mol dm 3 Cl A. I III IV B. I IV III C. I II III D. II I III 1. Consider the following equilibrium reaction. SO (g) O(g) SO (g) ë Ö = 197 kj 3 Which change in conditions will increase the amount of SO 3 present when equilibrium is re-established? A. Decreasing the concentration of SO 3. When equal volumes of four 0.1 mol dm 3 solutions are arranged in order of increasing p (lowest p first), what is the correct order? A. C 3 COO < NO 3 < C 3 C N < KO B. NO 3 < C 3 COO < C 3 C N < KO C. C 3 C N < NO 3 < C 3 COO < KO D. KO < C 3 C N < C 3 COO < NO 3 4. What happens at the negative electrode in a voltaic cell and in an electrolytic cell? Voltaic cell Electrolytic cell A. oxidation reduction B. reduction oxidation C. oxidation oxidation D. reduction reduction B. Increasing the volume C. Decreasing the temperature D. Adding a catalyst

5 11 M09/4/CEMI/SPM/ENG/TZ1/XX+ 1 M09/4/CEMI/SPM/ENG/TZ1/XX+ 5. Consider how current is conducted in an electrolytic cell. Which statement is correct? A. Electrons move through the electrolyte and the external circuit. B. Ions move through the electrolyte and the external circuit. C. Electrons move through the external circuit and ions move through the electrolyte. D. Electrons move through the electrolyte and ions move through the external circuit. 9. Which conditions are required to obtain a good yield of a carboxylic acid when ethanol is oxidized using potassium dichromate(vi), K Cr O 7 (aq)? I. Add sulfuric acid II. III. eat the reaction mixture under reflux Distil the product as the oxidizing agent is added 6. Which three compounds can be considered to be a homologous series? A. C 3 O, C 3 C O, C 3 C C O B. C 3 C O, C 3 CO, C 3 COO C. C 3 C C(O)C 3, C 3 C C C O, (C 3 ) 3 CO D. C 3 C C C O, C 3 C OC C 3, (C 3 ) C CO 7. What is the IUPAC name for C 3 C C(C 3 )C 3? A. 1,1-dimethylpropane B. -ethylpropane 30. A student recorded the volume of a gas as dm 3. ow many significant figures are there in this value? A. 3 B. 4 C. 5 D. 6 C. -methylbutane D. 3-methylbutane 8. When bromine water is shaken with a liquid organic compound, it is rapidly decolourized. What can be determined from this test? A. The compound is an alcohol. B. The compound is an alkane. C. The compound is an alkene. D. The compound is an iodoalkane

6 3 M10/4/CEMI/SPM/ENG/TZ1/XX+ 4 M10/4/CEMI/SPM/ENG/TZ1/XX+ 1. Which amount of the following compounds contains the least number of ions? A. mol of NaO B. 1 mol of N 4 Cl C. mol of CaCl D. 1 mol of Al O molecules of hydrogen gas, (g), and 5 molecules of oxygen gas, O (g), were mixed together under conditions which allowed the reaction to go to completion, according to the following equation. (g) O (g) O(g) The following diagram represents the mixture of reactants. Key: Oxygen atom. What is the approximate molar mass, in g mol 1, of MgSO4i7 O? A. 10 B. 130 C. 138 Which diagram represents the reaction mixture when the reaction was complete? A. ydrogen atom D Which is both an empirical and a molecular formula? B. A. C 5 1 B. C 5 10 C. C 4 8 D. C 4 10 C. D

