1. A colorless aluminum salt, soluble in water which is used in paper industry, tanning and water purification a. Alum b. D 2. As water boils, the temperature a. Increases b. Remain constant at 100⁰C 100⁰C until all is changed changed to vapor 3. Saltwater boils at a. Slightly higher than 100⁰C b. 100⁰C c.
Slightly lower than 100⁰C
4. Steps in formation of PVC a. Calcium carbide – vinyl chloride – PVC b. Calcium carbine – acetylene – vinyl chloride – PVC 5. Buffer solution resists changes in acidity. If an acid is added to a buffer solution, the ___ remains the same a. pH b. concentration c.
temperature
6. Specific volume of compressed air at 150 bars at 160 K 7. Viscosity of compressed air at 125 bars and 200 K 8. The temperature of compressed air with a specific enthalpy of 50.05 kJ/kg and 70 bar s a. 150 K b. Nearly 160 K 9. An ideal gas in a piston at 5000 psia expands isothermally against a resisting pressure of 500 psia until its volume is doubled. Find the work done. 10. Jellies and paints are examples of a. Gel b. Emulsion c.
Sol
11. Which is not a derivative of benzene? a. Phenanthnene b. Ethylbromide c.
Anthrocene
12. Which determines the characteristics of a hydrocarbon? a. Number of carbon atoms b. Types of carbon bonds c.
Number of hydrogen atoms
13. 41.6 g of aluminum is mixed with HCl. The gas liberated from this reaction is passed with copper oxide. How much copper is formed with this reaction? 14. A 32 g of compound X is mixed with 450 g CCl4. Find the molecular weight of the compound if
the boiling point rise is 6.21⁰C, K=5.03
For the synthesis of ammonia N2 + H2 = NH3 Percent yield of ammonia (by volume) Temperature 30 atm
100 atm
200 atm
200⁰C
67.6%
81.5%
90.0%
400⁰C
10.2%
25.1%
47.0%
600⁰C
1.7%
4.5%
3.8%
15. What is the partial pressure of ammonia at 30 atm, 400⁰C? 16. What is the partial pressure exerted by nitrogen at 100 atm, 200⁰C? 17. What is the Kp at 30 atm, 400⁰C 18. Who gave the name of oxygen? a. Priestly b. Scheele 19. Discovered water by exploding H2+O2 a. Lewis b. Lavoisier c.
Scavendish
d. Usey 20. The most component of pitchblende? a. Uranium 21. What is the molarity of KH(IO3)2 with a mass of 2.5 g and volume of 500 mL? 22. What expressions of concentration are independent of temper ature? a. Molality and mole fraction b. Molarity and normality c.
Molarity and mole fraction
23. Which dissolves fastest in coffee? a. Lump sugar in hot coffee b. Granular sugar in hot coffee c.
Granular sugar in cold coffee
d. Lump sugar in cold coffee 24. How many millimeters of 6.0 M HCl needed to prepare 250 mL of 1.2 M HCl? 25. 184 g of ethanol is mixed with 1 gmol glycerol. What is the vapor pressure o f resulting solution if the vapor pressure of ethanol at the working temperature is 200 mmHg? Assume that glycerol is nonvolatile. 26. How much heat is required to raise 4000 g of methanol from 2 t o 220⁰C (Cp of methanol is 0.6
cal/g⁰C) 27. At equilibrium, a 1 L PCl5 is found to contain (in mole/L)
PCl5 = 7.05 PCl3 = 0.54 Cl2 = 0.54 Find the equilibrium constant 28. What is the color of nickel chloride? a. White b. Yellow c.
Green
d. Red 29. What is the molecular weight of ammonium perchlorate? 30. Naming H2C=C-C=C | CH3 a.
Isoamylene
b. Isoprene 31. A barometer is a. Sealed-end manometer b. Open-ended manometer 32. A carbon compound is a. One carbon and one oxygen bounded by a double bond b. One carbon and one oxygen bounded by a single bond c.
