RVHS 2026 Prelim P1 QP

RIVER VALLEY HIGH SCHOOL Preliminary Examination CANDIDATE NAME CLASS CENTRE NUMBER S INDEX NUMBER CHEMISTRY 9476/01 Paper 1 Multiple Choice 1 hour You must answer on the question paper. You will need: Multiple choice answer sheet Data booklet Soft clean eraser Soft pencil (type B or HB is recommended) INSTRUCTIONS • There are thirty questions on 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 in soft pencil on the multiple choice answer sheet. • Follow the instructions on the multiple choice answer sheet. • Write in soft pencil. • Write your name, centre number and index number on the multiple choice answer sheet in the spaces provided unless this has been done for you. • Do not use correction fluid or tape. • You may use an approved calculator. INFORMATION • The total mark for this paper is 30. • Each correct answer will score one mark. • Any rough working should be done on this question paper. This document has 16 pages. Any blank pages are indicated. [Turn over

2 River Valley High School 9476/01/Prelims/26 1 Use of the Data Booklet is relevant to this question. Which particle would, on losing an electron, have a half-filled set of p orbitals? 1 N− 2 S 3 Cl+ A 1 and 2 only B 1 and 3 only C 2 and 3 only D 1, 2 and 3 2 Element X has the following successive ionisation energies: ionisation energy 1st 2nd 3rd 4th 5th energy/ kJ mol−1 578 1817 2745 11577 14842 What is the formula of an oxide formed by element X? A X2O3 B XO C XO2 D X2O 3 Which of the following statements about ionisation energy of Period 3 elements is incorrect? A The first ionisation energy of Mg is higher than that of A l as Mg has a higher nuclear charge. B The first ionisation energy of Ar is higher than that of C l as Ar has a higher nuclear charge. C The first ionisation energy of P is higher than that of S as the electron to be removed from P experiences less electronic repulsion. D The shielding effect experienced by the valence electrons of Mg and P is similar. 4 Which of the following statements cannot be explained by hydrogen bonding? A Ice has a lower density than water at 0 C. B The boiling point of fluoromethane is higher than that hydrogen chloride. C The boiling point of 4-nitrophenol is higher than that of 2-nitrophenol. D The relative molecular mass of ethanoic acid is 120 when dissolved in benzene.

3 River Valley High School 9476/01/Prelims/26 [Turn over 5 C2N is a very unstable molecule that is not found naturally on Earth. Given that this molecule • has a carbon-carbon-nitrogen sequence of atoms, • has two  bonds, • is linear. What could be the number of lone pairs of electrons and unpaired electrons present in one molecule of C2N? lone pair of electrons unpaired electrons A 1 1 B 1 2 C 2 1 D 3 0 6 Which graph correctly describes the behaviour of fixed masses of the ideal gases L and M where the molar mass of L is smaller than the molar mass of M? A B C D

4 River Valley High School 9476/01/Prelims/26 7 In which reaction is H2S acting as a Bronsted-Lowry base? A H2S + 2NH3 → (NH4)2S B H2S + H2O  H3O+ + SH‒ C H2S + H2SO4 → H3S+ + HSO4‒ D H2S + NaOH → NaSH + H2O 8 An experiment was carried out to determine the enthalpy change of neutralisation in a reaction between NaOH and HNO3 using a polystyrene cup as a simple calorimeter. Which of the following changes will result in a lower temperature change? 1 conducting the experiment during cold weather 2 using lower concentrations of both reactants 3 using a higher concentration of NaOH A 1 and 2 only B 1 and 3 only C 2 and 3 only D 1, 2 and 3 9 Given that 6.01 kJ of energy is required to convert one mole of ice to water, calculate entropy change when 3.6 g of ice is converted to liquid water at 0 °C. A −4.4 J mol−1 K−1 B −0.0044 J mol−1 K−1 C +4.4 J mol−1 K−1 D +0.0044 J mol−1 K−1 10 The oxidation of iron by oxygen gas forming iron(III) oxide is an exothermic process. Which of the following statements about this reaction is true? A The reaction is spontaneous at all temperatures. B The reaction is spontaneous at high temperatures. C The reaction is spontaneous at lower temperatures. D The reaction is not spontaneous at any temperatures.