7 5 5. Which of the following is an isotope of 4 1 Mg? A. 4 1Mg + B. 6 1Mg C. 4 13Mg D. 6 13Mg 6. Which describes the visible emission spectrum of hydrogen? A. A series of lines converging at longer wavelength B. A series of regularly spaced lines C. A series of lines converging at lower energy D. A series of lines converging at higher frequency M10/4/CEMI/SPM/ENG/TZ1/XX+ 6 M10/4/CEMI/SPM/ENG/TZ1/XX+ 8. Which statements about period 3 are correct? I. The electronegativity of the elements increases across period 3. II. The atomic radii of the elements decreases across period 3. III. The oxides of the elements change from acidic to basic across period Which is the best description of the bonding present in the ammonium ion, N + 4? A. Sharing of electrons between atoms B. Electrostatic attraction between ions C. Electrostatic attraction between positive ions and delocalized electrons 7. Which statements about the periodic table are correct? I. Elements in period 3 have similar chemical properties. II. III. Elements in group 7 show a gradual change in physical properties. The position of an element in period 3 is related to the number of electrons in the highest occupied energy level. D. Sharing of electrons between atoms and electrostatic attraction between ions 10. The formula of cerium(iii) sulfate is Ce (SO 4 ) 3. What is the correct formula of cerium(iii) phosphate? A. CeP B. Ce (PO 4 ) 3 C. Ce 3 (PO 4 ) D. CePO

8 7 11. Which molecule has the shortest carbon-oxygen bond length? A. C 3 COO B. C 3 C O C. CO D. CO M10/4/CEMI/SPM/ENG/TZ1/XX+ 8 M10/4/CEMI/SPM/ENG/TZ1/XX+ 15. Which types of reaction are always exothermic? I. Neutralization II. Decomposition III. Combustion 1. Which pair of compounds is arranged in correct order of relative boiling points? Lower Boiling Point igher Boiling Point A. S O B. N 3 P 3 C. F Cl D. C 3 COO C 3 C O 13. Which statement about the bonding between carbon atoms is correct? 16. A pure aluminium block with a mass of 10 g is heated so that its temperature increases from 0 C to C. The specific heat capacity of aluminium is Jg K. Which expression gives the heat energy change in kj? A B C A. In C 60 fullerene each carbon atom is covalently bonded to three other carbon atoms. B. In C 60 fullerene each carbon atom is covalently bonded to four other carbon atoms. D C. In graphite each carbon atom is covalently bonded to four other carbon atoms. D. In graphite each carbon atom forms a double covalent bond with three other carbon atoms. 14. Which intermolecular forces exist between molecules of carbon monoxide, CO? A. ydrogen bonds and van der Waals forces B. Dipole-dipole attractions and van der Waals forces C. Van der Waals forces only 17. Under which conditions will the reaction between 1.0 g calcium carbonate and excess hydrochloric acid be the fastest? Assume that all reactions are carried out at the same temperature. A. One large piece of calcium carbonate and mol dm 3 hydrochloric acid B. One large piece of calcium carbonate and 1 mol dm 3 hydrochloric acid C. Powdered calcium carbonate and mol dm 3 hydrochloric acid D. Powdered calcium carbonate and 1 mol dm 3 hydrochloric acid D. Dipole-dipole attractions only

9 9 M10/4/CEMI/SPM/ENG/TZ1/XX+ 10 M10/4/CEMI/SPM/ENG/TZ1/XX+ 18. Powdered manganese(iv) oxide, MnO (s), increases the rate of the decomposition reaction of hydrogen peroxide, O (aq). Which statements about MnO are correct? I. The rate is independent of the particle size of MnO. II. III. MnO provides an alternative reaction pathway for the decomposition with a lower activation energy. All the MnO is present after the decomposition of the hydrogen peroxide is complete. 19. Which statement is correct for a crystal of iron(ii) sulfate in a state of equilibrium with a saturated solution of iron(ii) sulfate? stopper flask iron(ii) sulfate solution iron(ii) sulfate crystal A. The colour of the solution darkens as the crystal continues to dissolve. 0. The aber process uses an iron catalyst to convert hydrogen gas, (g), and nitrogen gas, N (g), to ammonia gas, N 3 (g). 3 (g) N (g) N (g) 3 Which statements are correct for this equilibrium system? I. The iron catalyst increases the rates of the forward and reverse reactions equally. II. The iron catalyst does not affect the value of the equilibrium constant, K c. III. The iron catalyst increases the yield of ammonia gas, N 3 (g). 1. Which property is characteristic of acids in aqueous solution? A. Acids react with ammonia solution to produce hydrogen gas and a salt. B. Acids react with metal oxides to produce oxygen gas, a salt and water. C. Acids react with reactive metals to produce hydrogen gas and a salt. D. Acids react with metal carbonates to produce hydrogen gas, a salt and water. B. The concentration of the iron(ii) sulfate solution increases as the water evaporates. C. The shape of the iron(ii) sulfate crystal does not change. D. The colour of the solution does not change but the shape of the crystal may change.. A student has equal volumes of 1.0 mol dm 3 sodium hydroxide and ammonia solutions. Which statement about the solutions is correct? A. Sodium hydroxide has a lower electrical conductivity than ammonia. B. Sodium hydroxide has a higher hydrogen ion concentration than ammonia. C. Sodium hydroxide has a higher p than ammonia. D. Sodium hydroxide has a higher hydroxide ion concentration than ammonia

