1. Which pair of substances could be separated by mixing with water and filtering? (A) NaNO3 and K2SO4 (B) CH3OH and CH3COCH3 (C) MgCO3 and Fe(OH)3 (D) KCl and CuS 2. Which gas produces an acidic solution when bubbled into water? (A) NH3 (B) Cl2 (C) H2 (D) CH4 3. A dilute HCl solution is to be prepared from a more concentrated solution. Which of pieces of glassware will give the highest level of precision? (A) graduated cylinder and volumetric flask (B) two graduated cylinders (C) pipet and graduated cylinder (D) pipet and volumetric flask 1) 2Mn2+(aq) + 4OH¯(aq) + O2(g) ---> 2MnO2(s) + 2H2O(l) 2) MnO2(s) + 2I¯(aq) + 4H+(aq) ---> Mn2+(aq) + I2(aq) + 2H2O(l) 3) 2S2O32¯(aq) + I2(aq) ---> S4O62¯(aq) + 2I¯(aq) (A) 0.5 (B) 1 (C) 2 (B) 0.60 M (C) 0.35 M (D) 0.30 M 12. How many electrons are present in 2.0 x 10¯3 moles of 188O2¯? (A) 1.2 x 1021 (C) 1.2 x 1022 (B) NaOH (D) SiO2 (D) 4 11. A 15 mL sample of 0.20 M MgCl2 is added to 45 mL of 0.40 M AlCl3. What is the molarity of Cl¯ ions in the final solution? (A) 1.0 M 4. Which substance is likely to show the greatest change in mass when exposed to air? (A) Al (C) CaCO3 10. These three equations describe an oxidationreduction method for determining dissolved oxygen in water. How many moles of S2O32¯ are equivalent of each mole of O2? (B) 9.6 x 1021 (D) 1.9 x 1022 13. In which change of state are covalent bonds broken? 5. Which is a yellow solid? (A) C (B) Na (C) S8 (D) I2 6. An alloy of gold and silver contains 38.5% silver by mass and has a density of 14.6 g mL¯1. What is the molar concentration of silver in this alloy? (A) 52.1 mol L¯1 (C) 3.57 mol L¯1 (B) 45.6 mol L¯1 (D) 2.64 mol L¯1 (A) evaporation of water (B) fusion of sodium chloride (C) vaporization of diamond (D) sublimation of dry ice 14. By what factor does the average velocity of a gaseous molecule increase when the absolute temperature is doubled? (A) 1.4 7. As2S3 reacts with O2 to give SO2 and As2O3. What is the smallest whole number coefficient for O2 when the equation for this reaction is balanced correctly? _As2S3(s) + _O2(g) ---> _As2O3(s) + _SO2(g) (A) 3 (B) 5 (C) 7 (D) 9 8. A 0.242 g sample of potassium is heated in oxygen. The result is 0.440 g of a crystalline compound. What is the formula of this compound? (A) KO (B) K2O (C) KO2 (D) KO3 9. What volume of 3.0 M Na2SO4 must be added to 25 mL of 1.0 M BaCl2 to produce 5.0 g of BaSO4? (A) 7.2mL (B) 8.3mL (C) 10.0mL (D) 14mL (B) 2.0 (C) 2.8 (D) 4.0 15. Which species is expected to have the highest boiling point at 1 am pressure? (A) O2 (B) CO (C) CO2 (D) HCHO 16. Which combination of vapor pressure, intermolecular forces and ΔHvaporization is matched correctly? vapor pressure (A) high intermolecular forces weak ΔHvaporization (B) high strong large (C) low weak large (D) low strong small : small 17. Which halogen in its standard state has the greatest absolute entropy per mole? (A) F2(g) (B) Cl2(g) (C) Br2(l) (D) I2(s) 18. Calculate ΔH° for this reaction. C2H2(g) + 2H2(g) ---> C2H6(g) ΔHcombustion, kJ mol¯1 C2H2(g) -1300 H2(g) -286 C2H6(g) -1560 (A) -312 kJ (B) -26 kJ (C) +26 kJ (D) +312 kJ 24. The reaction between KMnO4 and H2C2O4 can be followed by monitoring the disappearance of the purple color of the MnO4¯ ion. These data were obtained for the reaction carried out at a constant temperature of 25 °C. Initial Rate, Exp [MnO4¯] [H2C2O4] Disappearance of MnO4¯ (aq), M s¯1 1 1.08 x 10¯2 M 1.98 M 5.4 x 10¯5 2 1.08 x 10¯2 M 3.97 M 1.1 x 10¯4 3 2.17 x 10¯2 M 1.98 M 2.1 x 10¯4 Specify the order of this reaction with respect to [MnO4¯] and [H2C2O4] [MnO4¯] [H2C2O4] (A) 1st order 2nd order 19. For which process would ΔS° be expected to have the greatest positive value? (B) 2nd order 1st order (C) 1st order 1st order (A) O2(g) + 2H2(g) ---> 2H2O(g) (B) H2O(s) ---> H2O(l) (C) H2(g) + I2(g) ---> 2HI(g) (D) N2O4(g) ---> 2NO2(g) 25. For which reaction order is the half-life independent of the initial concentration? 