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PREBOARD EXAM (PHYSICALAND CHEMICAL PRINCIPLES) 1) _______ is the conversion of molecular nitrogen into nitrogen compounds. a) Nitrogen fixation c) Nitrite reduction b) Denitrification d) Industrial fixation 2) Above the stratosphere, the concentration of ozone and other gases is low, and the temperature decreases with increasing altitude a) Troposphere c) mesosphere b) Stratosphere d) ionosphere 3) The layer of the atmosphere that contains about 80 percent of the total mass of air and practically all of the atmosphere’s water vapor. a) Troposphere c) mesosphere b) Stratosphere d) ionosphere 4) Above the troposphere, is the ________, which consists of nitrogen, oxygen, and ozone. The air temperature rises with altitude. a) Troposphere c) mesosphere b) Stratosphere d) ionosphere 5) The incoming streams of solar protons and electrons are oriented by Earth’s magnetic field so that most auroral displays occur in doughnut-shaped zones about 2000km in diameter centered on the north and south poles. __________ is the name given to his phenomenon in the Northern Hemisphere. a) Aurora borealis c) both a and b b) Aurora australis d) none of these 6) An international treaty -________- was signed by most industrialized nations in 1987, setting targets for cutbacks in CFC production and the complete elimination of these substances by the year 2000. a) Stockholm Convention c) Kyoto Predict b) Kyoto Protocol d) Montreal Protocol 7) Extracting the metals often entails _________-that is, heating the metal sulfide in air to form the metal oxide and sulfur dioxide. a) Galvanizing c) Smelting b) Vulcanizing d) Mining 8) A curie corresponds to _______ disintegrations of radioactive nuclei per second a) 3.70 x 10^7 c) 3.70 x 10^9 b) 3.70 x 10^8 d) 3.70 x 10^10
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PREBOARD EXAM (PHYSICALAND CHEMICAL PRINCIPLES) 9) _______ is a rather disagreeable-smelling preservative for laboratory specimens. a) Acetaldehyde c) Methanal b) Methanol d) Valeraldehyde
liquid
used
10) Reactions proceeds spontaneously at low temperatures. temperatures, the reverse reaction becomes spontaneous. a) + Δ H and + ΔS c) - Δ H and + ΔS b) - Δ H and – ΔS d) + Δ H and - ΔS
as
At
a
high
11) Geometrically, ________ is the most symmetrical molecule known. a) Buckminsterfullerene c) fullerenes b) Graphite d) Buckytubes 12) Alcohol boils t 79oC and H2O boils at 100oC at 1atm pressure. A mixture of the two will have a boiling point a) lower than 79oC c) higher than 79oC b) higher than 100oC d) between 79oC and 100oC 13) What determines the degree of completeness of a reaction? a) catalyst c) rate of reaction b) intimacy of d) equilibrium constant 14) What is the substance called that causes an alteration of the speed of a chemical reaction? a) variable c) catalyst b) gas d) equilibrium constant 15) What substance does not have catalytic capability, but does increase the effectiveness of a catalyst? a) enzyme c) anti-catalyst b) promoter d) true constant 16) Who first proposed the atomic theory? a) John Dalton c) Lord Kelvin b) Julius Robert d) William Thomson 17) What is the temperature at which slightly exceeds the pressure of a) absolute zero c) b) boiling point d) 18) What theory states that equal same number of molecules when a) Quantum Theory b) Kinetic Theory
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the vapor pressure of a liquid the atmosphere above the liquid? Kelvin melting point
volumes of different gases contain the compared under the same conditions. c) Molecular Law d) Avogadro's Law
PREBOARD EXAM (PHYSICALAND CHEMICAL PRINCIPLES) 19) Who first came up with the periodic table? a) Amedeo Avogadro c) Charles Darwin b) Dmitri Mendeleev d) Isaac Newton 20) What is the number of the element on the Periodic Table called? a) periodic number c) quantum number b) element number d) atomic number 21) Who invented the X-ray? a) Wilhelm Conrad Roentgen b) Marie Curie