10 11 M10/4/CEMI/SPM/ENG/TZ1/XX+ 1 M10/4/CEMI/SPM/ENG/TZ1/XX+ 3. Which definition of oxidation is correct? A. Loss of electrons and a decrease in oxidation number B. Loss of electrons and an increase in oxidation number C. Gain of electrons and a decrease in oxidation number D. Gain of electrons and an increase in oxidation number 6. Which is the best definition of structural isomers? A. Compounds which have atoms with the same atomic numbers but different mass numbers B. Compounds which have the same general formula but differ by a C group C. Compounds which have the same empirical formula but different molecular formulas D. Compounds which have the same molecular formula but different arrangements of atoms 4. What is the IUPAC name of Fe O 3? 7. Which is the correct classification of these alcohols? A. Iron oxide B. Iron(II) oxide C C C C C C C C C C. Iron(III) oxide D. Di-iron trioxide C C C O C C O O C 5. Which labels of the electrolytic cell are correct? Pt Pt KBr (l) 3 crucible A. tertiary secondary primary B. tertiary primary secondary C. tertiary tertiary secondary D. secondary primary secondary 8. Which substances are possible products of the incomplete combustion of octane? A. site of reduction site of oxidation conductor electrolyte B. site of oxidation site of reduction electrolyte conductor C. site of reduction site of oxidation electrolyte conductor D. site of oxidation site of reduction conductor electrolyte A. Carbon dioxide and hydrogen gas B. Carbon monoxide and water vapour C. Carbon monoxide and hydrogen gas D. Methane and hydrogen gas

11 13 M10/4/CEMI/SPM/ENG/TZ1/XX+ 3 M10/4/CEMI/SPM/ENG/TZ/XX+ 9. Which structure could represent a repeating unit of a polymer formed from propene? A. ( C C(C 3 ) B. ( C C C ( ( ( C. ( C(C 3 ) C(C 3 ) D. ( C C ( 30. Which experimental procedure is most likely to lead to a large systematic error? A. Determining the concentration of an alkali by titration with a burette B. Measuring the volume of a solution using a volumetric pipette C. Determining the enthalpy change of neutralization in a beaker D. Measuring the volume of a gas produced with a gas syringe 1. What is the coefficient of Fe 3 O 4 when the following equation is balanced using the lowest whole numbers? A. B. 3 C. 4 D. 5 Al(s) Fe O ( s) Al O ( s) Fe(s) What is the mass, in g, of one molecule of ethane, C 6? A B C. 30 D Which molecular formula is also an empirical formula? A. PCl 3 B. C 4 C. O D. C 6 1 O 6 4. Which of the following is consistent with Avogadro s law? A. B. P constant (V, n constant) T V constant (P, n constant) T C. V n constant (P, T constant) D. V constant (P, T constant) n