20. (1/2) N2(g)+ (3/2) H2(g) ---> NH3(g) For this reaction at 25 °C, ΔG°f is -16.5 kJ mol¯1. What is the equilibrium constant, Keq, for this reaction at this temperature? 2 (A) 1.08 (B) 7.80 x 10 (C) 4.57 x 10 6 (D) 2nd order 2nd order (D) 2.98 x 10 34 21. What are the signs for ΔH, ΔS, and ΔG for the freezing of liquid water at -10 °C? ΔH ΔS ΔG (A) I only (C) both I and II II second order (B) II only (D) neither I nor II 26. What is the activation energy for the reverse of this reaction? N2O4(g) ---> 2NO2(g) Data for the given reaction is: ΔH = + 54.0 kJ and Ea = +57.2 kJ. (A) + (B) - - (C) - + - (A) -54.0 kJ (B) +3.2 kJ (C) +60.2 kJ (D) +111.2 kJ (D) - - 22. Which of these factors affect the value of the specific rate constant for the reaction 2A(g) ---> B(g)? 27. How does an increase in temperature affect the rates of the foward and reverse reactions for an exothermic reaction? rate of foward reaction rate of reverse reaction I concentration (A) increases increases (B) increases decreases (C) decreases increases (D) increases remains the same (A) I, II, and III (C) II and III only + 0 I first order - II pressure III temperature (B) I and II only (D) III only 23. Which statement about work and heat is true? (A) A given quantity of heat can be completely converted to work. (B) Heat and work are both state functions. (C) Some heat is always produced when work is done. (D) Work is a state function, whereas heat is not. 28. The reaction between chloroform, CHCl3(g), and chlorine, Cl2(g), to form CCl4(g) and HCl(g) is believed to occur by this series of steps. Step 1 Cl2 ---> Cl(g) + Cl(g) Step 2 CHCl3(g) + Cl(g) ---> CCl3(g) + HCl(g) Step 3 CCl3(g) + Cl(g) ---> CCl4(g) If this reaction is first order in CHCl3 and half order in Cl2, which statement about the relative rates of step 1, 2, and 3 is correct? (A) Step 1 is the slowest. (B) Steps 1 and 2 must both be slow. (C) Step 2 must be slower than step 1. (D) Step 3 must be the slowest 34. Which mixture forms a buffer when dissolved in 1.0 L of water? (A) 0.2 mol NaOH + 0.2 mol HBr (B) 0.2 mol NaCl + 0.3 mol HCl (C) 0.4 mol HNO2 + 0.2 mol NaOH (D) 0.5 mol NH3 + 0.5 mol HCl 29. This reaction occurs readily above 500 °C. 2HgO(s) ---> 2Hg(l) + O2(g) What is the equilibrium for this reaction? 35. The equilibrium constant for this reaction is 3.6 x 10¯7 OCl¯(aq) + H2O(l) <===> HOCl(aq) + OH¯(aq) What is Ka for HOCl? (A) K = [Hg]2[O2] / [HgO]2 (B) K = [Hg][O2] / [HgO] (C) K = [Hg]2[O2] (D) K = [O2] (A) 2.8 x 10¯8 (B) 3.6 x 10¯7 (C) 6.0 x 10¯4 (D) 2.8 x 106 30. Consider this equilibrium, for which ΔH < 0. HgO(s) + 4I¯(aq) + H2O(l) <===> HgI42¯ + 2OH¯ Which changes will increase the equilbrium concentration of HgI42¯? 