c) Pierre Curie d) Ernest Rutherford
22) Who's theory proposed that electrons are arranged in shells, or quantum levels, at a distance from the nucleus? a) Rutherford c) Bohr b) Newton d) Davis 23) What was Melvin Calvin was known for his study of? a) x-rays c) magnetics b) photosythesis d) boiling point 24) What are chemical changes in organic substances caused by the action of enzymes called? a) reaction c) enzymiphication b) oxidation d) fermentation 25) What compounds are formed by the reaction of acids and alcohols? a) ethers c) esters b) enzymes d) bases 26) Who was key to developing the valence theory? a) Melvin Calvin c) Sir Edward Franklin b) Henry Dow d) Humphry David 27) Who invented vulcanization for the rubber industry? a) Charles Goodyear c) Robert Michelin b) James Firestone d) Albert Brookstone 28) What process combines rubber and sulfur at a high temperature? a) fulmination c) fermentation b) vulcanization d) distillation 29) Who won the 1944 Nobel Prize in chemistry for his work in nuclear fission? a) Fritz Straussmann c) Otto Hahn b) Joseph Lussac d) Johann Glauber 30) Who invented the Carbon-14 dating method? a) Irving Langmuir c) August Hofmann b) Williard Libby d) Otto Hahn
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PREBOARD EXAM (PHYSICALAND CHEMICAL PRINCIPLES)
31) What is the ability of a solid substance to resist abrasion and surface deformation called? a) hardness c) conductivity b) softness d) tensile strength 32) What is the resistance to breakage called? a) hardness c) malleability b) elasticity d) tensile strength 33) What is the ability to return to the original shape after being deformed called? a) hardness c) malleability b) elasticity d) tensile strength 34) What is the ability to be shaped called? a) hardness c) malleability b) elasticity d) tensile strength 35) A 0.8040-g sample of an iron ore is dissolved in acid. The iron is then reduced to Fe+2 and titrated with 47.22 mL of 0.02242 M KMnO4 (158.04g/mol) solution. Calculate the results of this analysis in of %Fe (55.847g/mol). a) 22.06% b)36.77% c)14.71% d)44.12% 36) A 0.992-g sample of canned tuna was analyzed by the Kjeldahl method; 22.66 mL of 0.1224 M HCl were required to titrate the liberated ammonia. Calculate the percentage of Nitrogen in the sample. a) 11.74% b)7.83% c)3.91% d)0.28% 37) Calculate the pH of a buffer prepared by adding 10 mL of a 0.10 M acetic acid to 20 mL of 0.10 M sodium acetate. (Ka = 1.75^-5) a) 5.06 b)4.46 c)9.54 d)6.02 38) What is the pH of an aqueous solution that is 14.0% HCl (36.46g/mol) by weight and has a density of 1.054 g/mL? a) -0.573 b)-0.507 c)-0.673 d)-0.607 39) What is the pH of the resulting solution made by mixing 25 mL of 0.1 M HCl and 15 mL of 0.1 M NaOH? a) 1.40 b)1.60 c)1.00 d)0.40 40) The Zn in a 0.7556-gram sample of foot powder was titrated with 21.27 mL of 0.01645 M EDTA. Calculate the percent Zn (65.37g/mol) in this sample. a) 2.87% b)2.95% c)3.03% d)3.18%
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PREBOARD EXAM (PHYSICALAND CHEMICAL PRINCIPLES) 41) A 0.7121 g sample of wheat flour was analyzed by the Kjeldahl method. The ammonia formed by addition of concentrated base after digestion with H2SO4 was distilled into 25.00 mL of 0.04977 M HCl. The excess HCl was then back titrated with 3.97 mL of 0.04012 M NaOH. Calculate the percent protein in the flour (f = 5.70) a) 12.16% b)24.32% c)12.79 d)6.40% 42) Calculate the pH of a 0.010 M solution of NaCN. (Ka = 7.2^-10) a) 11.57 b)10.57 c)12.57 d)9.57 43) Using the equilibrium constants given for reactions (1) and (2), what is the equilibrium constant for reaction (3)? (1) 2NO(g) + O2(g) → N2O4(g) Kp = 1.49 × 10^13 (2) 2NO(g) + O2(g) → 2NO2(g) Kp = 1.66 × 10^12 (3) N2O4(g) → 2NO2(g) a) 0.0123 b) 0.111 c) 8.98 d) 80.3 44) Calculate the difference in calories between G and A at 25C the reaction: H2 (g, 1atm) + 1/2 O2 (g, 1 atm) H2O(l) a. –256 cal