One carbon and two oxygen bounded by one single and one double bond
d. One carbon and two oxygen bounded by two double bonds 33. Water flows down at 1000 gal/min. If 80% of the energy produced can light 100 75-W bulbs for 60 secs, what is the height of the pipe through with the wate r flows? a. 49.73 ft 34. The best indicator to be used in the filtration of a weak acid and a strong base is a. Phenolphthalein b. Methyl orange c.
Bromthymol blue
35. It required 82 mL H2SO4 to neutralize 12.0 g NaOH. What is the molarity of H2SO4 36. A 620 mg ideal gas occupies 175 cc at STP. What is the molecular weight of the ideal gas? a. 79 37. A 0.1M acetic acid is found to cont ain 1.32 x 10-3 mol/L of H+ at equilibrium. What is the ionization constant? 38. A 2 L flask is filled with 0.2 mol of HO. It is allowed to reach equilibrium at high temperature. If at equilibrium the flask was found to contain 0.078 M HI, what is the Kc? 39. The percentage abundance of Xe in the atmosphere (% volume is a. 1.4 x 10-4 b. 8.0 x 10-6 c.
1.32%
d. 0.93%
40. Brix scale is used for a. Sugar solutions b. LPG c.
Petroleum
d. Water 41. The first step in precipitation is the formation of ____ a. Nuclei 42. Cr(NH3)5SO4Cl represent ___ atoms a. 27 b. 12 43. The mass contribution of an electron in an atom is a. 1/1,837 that of the proton b. equal to that of a proton c. equal to that of the neutron 44. An atom is __________ a. Electrically positive spherical species with a neutral center and negatively charged electron. b. An electrically positive spherical species with a positive center and negatively charged electron c. An electrically neutral spherical species with a neutral center and negatively charged electron. d. An electrically negative spherical species with a positively charged center and negatively charged elections. 45. Along a row in the periodic table elements have the same a. energy b. configuration c. size 46. The electrons of metals are free to move in a solid. This explains why a. metals are unstable b. metals can be easily molded c. metals have high reflectivity d. metals have high conductivity 47. A 4.256 grams compound is dissolved in 100 grams toluene. What is the molecular weight (MW) of the compound if the vapor pressure of the solution in 28.209? The vapor pressure of toluene at the working temperature is 28.829 mmHg. Assume that the compound is a nonvolatile, non-dissociating solute. 48. A flue gas is analyzed to contain (dry basis): 11.6% CO2, 6.8% O2, 0.5% CO and leaves the boiler at 5380K. The inlet air is at 2870K and the fuel contains 29.4% C. What is the amount of heat carried by the flue gas per kg of fuel burnt? The mean heat capacity of the flue gas is 1.005 kJ/kg 0K. 49. Which of the following represents reduction? a. ethanol ---> ethanaldehyde b. acetylene ---> ethylene
50. What are the products of destructive distillation? a. coal tar, coal gas, ammonia b. coal gas, ammonia, graphite 51. Which of the following is insoluble in H20? a. aluminum sodium silicate b. aluminum sulfate c. ammonium oxalate d. ammonium bromide 52. A compound is found to contain by mass: 22.79% C, 1.42% H and 75.9% Br. What is the molecular formula of the compound if its molecular weight is 422? a. C4H6Br4 b. C2H3Br2 53. Defines a base as a compound that dissolves in water to produce OH- is a. Arrhenius b. Bronsted-Lowry c. Lewis 54. Defines an acid as a compound that dissolves in water to produce H+ ions is a. Arrhenius b. Bronsted-Lowry c. Lewis 55. One gmole of a species is that weight of the species equal to its a. molecular weight b. atomic mass 56. Arrange Ca, Be and Mg according to increasing size a. Ca < Mg < Be b. Be < Mg < Ca c. Ca < Be < Mg d. Mg < Ca < Be 57. Arrange Ca, Be and Mg according to increasing ionization energy a. Be < Mg < Ca b. Mg < Ca < Be c. Ca < Mg < Be d. Ca < Be < Mg 58. Arrange Ca, Be and Mg according to increasing electron affinity a. Mg < Ca < Be c. Ca < Be < Mg c. Be < Mg < Ca d. Ca < Mg < Be 59. 