SRJC H2 Chem 2013 Prelim P1 QP

1   Turn Over] SERANGOON JUNIOR COLLEGE General Certificate of Education Advanced Level Higher 2 Candidate Name Class CHEMISTRY 9647/01 JC2 Preliminary Examination 30 Aug 2013 Paper 1 Multiple Choice 1 hour Additional Materials: Data Booklet Optical Mark Sheet (OMS) READ THESE INSTRUCTIONS FIRST On the separate multiple choice OMS given, write your name, subject title and class in the spaces provided. Shade correctly your FIN/NRIC number. There are 40 questions in this paper. Answer all questions. For each question there are four possible answers A, B, C and D. Choose the one you consider correct and record your choice using a soft pencil on the separate OMS. Each correct answer will score one mark. A mark will not be deducted for a wrong answer. You are advised to fill in the OMS as you go along; no additional time will be given for the transfer of answers once the examination has ended. Any rough working should be done in this question paper.     This document consists of 18 printed pages and 2 blank pages.  1204

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3   Turn Over] 4 The boiling point of water (100 oC) is greater than that of ammonia (–33 oC). Which statement is a correct explanation of this? A Ammonia has intramolecular hydrogen bonds, which water does not have. B The Mr of water is greater than that in ammonia, so van der Waals’ forces are stronger in water. C There are, on average, more hydrogen bonds between water molecules than there are between ammonia molecules. D The O–H bond requires 460 kJ mol –1 to overcome, while the N–H bond only requires 390 kJ mol–1 to overcome. 5 The standard enthalpy change of formation of hydrazine, N2H4(g), is x kJ mol–1. The bond energy of the NN bond is y kJ mol–1. The bond energy of the H–H bond is z kJ mol–1. What is the standard enthalpy change of atomisation of hydrazine? A (x + y + 2z) kJ mol –1 B (y + 2z – x) kJ mol–1 C (x + 2y + 4z) kJ mol–1 D (2y + 4z – x) kJ mol–1 6 The Gsolution  and Ssolution  for silver chloride are +55.6 kJ mol –1 and +33.2 J mol –1 K–1 respectively. What is the enthalpy change when 287 g of silver chloride is precipitated under the same conditions? A +65.5 kJ B –65.5 kJ C +131 kJ D –131 kJ 1206

4   Turn Over] 7 The diagram shows the reaction pathway diagram for an uncatalysed reversible reaction. The reaction was then catalysed. What are the changes in the rate constant, equilibrium constant and the reaction pathway diagram? Rate constant, k Equilibrium constant, Kc Energy profile A Unchanged Increase B Increase Unchanged C Increase Increase D Increase Unchanged 1207

5   Turn Over] 8 Steam dissociates at an initial pressure of 1 atm at T K to form hydrogen gas and oxygen gas. 2H2O(g) 2H2(g) + O2(g) If the total pressure at equilibrium is 1.3 atm, what is the numerical value of the equilibrium constant, Kp, of the reaction at T K? A 0.028 B 0.135 C 0.450 D 0.675 9 The following graphs show the change in pH when four different pairs of acid and base were titrated against each other. In each titration, a 1.0 mol dm -3 solution of an acid is gradually added to 20 cm 3 of a 1.0 mol dm-3 solution of a base. Which pair of solutions could not have given any of the graphs above? A HNO3 and NH3 B HCl and Ca(OH)2 C H2SO4 and NaOH D CH3COOH and NH3 1208

10 A lea ad A B C D 11 U s Th E Th Tw B : C: W A B C D solution c o ad ( II) co m dded dropw se of the Da he diagra  (Sn2+(aq)/S he e.m.f of t wo students : [H+ (aq)] w : [Sn2+(aq)] Which of thei Both B an B only C only Neither B Stan ontains 1 x 1 mpound will wise to the s Comp Lead (II) Lead (II) Lead (II) Lead (II) ata Booklet m repres e Sn(s)), the the cell was s, B and C, was greater was greate ir suggestio nd C B nor C ndard tin ha ce electro 10-3 mol dm be precipi t olution at 2 pound bromide sul fate fluoride iodide t is relevant ents an standard el s found to b suggested than 1.00 m er than 1.00 ons could be alf ell ode 6 m-3 of bromid tated first w 25 oC? to this ques experimen ectrode pot be 0.18 V ra possible ex mol dm-3. 0 mol dm-3. e correct? de, fluoride, when 0.01 So stion. nt to de t tential of tin ather than th xplanation. iodide and mol dm -3 o olubility prod 4.0 x 1.6 x 2.7 x 7.1 x ermine t h n he expected H2 (g) 1 Pt 1 mol d 25oC Tur d sulfate ion of lead ( II) duct at 25 oC 10-5 10 −8 10 −8 10 −9 he value d 0.14 V. atm dm-3 H+ (aq rn Over] ns. Which nitrate is C of the ) 1209

7   Turn Over]   12 The graph below shows the first thirteen ionisation energies for element D. What can be deduced from the graph about element D? A It is a transition element. B It is in Group IV of the Periodic Table. C It has one electron in its outermost shell. D It is in the third period (Na to Ar) of the Periodic Table. 13 Use of the Data Booklet is relevant to this question. The graph below shows the variation in the melting points for eight consecutive elements in the Periodic Table, all with atomic number below 20. What statement is correct? A Element D burns with a brilliant yellow flame. B Element F conducts electricity at room temperature. C Element H does not react with air at room temperature. D Element C is a gas which is chemically inert at room temperature. ionisation energy number of electrons removed 1210

8   Turn Over]     14 Use of the Data Booklet is relevant to this question. Zinc and magnesium are metals that are widely used in alloys such as Mazak which is used to make die-cast toys. Each metal forms many compounds containing a M 2+ ion. Which statement about the electron arrangements in the atoms and ions of zinc and magnesium is correct? A A zinc atom has fewer electrons than a magnesium atom. B A Zn 2+ ion has one more occupied electron shell than a Mg atom. C A Zn atom has two more occupied electron shells than a Mg2+ ion. D A Zn2+ ion has an outer electronic configuration of 4s2, while a Mg2+ ion has an outer electronic configuration of 3s2. 15 How would the magnitude of the following vary down Group II? (i) the lattice energy of the sulfate, H  latt, (ii) the standard enthalpy change of hydration of M 2+ (g), H hyd, (iii) the standard enthalpy change of solution of the sulfates, H  soln. H latt H hyd H soln A decreases decreases increases B decreases increases increases