12 4 M10/4/CEMI/SPM/ENG/TZ/XX+ 5 M10/4/CEMI/SPM/ENG/TZ/XX+ 5. A sample of element X contains 69 % of 63 X and 31 % of 65 X. What is the relative atomic mass of X in this sample? A B C D Which oxides produce an acidic solution when added to water? I. P 4 O 10 II. MgO III. SO ow many electrons does the ion 15 P contain? A. 1 B. 15 C. 16 D What is the formula of magnesium fluoride? A. Mg F 3 B. Mg F C. Mg 3 F 7. What is the electron arrangement of the Mg + ion? A., B.,8 C.,8, D.,8,8 8. Which property decreases down group 7 in the periodic table? A. Melting point B. Electronegativity C. Atomic radius D. Ionic radius D. MgF 11. What is the shape of the ammonia molecule, N 3? A. Trigonal planar B. Trigonal pyramidal C. Linear D. V-shaped (bent) 1. Which molecule is polar? A. C Cl B. BCl 3 C. Cl D. CCl 4

13 6 M10/4/CEMI/SPM/ENG/TZ/XX+ 7 M10/4/CEMI/SPM/ENG/TZ/XX+ 13. Which substance can form intermolecular hydrogen bonds in the liquid state? A. C 3 OC 3 B. C 3 C O C. C 3 CO D. C 3 C C Which is correct about energy changes during bond breaking and bond formation? Bond breaking Bond formation A. exothermic and positive endothermic and negative B. exothermic and negative endothermic and positive C. endothermic and positive exothermic and negative D. endothermic and negative exothermic and positive 14. Which compound has a covalent macromolecular (giant covalent) structure? A. MgO (s) B. Al O 3 (s) C. P 4 O 10 (s) D. SiO (s) 15. The standard enthalpy changes for the combustion of carbon and carbon monoxide are shown below. C(s) O (g) CO (g) 394 kj mol Ö 1 c 1 Ö CO(g) O(g ) CO(g ) c 83 kj mol Which processes are exothermic? I. Ice melting II. Neutralization III. Combustion What is the standard enthalpy change, in kj, for the following reaction? 1 C(s) O (g) CO(g) 18. Which unit could be used for the rate of a chemical reaction? A. 677 B. 111 C D A. mol B. mol dm 3 C. mol dm 3 s 1 D. dm

14 8 M10/4/CEMI/SPM/ENG/TZ/XX+ 9 M10/4/CEMI/SPM/ENG/TZ/XX+ 19. Which of the following can increase the rate of a chemical reaction? I. Increasing the temperature II. Adding a catalyst III. Increasing the concentration of reactants 0. What is the equilibrium constant expression, K c, for the following reaction? NO A. K c [ ] [ NO] 4 NO B. K c [ ] [ NO ] NO C. K c [ ] [ NO ] D. K c [ NO][ NO 4] 4 4 NO(g) NO (g) 4. Which species behave as Brønsted-Lowry acids in the following reversible reaction? PO ( aq) CN ( aq) CN (aq) PO ( aq) 4 4 A. CN and CN B. CN and PO 4 C. PO 4 and PO 4 D. CN and PO 4 3. Which of the following are weak acids in aqueous solution? I. C 3 COO II. CO 3 III. Cl 4. In which species does sulfur have an oxidation number of 0? A. SO 3 1. Consider the endothermic reaction below. 5CO(g) IO(g) 5CO (g) I(g) 5 According to Le Chatelier s principle, which change would result in an increase in the amount of CO? B. S 8 C. Na SO 4 D. S A. Increasing the temperature B. Decreasing the temperature C. Increasing the pressure D. Decreasing the pressure