19.6 grams of Carbon Disulfide is reacted with excess oxygen to form carbon dioxide and sulfur dioxide. What is the amount of sulfur dioxide formed? a. 32 grams 60. The ionization constant of NH4 OH is 1.8 x 10-5. What is the formality of a solution of NH4OH which is 1.3% ionized? a. 0.10 61. A uniform current deposits 0.6332 grams of Ag in 90 minutes. The 45.2 mL volume of H2 at 25 degC and 740 mm measured over water it would liberate in 60 minutes is
a. 50.8 mL b. 60.2 mL c. 30.5 mL d. 45.2 mL e. None of the above 62. A compound has the following percent composition: Na-19.3%, S-26.9%, O-53.8%. Its molecular mass is 238. Derive its molecular f ormula. a. NaSO4 b. Na2SO4 c. Na2S2O8 d. Na2SO3 e. NaSO3 63. In the flow processes, neglecting KE and PE changes, the expansion -? PV represents a. heat transfer b. shaft work c. closed system work d. enthalpy change e. none of the above 64. If 0.680 gram of an unknown acid, H2B, required 25 mL of 0.125 N NaOH, the equivalent weight of the acid is a. 229.8 b. 459.6 c. 435.2 d. 217.6 e. 333 65. From which of the given alkanes should be easiest to prepare a single pure monochloro product? a. n-butane b. isobutene c. n-hexane d. cyclohexane e. isohexane 66. Thermolar solubility of salt AB2 with Ksp = 10^-12 is a. 6.29 x 10^ –5 b. 1 x 10^–4 c. 3.16 x 10^ –4 d. 7.93 x 10^ –5 e. 2 x 10^ –3 67. A 0.2 molal solution of KCl freezes at –0.680 degC. The osmotic P at 0 degC is a. 7.3 atm b. 6.5 atm c. 8.2 atm d. 5.6 atm e. none of the above 68. Which of the following aqueous salt solution will have a pH below neutral value? a. NaACO
b. Na2CO3 c. Na2S d. KCl e. none of the above 69. For HOAc, the melting point at 1 atm is 16.61 degC. Delta Hf = 2800 cal/mol, Delta Vf = 9.614 cal/mol. What is the melting point at 11 atm? a. 16.61 degC b. 17.24 degC c. 9.02 degC d. 16.85 degC e. none of the above 70. In following pair of elements, the pair belonging to metalloids is a. B and C b. Ca and Mg c. P and S d. As and Te e. K and Sr 71. In the titration of water sample using double indicator, the volume of standard acid required for the methyl orange end point is equal to the volume required for the phenolphthalein end point. The impurity (ies) is a. NaOH only b. Na2CO3 only c. NaHCO3 only d. Na2CO3 and NaOH e. Na2CO3 and NaHCO3 72. If equal volumes of saturated silver chloride and silver bromidesolution are mixed a. silver chloride will precipitate b. silver bromide will precipitate c. silver chloride and silver bromide will precipitate d. there will be no precipitate e. none of the above 73. 3000 cfm of 65 degF air is required to maintain a house at 76 degF. 25% of the air entering the air conditioner is from outside at 90 degF and the remainder is recycled from inside at 76 degF. Determine the rating in tons of airconditions. (Assume sensible heat changes only and ignore dehumidification). a. 3.95 b. 9.8 c. 2.68 d. 4.05 e. none of the above 74. Which of the following gases has lifting power? a. nitrogen b. oxygen c. sulfur trioxide d. all of the above e. none of the above
