MJC H2 Chem 2012 Prelim P1 QP

1 Name ________________________ Class: ___________ Reg Number: _____ MERIDIAN JUNIOR COLLEGE JC2 Preliminary Examination Higher 2 _________________________________________________________________________ Chemistry 9647/1 Paper 1 Multiple Choice 20 September 2012 1 hour Additional Materials: OMR Sheet Data Booklet ___________________________________________________________________ INSTRUCTIONS TO CANDIDATES Write your name, class and register number in the spaces provided at the top of this page. Write your calculator brand and model/number in the box provided above. There are forty questions in this section. Answer all questions. For each question, there are four possible answers labelled A, B, C and D. Choose the one you consider correct and record your choice in soft pencil on the OMR answer sheet. Read very carefully the instructions on the use of the OMR answer sheet. You are advised to fill in the OMR Answer Sheet as you go along; no additional time will be given for the transfer of answers once the examination has ended This document consists of 19 printed pages and 1 blank page. Calculator Model / No. Use of OMR Answer Sheet Ensure you have written your name, class register number and class on the OMR Answer Sheet. Use a 2B pencil to shade your answers on the OMR sheet; erase any mistakes cleanly. Multiple shaded answers to a question will not be accepted. For shading of class register number on the OMR sheet, please follow the given examples: If your register number is 1, then shade 01 in the index number column. If your register number is 21, then shade 21 in the index number column.

2 pV p p pV Section A For each question there are for possible answers, A , B, C and D. Choose the one you consider to be correct. 1 Which of the following statements contains one mole of the stated particle? A Molecules in 19.0 g of fluorine gas. B Electrons in 24.0 dm3 of hydrogen gas at room temperature and pressure. C Neutrons in 1.00 g of helium gas. D Protons in 2.02 g of neon gas. 2 Which of the following diagrams correctly describes the behaviour of a fixed mass of an ideal gas at constant T? A C B D p pV T p pV T

3 3 Two elements X and Y have the following properties. · X and Y form ionic compounds Na2X and Na2Y respectively. · Element Y forms YF6 molecule whereas X is unable to do so. Which pair of electronic configurations of X and Y is correct? X Y A [He]2s22p2 [Ne]3s23p2 B [He]2s22p2 [Ne]3s23p4 C [He]2s22p4 [Ne]3s23p2 D [He]2s22p4 [Ne]3s23p4 4 Ions of the two most common isotopes of zinc are shown below: 64 30 2+Zn 66 30 2+Zn Which of the following statements is correct? A Both these Zn 2+ ions have the same number of electrons but different number of protons. B B oth these Zn 2+ ions have the same electron configuration 1s22s22p63s23p63d84s2. C The 64 30 2Zn + ion has fewer neutrons in its nucleus than the 66 30 2Zn + ion. D T he 66 30 2+Zn ion will be deflected more than the 64 30 2Zn + ion in an electric field of the same strength. 5 For the pairs of species shown below, in which does the first species have a larger bond angle than the second? A PH3, NH3 C SO32-, CO32- B CH 2Cl2, OCl2 D BrF2-, BeCl2

4 6 In an experiment, a radioactive sample of the sodium thiosulfate, Na 2S2O3 was prepared by boiling solid sulfur containing 35S with sodium sulfite, Na 232SO3. Adding HC l (aq) to this sample causes all the 35S to precipitate as sulphur, leaving a resulting solution that contains non-radioactive sulfite ions. Which of the following depicts the correct displayed formula of the thiosulfate ion produced? A S 32 O O O S 35 2- C S 35 O O S 32 O 2- B S 32 O O O S 35 2- D S 32 O O S 35 O 2- 7 An experiment is conducted to investigate the kinetics of reaction between bromopropane and 0.1 mol dm-3 sodium hydroxide. The rate equation is as follows: Rate = k [bromopropane] [OH-] The half-life of bromopropane in one of the experiments is t minutes. What is the new half-life (in minutes) of bromopropane when the concentration of bromopropane is doubled and concentration of sodium hydroxide is reduced to 0.01 mol dm -3? A 0.05t B 0.1t C 5 t D 10t

5 8 Consider the following equilibrium system: H2 (g) + I2 (g) 2HI (g) DH = +53 kJ mol-1 Which of the following change is incorrect? A Numerical value of Kp is not equal to Kc at 25 °C. B Increasing the mass of H 2 will not cause the equilibrium constant to increase. C Increasing t emperature increases the rate constant and equilibrium constant. D Rate of forward reaction is equal to rate of backward reaction when equilibrium is reached. 9 The graph shows the change in pH when 0.25 mol dm -3 acid is gradually added to V cm3 of 0.25 mol dm-3 base. Which pair of solutions will give the result as shown in the graph? A HNO 3 and NH3 B H 2SO4 and CH3NH2 C CH 3COOH and Ca(OH)2 D CH 2(COOH)2 and NaOH pH Volume of acid added /cm3 14 7 ½ V V

6 10 The solubility product of iron( II) carbonate is 2.1 ´ 10–11 while that of silver carbonate is 8.1 ´ 10–12 at 25°C. Which of the following statements is true? A Addition of silver nitrate increases the solubility of silver carbonate. B Addition of sul furic acid to a solution containing iron( II) carbonate increases the solubility product of iron(II) carbonate. C Iron(II) carbonate precipitates first when sodium carbonate is added to a solution containing equal concentrations of iron(II) and silver ions. D The solubility of iron( II) carbonate is higher than the solubility of silver carbonate. 11 Liquid E has an DHq of vapouri sation of +10.0 kJ mol-1 and a boiling point of 266 K. What is the DSq of condensation of vapour E? A –2 6.6 J mol-1 K-1 B – 37.6 J mol-1 K-1 C +26.6 J mol-1 K-1 D +37.6 J mol-1 K-1 12 Which of the following has an exothermic enthalpy change? A Ca (g) ® Ca2+ (g) + 2e B CaO (s) ® Ca2+ (g) + O2- (g) C ½ O2 (g) ® O (g) D O (g) + e ® O- (g)

7 13 When a solution of concentrated sodium carboxylate is electrolysed, the equation for the reaction is 2RCO2Na (aq) + 2H2O (l) R– R (l) + 2CO2 (g) + 2NaOH (aq) + H2 (g) Which statement regarding the electrolysis is correct? A Carbon dioxide is liberated at the cathode. B Hydrogen is liberated at the cathode. C R– R is liberated at the cathode. D The solution around the anode turns red litmus blue. 14 When a large current was passed through acidified aqueous copper( II) sulfate, there was simultaneous liberation, at the cathode, of x mol of copper and y dm 3 of hydrogen (measured at s.t.p.). How many moles of electrons passed through the solution? A 11.2 yx + C 2 11.2 yx + B 22.4 yx + D 2 22.4 yx + 15 Two cells, one containing a molten chloride of manganese and the other containing molten chromium (II) chloride were connected in series. 11.0 g of manganese and 15.6 g of chromium were deposited. What is the oxidation state of manganese ion in the chloride? A +2 B +3 C +4 D +5

8 16 Element G is in the third period of the Periodic Table. The chloride of G has a simple molecular structure while the oxide of G has a giant ionic structure. Which of the following statements is true about G? A The atomic radius of G is smaller than that of Cl. B The first ionisation energy of G is higher than that of Mg. C The chloride of G dissolves in water to give a neutral solution. D The oxide of G reacts with excess aqueous sodium hydroxide to form a colourless complex. 17 J, K and L are elements in Period 3. K has a larger ionic radius than J , and L has a less endothermic first ionisation energy than K. What are ele