15 10 M10/4/CEMI/SPM/ENG/TZ/XX+ 5. What is the reducing agent in the reaction below? MnO ( aq) Br ( aq) O(l) MnO (s) BrO ( aq) O ( aq) 4 3 A. Br B. BrO 3 C. MnO 4 D. MnO 6. Which changes could take place at the positive electrode (cathode) in a voltaic cell? I. Zn + (aq) to Zn (s) II. Cl (g) to Cl (aq) III. Mg (s) to Mg + (aq) 11 M10/4/CEMI/SPM/ENG/TZ/XX+ 8. What happens when a few drops of bromine water are added to excess hex-1-ene and the mixture is shaken? I. The colour of the bromine water disappears. II. III. The organic product formed does not contain any carbon-carbon double bonds. -bromohexane is formed. 9. What is the product of the following reaction? A. C 3 COO B. C 3 COC 3 C. C 3 C COO 7 C C(O)C 3 3 Cr O / D. C 3 C C 3 7. What is the structural formula of,3-dibromo-3-methylhexane? A. C 3 CBrCBrC(C 3 )C C 3 B. C 3 CBrCBr(C 3 )C C C 3 C. C 3 C CBrCBr(C C 3 ) D. C 3 CBrCBrC(C C 3 ) 30. ow many significant figures are there in ? A. B. 3 C. 5 D

16 3 N08/4/CEMI/SPM/ENG/TZ0/XX 4 N08/4/CEMI/SPM/ENG/TZ0/XX 1. Analytical chemists can detect amounts of amino acids as small as mol of molecules. ow many molecules does this represent? A B C D Complete combustion of a hydrocarbon produces 0.44 g of CO and 0.18 g of O. What is the empirical formula of the hydrocarbon? A. C B. C C. C 3 D. C 4. One stage in the manufacture of nitric acid is the oxidation of ammonia: N 3(g) O (g) NO(g) O(l) When the equation is balanced using the smallest possible whole numbers, what is the coefficient for N 3? A. B Which species contains the same number of electrons and neutrons? A. 1 1 B. 1 C. 7 3 Li D Cl C. 5 D What amount of solute ions, in moles, is present in 50 cm 3 of 0.10 mol dm 3 sodium hydroxide solution? A B C D

17 5 6. The mass spectrum of a sample of an element is shown below. N08/4/CEMI/SPM/ENG/TZ0/XX 6 N08/4/CEMI/SPM/ENG/TZ0/XX 8. The graph shows the trend in a physical property down group 7 in the periodic table. 40 % abundance 0 Physical property mass / charge What is the physical property? F Cl Br I Which value is closest to the relative atomic mass of the element? A B C A. Atomic radius B. Electronegativity C. Density D. Melting point D The table shows the boiling points of the hydrogen halides. 7. In what order are the elements listed in the periodic table? A. In order of relative atomic mass B. In order of reactivity C. In order of nuclear charge D. In order of electronegativity Compound Boiling point / C F 0 Cl 85 Br 67 I 35 Which statement explains the higher boiling point of hydrogen fluoride? A. The covalent bond in hydrogen fluoride is stronger than those in the other hydrogen halides. B. There is strong hydrogen bonding between the hydrogen fluoride molecules. C. Fluorine is the most reactive element in group 7. D. Fluorine has the highest first ionization energy in group

18 7 10. What happens when lithium and oxygen react together? A. Each lithium atom gains one electron. B. Each lithium atom loses one electron. C. Each oxygen atom gains one electron. D. Each oxygen atom loses one electron. N08/4/CEMI/SPM/ENG/TZ0/XX 8 N08/4/CEMI/SPM/ENG/TZ0/XX 14. Which graph shows the variation in volume of a fixed mass of an ideal gas with temperature in C at constant pressure? A. Volume / cm 3 B. Volume / cm Which substance has the lowest electrical conductivity? Temp / C Temp / C A. Al (s) B. Al O 3 (l) C. KCl (aq) D. Cl (g) C. Volume / cm 3 D. Volume / cm 3 1. What is the C C C bond angle in C 3 COC 3? A. 180 B Temp / C 15. Which statement about covalent bonds is correct? Temp / C C. 109 D. 90 A. Breaking covalent bonds is exothermic and releases energy. B. Breaking covalent bonds is endothermic and absorbs energy. C. Making covalent bonds is exothermic and absorbs energy. 13. Which sample contains molecules with the greatest average kinetic energy? D. Making covalent bonds is endothermic and releases energy. A. at 100 K B. C 3 8 at 73 K C. N at 73 K D. Br at 373 K

