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BOND ENERGIES (kJ/mol)
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PCl3(g) O2(g) POCl3(g) (a) (b) (c) (d) (e)
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P Cl O=O O O
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Determine the enthalpy change for the above reaction Estimate the PO bond energy Is the PO bond a single or a double bond Justify your answer Calculate the entropy change for the reaction Is this reaction spontaneous or nonspontaneous at 25 C Justify your prediction
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314 U STEP 5 Build Your Test-Taking Confidence
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Question 3 The following materials are made available for the determination of the molar mass of an unknown nonvolatile solid analytical balance test tube thermometer stopwatch beaker hot plate support stand and clamp
Phenol (melting point = 43 C and Kf = 740 C/m) is available as the solvent The unknown behaves as a nonelectrolyte in phenol (a) Plot a cooling curve for phenol on the axes below, and plot the cooling curve for a solution of the unknown in phenol
Solution:
Pure Phenol:
43 C
43 C
Time
Time
(b) (c) (d)
What information must be obtained from the two graphs in order to calculate the molar mass What additional information is needed to determine the molar mass of the unknown solid Show how the above information may be used to calculate the molar mass of the unknown solid
STOP
AP Chemistry Practice Exam 1 315
Part B Time 40 minutes
You may not use a calculator for part B Question 4 Answer all three of the following questions Each question will have two parts writing the balanced chemical equation and answering a question about the reaction Coefficients in the balanced chemical equation must be in the lowest whole-number ratio Do not include formulas for substances that remain unchanged during the reaction Unless otherwise noted, assume all the reactions occur in aqueous solution If a substance is extensively ionized and therefore is present as ions in solution, write its formula as ions Example: Hydrochloric acid is added to a lead(II) nitrate solution
2+ Pb + 2 Cl PbCl2
(a) Excess potassium cyanide is added to an iron(III) nitrate solution Which species behaves as a Lewis base in the reaction Explain (b) Chlorine gas is bubbled through a solution of calcium iodide Identify the oxidizing and reducing agents in this reaction (c) An iron(III) nitrate solution is made basic with potassium hydroxide solution Identify the spectator ions, if any, in this reaction Question 5 A sample of a solid, weak monoprotic acid, HA, is supplied along with standard sodium hydroxide solution The sodium hydroxide solution was standardized with potassium hydrogen phthalate (KHP) (a) (b) (c) (d) (e) List the apparatus required to titrate an HA solution Sketch a pH versus volume of base added curve for the titration Sketch the titration curve if the unknown acid was really a diprotic acid Describe the steps required to determine the molar mass of HA How would the molar mass of HA be changed if the KHP contained an inert impurity
Question 6 Relate each of the following to atomic properties and the principles of bonding (a) The ionization energy of nitrogen atoms is higher than expected (b) Draw the Lewis electron-dot structures for CO2 and CO Explain the polarity of these compounds (c) The compound C2H3F is polar, but compounds with the general formula C2H2F2 are sometimes polar and sometimes nonpolar Show the structures and explain (d) There are two isomers with the formula C2H6O One of the isomers is more soluble in water than the other Use the structures of these two compounds to explain the difference in solubility (e) Why does SiF4 react with fluoride ion, and CF4 not react
STOP End of AP Chemistry Practice Exam 1
316 U STEP 5 Build Your Test-Taking Confidence
U Answers and Explanations for Exam 1 Multiple Choice
1 C This is the only one that has a pair of electrons to donate 2 B All can behave as Br nsted bases Only B cannot behave as an acid 3 A This is the definition of a Lewis base 4 E The buret should be rinsed with titrant, not water 5 D The others are normally monatomic anions 6 C Increasing sizes indicate decreasing charge, lower position in a column on the periodic table, or position to the left in a period on the periodic table 7 D The element furthest away from F 8 D Hexammine = (NH3)6; chromium(III) = 3+ Cr ; chloride = Cl 9 B 2 Fe(OH)3(s) + 3 H2SeO4(aq) Fe2(SeO4)3(s) + 6 H2O(l) 10 C The soluble compounds should be separated and the spectator ions eliminated 11 B Magnesium nitride does form 12 D Some of the nickel remains, the sodium does not change, and two nitrates are formed per nickel(II) nitrate 13 A The reactions are: NH4 + OH NH3 + 2 2+ H2O and Ba + SO4 BaSO4 14 B Percentages: (A) 778; (B) 696; (C) 720; (D) 632; (E) 495 Approximate the atomic weights to simplify the calculations 15 E Percentage of water: (A) 11; (B) 20; (C) 43; (D) 50; (E) 56 16 D Nitric acid is the limiting reagent 17 A (221 g)(1 mol/442 g)(3 mol O2/2 mol) = 22 -3 750 10 mol Simplify to (15) 440 18 B 4 C4H11N(l) + 27 O2(g) 16 CO2(g) + 22 H2O(l) + 2 N2(g)
19 C Sulfuric acid is the limiting reagent 20 A (10 mol KClO3)(3 mol O2/2 mol KClO3) = 15 mol 21 C (0100 mol Sr)(l mol H2/l mol Sr) (224 L/mol) = 224 L H2 22 C The average velocity is related to temperature 23 D Water, whenever present, will contribute its vapor pressure 24 B T2 = (V2T1)/V1 = [(1500 L 400 K)/(600 L)] 273 = 727 C 25 D Small and nonpolar 26 A Definition 27 B Definition 28 D Definition 29 A 1 2[2 ClF(g) + O2(g) Cl2O(g) + OF2(g)] 1 2(1675 kJ) 1 1 2[2 F2(g) + O2(g) 2 OF2(g)] 2( 435 kJ) 1 2[Cl2O(g) + 3 OF2(g) 2 ClF3(l) + 2 O2(g)] 1 2(3941 kJ) ClF(g) + F2(g) C1F3(l) 1351 kJ
30 A Exothermic processes shift toward the starting materials when heated 31 A Definition 32 E Subtract the heat of vaporization from the original value
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