75. The relative abundance of 2 naturally occurring isotopes of boronof atomic weights 11.009 and 10.01 is 80.80% and 19.80% respectively. Calculate the relative average atomic weight of boron. a. 19.5 b. 10.81 c. 10.00 d. 11.4 e. 11.00 76. A solution of a weak acid and its salt which resists appreciable change In pH value is called a. normal solution b. colloidal solution c. neutral solution d. buffer solution e. molal solution 77. Ideally, in a chromatographic technique, the individual compound in a sample will a. leave the adsorbent on a different physical state than in which they entered it b. become separated from each other as they pass through theadsorbent c. become bonded to one another d. attach irreversibly to the adsorbent e. none of the above 78. The atom with the highest first ionization energy is a. sodium b. phosphorus c. chlorine d. aluminum e. potassium 79. If the repulsive forces are dominant, the compressibility factor, z, is a. greater than 1 b. less than 1 c. equal to one d. cannot be determined e. none of the above 80. 10.5 L of N2 at 75 degC and 760 mmHg are bubbled through an aqueous solution of a non volatile solute, whereby the solution loses 0.2455 grams in weight. If the total P above the solution is 760 monthly, what is the mole fraction of the solute in the solvent? a. 0.982 b. 0.018 c. 0.653 d. 0.347 e. none of the above 81. Mathematically, a thermodynamic property is a. A point function b. A path function c. Exact differential d. Discontinuous e. None of the above
82. The pH of a 0.10 M ammonium chloride solution is a. 6.37 b. 5.62 c. 6.88 d. 5.12 e. 7.3 83. For all spontaneously occurring processes in an isolated system, which expression best describes dS? a. dS = dQ/T b. dS = 0 c. dS > 0 d. dS < 0 e. none of the above 84. The total number of possible structures corresponding to the formula C4H7Br is a. 6 b. 7 c. 9 d. 10 e. 12 85. Which of the following quantum numbers for electrons could not occur? a. 3, 2, 2, +1/2 b. 3, 0, -1, +1/2 c. 1, 0, 0, -1/2 d. 2, 1, -1, +1/2 e. 4, 0, 0, -1/2 86. Ortho and para orienting substituents enhances the rate of electrophilic substitution reactions except in the case of a. methyl group b. hydroxyl group c. carboxyl group d. amino group e. ethyl group 87. Equilibrium conditions exist in all except which of the following? a. in a reversible process b. in processes where driving forces are infinitesimal c. in a steady state flow process d. when nothing can occur without an effect on the system e. none of the above 88. What volume of 0.56 N HCl must be added to 1 L of a 0.10 N HCl in order to obtain a solution that is 0.15 N as an acid? a. 132 mL b. 122 mL c. 120 mL d. 130 mL e. 125 mL
89. Which of the following statements is correct? a. Galvanic cells can be used in rechargeable batteries only when the overall reaction is reversible. b. Na+ his above Mg2+ in the standard reduction potentials. This means that Na+ will reduce Mg2+ to Mg. c. Cell diagrams generally give the cathode first. d. In the electrolysis of CuSO4, one Faraday of electricity is required to produce 1 mole copper e. None of the above. 90. During the adiabatic expansion of an ideal gas, work is done by the system and its delta U a. decreases b. increases c. does not change d. all of these e. none of the above 91. Given the equilibrium reaction at 250 ?C and 1 atm, PCl5 (g) <-> PCl3 (g) + Cl2 (g). The density was found to be 4.4 g/L. The fraction of PCl5 dissociates is a. 0.81 b. 0.093 c. 0.103 d. 0.42 e. none of the above 92. The solubility product constant is valid: a. for all soluble compounds b. for all insoluble salts c. only of saturated solutions d. only for fairly insoluble electrolytes e. only for fairly soluble electrolytes 93. 55,000 gallons of water passes through a heat exchanger and absorbs 28,000,000 Btu. The exit temperature is 110 degF. The entrance water temperature is nearest to a. 49 b. 56 c. 68 d. 73 e. none of the above 94. If 5.0 grams of KMnO4 are dissolved in 1 L solution, the normality when used for titration in acid medium is a. 0.0316 b. 0.2215 c. 0.1582 d. 0.0949 e. 0.4469 95. The maximum thermal efficiency that can be obtained in an ideal reversible heat engine operating between 300 degC and 100 degC is a. 0.67 b. 0.35