19 9 N08/4/CEMI/SPM/ENG/TZ0/XX 10 N08/4/CEMI/SPM/ENG/TZ0/XX 16. The average bond enthalpy for the C bond is 41 kj mol 1. Which process has an enthalpy change closest to this value? A. C (g) C(s) (g) 4 B. C (g) C(g) (g) 4 C. C 4(g) C(g) 4(g) D. C (g) C(g) (g) The graph below shows how the concentration of X changes with time during the following reaction: [X] / mol dm 3 X Y 17. A reaction has a positive Ö and a negative S Ö value. Which statement about this reaction is correct? A. It is not spontaneous at any temperature. B. It is spontaneous at all temperatures. C. It is spontaneous only at low temperatures. D. It is spontaneous only at high temperatures Time / s Which graph shows the change in concentration of Y during the same time period? A. [Y] / mol dm 3 B. [Y] / mol dm When 50 cm 3 of 1.0 mol dm 3 nitric acid solution, NO 3 (aq), is added to 50 cm 3 of 1.0 mol dm 3 potassium hydroxide solution, KO (aq), the temperature of the mixture increases by 6.4 C. What will be the temperature change when 5 cm 3 of each of these solutions are mixed together? A. 1.6 C C Time / s Time / s D. B. 3. C C. 6.4 C D. 1.8 C [Y] / mol dm Time / s Time / s [Y] / mol dm

20 11 N08/4/CEMI/SPM/ENG/TZ0/XX 1 N08/4/CEMI/SPM/ENG/TZ0/XX 0. Which statement about the activation energy of a reaction is correct? A. The activation energy is changed by the presence of a catalyst but not by an increase in temperature. B. The activation energy is changed by an increase in temperature but not by the presence of a catalyst. C. The activation energy is changed by both an increase in temperature and the presence of a catalyst. D. The activation energy is not changed by either an increase in temperature or the presence of a catalyst. 3. Which statement describes a difference between strong acids and weak acids? A. Solutions of weak acids cannot conduct an electric current but solutions of strong acids can conduct an electric current. B. Strong acids can form concentrated solutions but weak acids cannot form concentrated solutions. C. Weak acids are less soluble in water than strong acids. D. Strong acids are more dissociated in aqueous solution than weak acids. 4. Which combinations form buffer solutions? 1. The manufacture of ammonia is based on the equilibrium: N(g) 3 (g) N (g) Ö 9 kj mol 3 Which changes will increase the equilibrium concentration of ammonia? I. Increasing the pressure II. Decreasing the temperature III. Adding an iron catalyst 1 I. 50 cm 3 of 0.1 mol dm 3 C 3 COO (aq) + 5 cm 3 of 0.1 mol dm 3 NaO (aq) II. 50 cm 3 of 0.1 mol dm 3 C 3 COO (aq) + 50 cm 3 of 0.1 mol dm 3 NaO (aq) III. 50 cm 3 of 0.1 mol dm 3 C 3 COO (aq) + 50 cm 3 of 0.1 mol dm 3 C 3 COONa (aq) 5. Which statement about the electrolysis of molten sodium bromide is correct? A. Bromide ions lose electrons at the negative electrode. B. Bromide ions gain electrons at the positive electrode.. What alters the value of the equilibrium constant, K c, for a reversible reaction? A. Changing the temperature C. Bromide ions gain electrons at the negative electrode. D. Bromide ions move even if there is no current. B. Changing a reactant concentration C. Changing a product concentration D. Adding a catalyst

