1 AJC BT1 2013 9647/02/H2[Turn overANDERSON JUNIOR COLLEGE Block Test 1 2013 (modified) NAME: ____________ PDG: __________ Register No:_____ CHEMISTRY 9647/02 Higher 28 January 2013 Paper 2 Structured Questions1 hour 30 minutesCandidates answer on the Question Paper. Additional Materials: Data Booklet This document consists of 13 printed pages. Topics Tested: Chemical Energetics Chemical Equilibria Ionic Equilibria Chemical Periodicity Reaction Kinetics All Organic Chemistry until Arenes IMPORTANT! Please read this first! You need to revise on the topics first so that you can use this paper to consolidate your learning and find out which are the topics that you need to further work on. Please attempt this paper as a time trial, noting the time given (as indicated above) to complete it. Before you attempt the questions, check that you have the following: Data Booklet Calculator
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You need to revise on the topics first so that you can use thispaper to consolidate your learning and find out which are thetopics that you need to further work on.
Please attempt this paper as a time trial, noting the time given
(as indicated above) to complete it. Before you attempt the questions, check that you have the
3 (a) Many chemists have contributed to the development of the Periodic Table. John Newlandwas one of the first few chemists who attempted to classify elements in a systematic way,based on atomic weight. Part of Newland’s Periodic Table is shown below.
Row 1 5B 6C 7N 8O
Row 2 9F 11Na 12Mg 13 Al 14Si 15P 16S
Row 3 17Cl 19K 20Ca 24Cr 22Ti 25Mn 26Fe
On each of the grids below, sketch the general trends of the properties of the elementsacross Row 2 of Newland’s Periodic Table.
(i) (ii)
(iii) (iv)
[4](b) Aluminium oxide is amphoteric.
Write two equations that illustrate the amphoteric behavior of aluminium oxide and statewhich reaction is typical of a metal and which is typical of a non –metal.
(c) On crossing the second and third periods, the chlorides of the elements change in structureand in their reactions with water.
(i) 0.1 mol each of the four chlorides below is separately added to 1 dm of water.
Sketch a graph showing the variation in pH of these resulting solutions.
(ii) Account for the pH of the aqueous solutions of carbon tetrachloride and phosphoruspentachloride. Write balanced equations for the reactions, if applicable.
4 In a typical laboratory, gas phase reactions are difficult to control and hence not common.Industrial production utilising gas phase reactions are similarly difficult to control and typically onlyused for manufacture of organic chemicals, sulfuric acid (Contact process) or ammonia (Haberprocess).
The Contact process used to produce sulfuric acid involves a three –stage process. Using V2O5
as a catalyst, reaction II achieves 99.5% conversion of sulfur dioxide to sulfur trioxide. Theessential reactions are as follows:
In an experiment conducted at 25 oC, solid potassium hydrogen tartrate is firstdissolved in pure water until no more solid dissolves. The excess solid is then filteredoff to give a saturated solution. The solubility of potassium hydrogen tartrate at 25 oCwas found to be 0.0328 mol dm –3.
(i) Write an expression for the solubility product of potassium hydrogen tartrate.
(ii) From the data given on page 16, calculate a value for K sp of potassium hydrogentartrate at 25 oC and state its units.
K sp of potassium hydrogen tartrate ……………………………...
(iii) The saturated solution is now heated to 30 oC in a water bath. Concentrated aqueousKNO3 is then added dropwise to the heated solution.
The value of the K sp of potassium hydrogen tartrate at 30 oC is 1.58 x 10 –3.
Determine the concentration, in mol dm –3, of K+ ions present when the first trace ofprecipitate appears. State any assumption you have made.