36. For which titration would the use of phenophthalein introduce a significant error? Kindicator for phenolphthalein = 1 x 10¯9 I Increasing the mass of HgO(s) present II Increasing [I¯] III Adding 1 M HCI (A) I only (B) II only (C) II and III only (D) I, II, and III 31. The equilibrium constant for this reaction is approximately 10¯3. HPO42¯(aq) + HCO3¯(aq) <==> H2PO4¯(aq) + CO32¯(aq) Which is the strongest conjugate base in this reaction? (A) HPO42¯(aq) (B) HCO3¯(aq) (C) H2PO4¯(aq) (D) CO32¯(aq) (A) 2.2 x 10¯9 (C) 1.8 x 10¯8 32. A weak acid, HX, has Ka = 9.0 x 10¯6. Within which range does the percent dissociation for a 0.01 M HX solution lie? (A) between 1.0% and 10% (B) between 0.10% and 1.0% (C) between 0.01% and 0.10% (D) less than 0.01% 33. Which salt dissolves in water to produce a solution with a pH < 7? (A) NaC2H3O2 (C) AlCl3 37. When solid lead iodide is added to water, the equilibrium concentration of I¯ becomes 2.6 x 10¯3 M. What is the Ksp for PbI2? (B) Ba(NO3)2 (D) KClO4 (B) 8.8 x10¯9 (D) 3.5 x 10¯8 38. When these standard half reactions are combined to give a spontaneous reaction in a voltaic cell, what is the cell voltage? Standard Reduction Potentials, E° Sn (aq) + 2e¯ ---> Sn(s) -0.14 V Ag (aq) + e¯ ---> Ag(s) +0.80 V 2+ + (A) 1.74 V (C) 0.94 V (B) 1.46 V (D) 0.66 V 39. How many moles of elections are transferred when this equation is balanced with the smallest whole number coefficients? _IO3¯ + _H2O2 + _H+ ---> _I2 + _O2 + _H2O (A) 2 (B) 4 (C) 5 (D) 10 40. When anions undergo oxidation, they move toward the A. anode of a voltaic cell and the cathode of an electrolytic cell B. cathode of a voltaic cell and the anode of an electrolytic cell C. anodes of both types of cells D. cathodes of both types of cells 2nd B. N < C < Si D. Si < N < C 1.31 3.39 3rd 4th 5.30 7.47 5th 6th 2 2 2 B. 3 2 0 C. 3 1 2 D. 3 0 4 46. In the Lewis structure for the BrF4¯ ion, how many lone pairs of electrons are placed around the central atom? (B) 1 (C) 2 (D) 3 47. What term is used for the measure of an atom's attraction for the electrons that constitute a covalent bond? 42. These are the first eight ionization energies for a particular neutral atom. All values are expressed in MJ mol¯1. How many valence electrons does this atom possess? 1st A. (A) 0 41. When the elements C, N and Si are arranged in order of increasing first ionization energy, which is the correct order? A. C < N < Si C. Si < C < N sigma bonds pi bonds lone pairs of electrons 7th 8th 10.99 13.33 71.33 84.01 (A) ionization energy (C) electron affinity (B) bond dissociation energy (D) electronegativity 48. One way of writing the Lewis structure of the cyanate ion, OCN¯, places one double bond between the carbon atom and the oxygen atom and another double bond between the carbon atom and the nitrogen atom. What are the formal charges on the oxygen, carbon, and nitrogen atoms, respectively for this structure? (A) 0, 0, -1 (C) -1, +1, -1 (B) -1, 0, 0 (D) -2, 1, 0 49. Which pair are two different names for the same compound? 43. Which gaseous ion in its ground state has the greatest number of unpaired electrons? (A) acetic acid and ethanoic acid (B) formaldehyde and methanol (C) isopropyl alcohol and 1-propanol (D) ethene and ethyne A. Mn3+ 50. High solubility of an ionic solid in water is A. 1 B. 2 C. 4 B. Fe3+ D. 6 C. Co3+ D. Ni3+ 44. Which of these characteristics describe the PCl3 molecule? I trigonal planar shape II sp3 hybridized phosphorus atom III polar bonds IV nonpolar molecule A. I and II only C. I and IV only B. II and III only D. I, III, and IV only 45. According to the Lewis structure for the HNNH, how many sigma bonds, pi bonds, and lone pairs of electrons are present? favored by which of the following conditions? I. The existence of strong ionic attractions in the crystal lattice II. The formation of strong ion-dipole attractions III. An increase in entropy upon dissolving (A) I only (C) II only (B) I and II only (D) II and III only