21 13 N08/4/CEMI/SPM/ENG/TZ0/XX 14 N08/4/CEMI/SPM/ENG/TZ0/XX 6. In which compound does manganese have the highest oxidation number? A. MnCl B. MnO C. Mn O 3 D. MnSO 4 9. ow many different compounds have the molecular formula C 3 8 O? A. B. 3 C. 4 D Palladium chloride changes colour in the presence of carbon monoxide as shown below. PdCl (s) CO(g) O(l) Pd(s) CO (g) Cl(aq) orange black In terms of oxidation numbers, which changes occur during the reaction? I. Palladium is reduced. II. III. Carbon is oxidized. ydrogen is reduced. 30. Which compound, when hydrogenated, gives a product with a chiral centre? A. C = C B. C 3 CBr = C C. C 3 C CBr = C D. C 3 C C(C 3 ) = C 8. Which of the following can form an addition polymer? A. Alanine (-aminopropanoic acid) B. Butane C. But--ene D. 1,-dichlorobutane

22 3 M08/4/CEMI/SPM/ENG/TZ/XX+ 4 M08/4/CEMI/SPM/ENG/TZ/XX+ 1. What is the amount of atoms, in moles, in 88 g of carbon dioxide? A B C. 6 D. 1. The isotopic abundances for an element, X, are 8 14 X = 0 % and 9 14 X = 80 %. What is the relative atomic mass of element X? A. 14 B. 8. C. 8.5 D Which statement is correct about the molecular formula of a compound? 4. A sample of a hydrocarbon contains 84 g of carbon and 14 g of hydrogen. Which of the following statements are correct? I. The empirical formula of the compound is C. II. The molecular formula of the compound is C 4. III. There is not enough information to confirmthat the molecular formula ofthe compound is C An isotope of uranium has a mass number of 35. What is the number of neutrons in the nucleus and the atomic number for this isotope? Number of neutrons Atomic number A B C D A. It is an integer multiple of the empirical formula. B. It shows how the atoms are bonded together in the molecule. C. It is the smallest ratio between the atoms present in a molecule. D. It is the percentage composition of a molecule. 6. Which process is responsible for the lines in the visible emission spectrum of hydrogen? A. The release of energy by the electron B. The release of energy by the excited nucleus C. The excitation of the electron D. The absorption of energy by the electron

23 5 M08/4/CEMI/SPM/ENG/TZ/XX+ 6 M08/4/CEMI/SPM/ENG/TZ/XX+ 7. Which reactions are spontaneous? I. Cl (aq) KBr(aq) Br(aq) KCl(aq) II. I(aq) KBr (aq) Br (aq) KI(aq) III. Cl (aq) NaI(aq) I (aq) NaCl(aq) 10. What are the correct formulas of magnesium nitride and aluminium sulfide? A. Mg N 3 and Al S 3 B. Mg N 3 and Al S 3 C. Mg N 3 and Al S 3 D. Mg N 3 and Al S Which molecule is the most polar? A. C 4 8. Which statements support the description of aluminium oxide as amphoteric? I. It can show acidic behaviour in the presence of strong alkalis. II. It can show alkaline behaviour in the presence of strong acids. III. It dissolves in water to form a neutral solution. 9. Which species has the same electron arrangement as a Ca ion? A. Al 3 ion B. Br ion C. Ar atom D. K atom B. CCl 4 C. CF 4 D. CCl 3 1. What is the shape of PCl 3? A. Trigonal planar B. Trigonal pyramidal C. Tetrahedral D. V-shaped (bent) 13. Which changes occur when a liquid boils? I. The spacing between the particles increases. II. The average energy of the particles increases. III. The attractive forces between the particles become weaker