b. –888 cal
c. –904 cal
for
d. –1058 cal
45) A liquid is observed to boil at 120C under a pressure of 725 mm Hg. Its molar heat of vaporization is 8200 cal/mol. Calculate the normal boiling point of the liquid. a. 121.76C b. 120.80C c. 118.16C d. 112.54C 46) A 0.01 molal solution of K3Fe(CN)6 freezes at –0.062C. What is its apparent degree of dissociation? d. 78% a. 25.9% b. 47.2% c. 67.2% 47) How many grams of urea must be added to 4000 grams of water to make the solution boil at 100.32C? b. 150.5 grams a. 75.3 grams c. 185.4 grams d. 205.6 grams 48) What is the solubility of CaF2 in water in mols of CaF2 per L of solution? Ksp for CaF2 is 1.7 × 10^10. a. 9.2×10^—6 M b. 1.3×10^—5 M c. 3.5×10^—4 M d. 5.5×10^—4 M 49) What is the solubility in mol/L of BaF2 in 0.10M MgF2? Ksp for BaF2 = 1.7 × 10^-6. a. 1.7×10^-4 M b. 1.7×10^-5 M c. 4.3×10^-5 M d. 8.5×10^-6 M 50) Oxidation of which of the following compounds can lead to an aldehyde? a. primary alcohol b. secondary alcohol c. tertiary alcohol d. ether 51) Oxidation of which of the following compounds can lead to ketone? a. primary alcohol b. secondary alcohol c. tertiary alcohol d. ether
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PREBOARD EXAM (PHYSICALAND CHEMICAL PRINCIPLES) 52) Hydrolysis of an ester leads to two compounds. Which of the following pairs compounds is formed from such a hydrolysis? a. An alcohol and an aldehyde c. An alcohol and a carboxylic acid b. Two alcohols d. A ketone and a carboxylic acid 53) Which of the following compounds would you expect to be the most soluble in water? a. CH3CH2CH2CH2CH2CH2CH2CH3 c. CH3CH2CH2CH2CH2CH2CH2OH b. CH3CH2CH2OH d. CH3CH2CH2-O-CH2CH2CH3 54)
Which of nature of a. A soap b. A soap c. A soap d. A soap
the following is the best definition of the chemical soap? is a very long molecule. is a long chain carboxylic acid. is an ester of glycerol and a long chain carboxylic acid. is a salt of a long chain carboxylic acid.
55) The molecule among those in the following list that can be classified as an amide is a. CH3NH2 b. CH3CONH2 c. CH3CHO d. CH3COOH 56) Which of the following amino acids has sulfur in the R group? a. Serine b. Cysteine c. Asparagine d. Tyrosine 57) Triglycerides which are solids or semisolids at room temperature are called: a. oil b. Fat c. Steroid d. Cholesterol 58) One ml of a bacterial culture was pipetted into a 9 ml dilution blank. One-tenth ml of this dilution was pipetted into a 9.9 ml dilution blank. From this dilution, one-tenth ml was plated with 25 ml of culture medium. 220 colonies arose after incubation. How many colony-forming units were present per ml of the original culture? a. 2.2 x 10^6 b. 2.2 x 10^5
c. 2.2 x 10^4
d. 2.2 x 10^7
59) The Philippine cornstarch Corporation prepares pharmaceutical glucose from cornstarch by enzyme hydrolysis. It was observed that when the starch concentration of the slurry was 5%, the rate of conversion of starch to glucose was 0.04 kg/s. When the starch concentration was made 10%, the turnover rate was 0.07 kg/s. The maximum production level of glucose that can reasonably be attained per shift of 8 hours is a. 6084 kg
b. 8064 kg
c. 1008 kg
d. 0.28 kg
60) An act to Control Toxic Substances and Hazardous and Nuclear Wastes providing penalties for violation thereof a. RA 8749
b. RA 9003
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c. RA 9275
d. RA 6969
PREBOARD EXAM (PHYSICALAND CHEMICAL PRINCIPLES) 61) The difference between the actual property value of a solution and the value it would have as an ideal solution at the same T and P and composition is called a. Residual
b. Excess
c. Partial property
d. Gibbs free energy