c. 0.54 d. 0.82 e. none of the above 96. Which of the following statements is not correct? a. The absolute temperature of a gas is directly proportional to its volume at constant P. b. Nitrogen will diffuse faster than oxygen gas at fixed T & P. c. The product of P & V of a fixed amount of gas is constant. d. Most gases are cold during a free adiabatic expansion. e. None of the above 97. A compound whose molecules are not associated by H-bonding is a. CH3OH b. CH3NH2 c. (CH3)3N d. HCOOH e. HCONH2 98. The most probable valence of an element with an electronic configuration of 1s2 2s2 2p6 3s2 3p5 is a. +1 b. +2 c. +3 d. –2 e. –1 99. The process that has no heat transfer is called a. isentropic b. isothermal c. quasistatic d. polytropic e. none of the above 100. A 1.0 gram sample of impure K2CO3 is taken for analysis. Thesolution of the dissolved sample required 58.10 mL of 0.14 N HCl. However, 0.65 mL of NaOH was needed for back titration (1 mL of HCl is equivalent to 2.60 mL NaOH). Calculate the purity of the sample expressed as % K2O. a. 38.14% b. 40.23% c. 34.4% d. 42.1% e. 36.7% A carnot engine with thermal efficiency of 40% rejects 3000 KJ at a temperature of 101. 1200 degC. The combustion of 1 L gasoline (sp. gr. = 0.8, cv = 46.8 KJ/g) furnishes heat to the engine. The maximum work done by the engine is a. 5000 KJ b. 3000 KJ c. 2000 KJ d. 10,000 KJ e. none of the above
102. The percent sulfur in barium sulfate is: a. 34.30 b. 13.74 c. 58.85 d. 65.70 e. 76 103. Which of the following is incorrectly named? a. p-chloro aniline b. 3-methyl pentane c. methylbenzene d. ethyl benzene e. 2-ethyl butane 104. In the reaction H2O2 + KI -> KOH + I2, hydrogen peroxide acts as: a. catalyst b. oxidizing agent c. solvent d. reducing agent e. none of the above 105. The Volhard method, a volumetric technique for the determination of silver, uses which of the following indicators? a. Eosin b. Fluorescein c. Ferric Alum d. Potassium Chromate e. Ferroin 106. The proper sequence of steps for the conversion of benzene to 3-nitro toluene is: a. nitration, then Friedel Crafts Alkylation b. Friedel Crafts Alkylation, then nitration c. Simultaneous nitration and alkylation d. Any order will do e. None of the above 107. The state of a thermodynamic system is always defined by its a. absolute temperature b. process c. degrees of freedom d. nature e. none of the above 108. Following Markonikoff rule, when 1 butene is reacted with HOCl, the main product is: a. n-butane b. 1-chloro-2-butanol c. 2-butanol d. 2-chloro-3-butanol e. 2-chloro butane 109. Equation of state for a single component can be any of the following except a. ideal gas law b. Z=PVm/RT
c. Any relationship interrelating 3 or more state functions d. A mathematical expression defining a path between states e. None of the above 110. The percent of MnO2 (MW=86.94) in a 0.5 gram sample, which after addition of 50.0 mL of 0.1 N ferrous sulfate solution required 16.0 mL 0.08 N potassium dichromate for back titration. a. 16.17 b. 32.34 c. 48.51 d. 64.68 e. 40
. Cr(NH3)5SO4Cl represent ________ atoms. a. 27 c. b. 12 c. ???