24 7 M08/4/CEMI/SPM/ENG/TZ/XX+ 8 M08/4/CEMI/SPM/ENG/TZ/XX+ 14. A gas sample occupies a volume V 1 at a pressure P 1 and a Kelvin temperature T 1. What would be the temperature, T, of the gas if both its pressure and volume are doubled? 1 A. T = T 1 B. T T1 C. T T1 D. T 4T1 17. What should be the signs of G, and S for a chemical reaction to be spontaneous at any temperature? G S A. positive negative positive B. negative negative negative C. negative negative positive D. negative positive negative 15. Which of the following is correct about the energy changes during bond breaking and bond formation? Bond breaking Bond formation A. exothermic endothermic B. exothermic exothermic C. endothermic endothermic D. endothermic exothermic 18. Which of the following reactions is likely to have the largest negative entropy change, S? A. C(s) O(g) CO (g) B. NO(g) 4 NO (g) C. SO (g) O (g) SO(g) 3 D. N(g) 3(g) N 3(g) 16. A possible method of preparing hydrogen peroxide is: 1 Ö ( g) O (g) O(l) x 1 Ö O(l) O (g) O(l) y Which expression can be used to calculate the enthalpy change for the decomposition of hydrogen peroxide using this data? 19. Which statement explains why increasing the temperature increases the rate of a chemical reaction? A. More molecules have energy equal to or greater than the activation energy. B. At a higher temperature the activation energy for the reaction is lower. C. More molecules have the correct collision geometry. D. The reaction proceeds according to Le Chatelier s principle. O(l) (g) O (g) A. x y B. x y C. x y D. x y 0. What is the best way to describe the rate-determining step in a reaction mechanism? A. The fastest step of a chemical reaction B. The slowest step of a chemical reaction C. The step where the fewest molecules interact D. The step where most molecules have the highest energy

25 9 M08/4/CEMI/SPM/ENG/TZ/XX+ 10 M08/4/CEMI/SPM/ENG/TZ/XX+ 1. Consider the reaction: 4. Which pair of solutions can be used to prepare a buffer solution? A (g) 3B(g) C(g) D(g) What is the expression for the equilibrium constant, K c? [C][D] A. K c [A] 3[B] [A] 3[B] B. K c = [C] [D] [C][D] C. K c 3 [A] [B] 3 [A] [B] D. K c [C][D]. Consider the following reaction: N(g) 3(g) N (g) Ö 9kJ 3 Which of the following affects the value of K c? A. Adding a catalyst B. Increasing the pressure C. Increasing the concentrations of nitrogen and hydrogen A. C3 COONa (aq) / NaO (aq) B. N 3(aq) / N4NO 3(aq) C. N4 Cl(aq) / Cl(aq) D. NO 3(aq) / NaNO 3(aq) 5. What is the oxidation number of vanadium in the compound NaVO 3? A. 1 B. 0 C. + D Which statement about electrochemical cells is correct? A. The reaction in a voltaic cell is spontaneous. B. The reaction in an electrolytic cell is spontaneous. C. The reaction in a voltaic cell uses electrical energy. D. The reaction in an electrolytic cell produces electrical energy. D. Increasing the temperature 3. Which compound will produce a solution with a p greater than 7 when added to water? A. NaCO (s) 3 B. SiO (s) C. SO (g) 3 D. C CO (aq)

26 11 M08/4/CEMI/SPM/ENG/TZ/XX+ 1 M08/4/CEMI/SPM/ENG/TZ/XX+ 7. Consider the following reaction: Sn (aq) Fe (aq) Sn 3 (aq) Fe (aq) What is the correct combination of statements? Species Undergoes Acts as A. Sn 4+ oxidation oxidizing agent B. Fe + reduction reducing agent C. Sn 4+ reduction oxidizing agent D. Fe + reduction oxidizing agent 30. What type of linkage forms between two amino acids, when they react with each other? A. Ketone B. Amine C. Amide D. Ester 8. Which molecule has a chiral carbon atom? A. C CClC C 3 B. C COC C 3 3 C. (C )CC C 3 3 D. NC COO 9. The polymerization of ethene C Cproduces polythene as shown below. What type of reaction has ethene undergone? A. ydrogenation B. Addition C. Isomerisation D. Condensation n C = C [ C C ] n