62) A certain quantity of nitrogen gas collected over water at 20C and at a total pressure of 745 mm Hg has a volume of 200 mL. What will be the volume of the nitrogen in a completely dry state at 780 mm Hg pressure and at 48C. The vapor pressure of water at 20C is 17.54 mm Hg. d) 204.34 mL a) 211.45 mL b) 209.27 mL c) 206.75 mL 63) Among the following processes, all of the following will produce an alkane from an alkyl halide except a) Wurtz Synthesis c) Reduction with Zn b) Hydrogenation d) Corey-House Synthesis 64) The following are correctly named except a) 3-ethylpentane c) N-methylbutanamide b) p-dichlorobenzene d) 5-hexanone 65) Aromatic compounds are characteristics of a) Electrophilic substitution c) Nucleophilic substitution b) Electrophilic addition d) Electrophilic addition 66) Delocalization of pi electrons a) Rearrangement c)hyperconjugation b) isomerism d)resonance 67) Hydration of alkynes yields a) epoxide b) ketone c) alcohol
d) ether
68) The sequence of steps to produce o-nitrobenzoic acid from benzene is (1) Friedel-Crafts Alkylation (2) Nitration (3) Oxidation a) 123 b) 132 c) 213 d) 231 69) Markovnikoff’s addition of HBr to alkynes dominantly produces a) Geminal dihalide c) tetrahalide b) Vicinal dihalide d) halohydrin 70) Ozonolysis of alkenes gives a/an a) aldehydes b) alcohol c) ether
d) ester
71) Which of the following reactions will yield an alcohol from alkenes? a) Oxymercuration-Demercuration c) Hydroxylation b) Hydroboration-Oxidation d) all of the above
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PREBOARD EXAM (PHYSICALAND CHEMICAL PRINCIPLES) 72) Which of the following compounds has the highest boiling point? a) N-pentane b) isopentane c) neopentane d) isobutene 73) A sequence in which a C=C double bond is oxidatively converted to two carbonyl groups through sequential treatment with O3, followed by Zn in acetic acid a) Oxidation c) Oxymercuration-Demercuration b) Ozonolysis d) Hydroboration-Oxidation
74) An addition reaction initiated by attack by an electron-deficient reagent (an electrophile), often a proton from a hydronium ion a) Electrophilic Addition c) Oxidation b) Nucleophilic Addition d) Ozonolysis 75) A reaction sequence used to alkene; initiated by concerted syn with basic hydrogen peroxide a) Oxidation b) Ozonolysis
achieve anti-Markovnikov hydration of an addition of borane, followed by oxidation c) Oxymercuration-Demercuration d) Hydroboration-Oxidation
76) What is the common name of this compound – C6H5OCH3? a) Aniline b) Styrene
c) Cumene d) Anisole
77) The influence of mixing of s and p s character of the hybrid orbital, the a) Hybridization c) b) Hybrid Orbitals d)
orbitals; the greater the fraction of more electronegative is the atom Hybridization Effect Hybrid
78) Name the Alkane CH3 CH3
H 2C
CH H 3C
CH CH
CH3
a) b) c) d)
2-ethyl-3,4-dimethylpentane c) 3,4,5-trimethylhexane 4-ethyl-2,3-dimethylpentane 2,3,4-trimethylhexane
CH3
79) Name the Alkane CH3 CH3
CH H 3C
CH
a) b) c) d)
2-methyl-3-bromobutane 2-methyl-2-bromobutane 2-bromo-3-methylbutane 3-bromo-2-methylbutane
Br
80)A homolytic substitution of halogen for hydrogen, often in an alkane a) Nucleophilic substitution c) Electrophilic aromatic substitution b) Free radical substitution d) Electrophilic addition
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PREBOARD EXAM (PHYSICALAND CHEMICAL PRINCIPLES) 81) Name the Alkene H C H 3C
a) b) c) d)
CH3 C
2-methyl-2-butene 1,2-dimethylpropene 3-methyl-2-butene none of the above
CH3
82) Name the Alkene CH3 H2 C
C
H 3C H 2C
C
CH3
a) b) c) d)
Z-3,4-dimethyl-3-hexene Z-3,4-diethyl-3-hexene E-3,4-dimethyl-3-hexene E-3,4-diethyl-3-hexene
CH3
83) The alkene formed is the one that is more alkyl substituted. a) Markovnikoff’s Rule c) Saitsev’s Rule b) Hoffman’s Rule d) Huckel’s Rule 84) What is the IUPAC name of this compound? H2 C
F
H 3C
a) b) c) d)
4-ethyl-2-fluoroaniline 4-ethyl-2-fluoroanisole 4-ethyl-6-fluoroaniline 4-ethyl-6-fluoroanisole
NH2
85)What is the major product of the reaction?