5 River Valley High School 9476/01/Prelims/26 [Turn over 11 10 cm3 of a gaseous hydrocarbon, C xHy, was mixed with 90 cm3 of excess oxygen gas and ignited. The total volume of the gases remaining in the tube was found to be 65 cm3. When the remaining gas mixture was passed through aqueous potassium hydroxide, the volume was reduced to 25 cm3. All gases are measured at room temperature and pressure. What is the molecular formula of the hydrocarbon? A C3H8 B C4H8 C C4H10 D C5H12 12 A 1.25 g sample of an impure anhydrous Group 2 metal carbonate, MCO3, was strongly heated until decomposition was complete. MCO3(s) → MO(s) + CO2(g) The carbon dioxide gas evolved was collected in a gas syringe and occupied a volume of 288 cm3 at room temperature and pressure . Given that the sample is 96.0% pure by mass and the impurities do not decompose on heating, what is the identity of the metal M? A Ba B Ca C Mg D Sr

6 River Valley High School 9476/01/Prelims/26 13 The diagram represents the reaction profile of a typical reaction involving only gases. The reversible reaction is carried out under different conditions each time. Which of the following shows the correct changes in the rate constant for both the forward and backward reactions? condition rate constant for forward reaction rate constant for backward reaction A add a catalyst increase no change B increase concentration of reactant increase no change C heat the reaction mixture decrease increase D react the gases in a smaller container no change no change

7 River Valley High School 9476/01/Prelims/26 [Turn over 14 For the gaseous reaction 2 A(aq) + 2 B(aq) → 2C(l) + D(g), the reaction is first order with respect to A and second order with respect to B. In the first experiment, at given concentration of A and B, 40 cm3 of gas was collected after exactly one minute. In the second experiment, under the same temperature, the initial concentration of A is doubled and that of B is halved. What is the predicted volume of gas collected after exactly one minute? A 10 cm3 B 20 cm3 C 40 cm3 D 80 cm3 15 In the production of sulfuric acid, one of the reactions involves the oxidation of sulfur dioxide gas. 2SO2(g) + O2(g)  2SO3(g) Equal amounts of SO 2 and O 2 gas was introduced into a container. The mixture at equilibrium was found to contain 48.0% SO3 when the total pressure was 5 atm. What is the numerical value of Kp of this equilibrium? A 13.1 B 6.19 C 2.62 D 1.80

8 River Valley High School 9476/01/Prelims/26 16 The numerical values of the solubility product of BaSO 4, BaCO 3 and Ba(IO3)2 at 25 °C are given in the table below. compound solubility product BaSO4 1.1  10−10 BaCO3 2.6  10−9 Ba(IO3)2 4.0  10−9 An aqueous solution of BaC l2 was added slowly, until in excess, to a solution containing 0.5 mol dm−3 Na2SO4, 1.0 mol dm−3 Na2CO3 and 1.5 mol dm−3 NaIO3 at 25 °C. What is the correct order of precipitation of the three barium salts? First to precipitate Last to precipitate A BaSO4 BaCO3 Ba(IO3)2 B Ba(IO3)2 BaCO3 BaSO4 C BaSO4 Ba(IO3)2 BaCO3 D BaCO3 Ba(IO3)2 BaSO4 17 AgCl and AgBr are both partially soluble solids. AgX(s)  Ag+(aq) + X−(aq), where X is Cl or Br When aqueous NH 3 is added to separate solutions of each silver halide, only AgC l dissolves to give a colourless solution. Which of the following statements are true for this observation? 1 The Ksp value of AgCl is higher than that of AgBr. 2 The