a) Aniline b) Benzonitrile
c) Benzene d) Iodobenzene
86)The final product of hydration of an alkyne is a/an __________. a) Enol
b) Alkene
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c) Ketone
d) Alcohol
PREBOARD EXAM (PHYSICALAND CHEMICAL PRINCIPLES) 87-91) Consider a continuous steady-state process in which the following reactions take place: C6H12 + 6 H2O → 6 CO + 12 H2 C6H12 + H2 → C6H14 In process 250 moles of C6H12 and 800 moles of H2O are fed into the reactor each hour. The yield of H2 is 40.0% and the selectivity of H2 relative to C6H14 is 12.0. 87) What is the limiting reactant? a) Hexane b) Water c) Hydrogen d)Hexene 88) Calculate the molar flow rate (mol/h) of water in the output stream. a) 138.39 b) 453.32 c) 346.68 d) 640
89) Calculate the extent of the first reaction, is a) 53.33
b) 57.78
c) 346.68
90) Calculate the extent of the second reaction, is a) 53.33 b) 57.78 c) 346.68
d) 138.89 d) 138.89
91) Calculate the mole fraction of carbon monoxide in the output stream a) 0.09 b) 0.28 c) 0.21 d) 0.39 92) Balance the chemical equation given K4Fe(CN)6 + H2SO4 + H2O = K2SO4 + FeSO4 + (NH4)2SO4 + CO a) 1,6,6,2,1,3,6 c) 6,3,1,2,6,6,1 b) 2,6,6,2,1,3,6 d) 1,6,6,2,1,2,6 93) ________ is a method of sequencing amino acids in a peptide.[1] In this method, the amino-terminal residue is labeled and cleaved from the peptide without disrupting the peptide bonds between other amino acid residues. a) Markovnikov Degradation c) Lewis Sequencing b) Edman Degradation d) Hall reaction
94) A 5.00 mL aliquot of bleach (density = 1.61 g/mL) was diluted and treated with excess KI to convert hypochlorite to chloride. The liberated I2 required 22.85 mL of 0.214 M Na2S2O3 for titration. Calculate the % ClO– (51.45 g/mol) in the bleach. a)4.18% b) 2.72% c) 1.56% d) 3.12% 95) Balance the chemical equation K4Fe(CN)6 + KMnO4 + H2SO4 = KHSO4 + Fe2(SO4)3 + MnSO4 + HNO3 + CO2 + H2O a) b) c) d)
60,60,188,10,122,299,162,5,122 122,299,162,5,122,60,60,188,10 188,60,60,122,5,162,299,122,10 10,122,299,162,5,122,60,60,188
PREPARED BY: KENSOR ^.^
PREBOARD EXAM (PHYSICALAND CHEMICAL PRINCIPLES)
96) A base mixture sample weighing 976 mg was dissolved in sufficient water to make 100 mL solution and divided into two equal portions. The first portion was titrated with 52.05 mL of 0.1004M HCl to the methyl red end point. The other portion was titrated with 23.02 mL of the acid to the phenolphthalein endpoint. Calculate the % composition of sample. a) 50.16% NaHCO3, 50.20% Na2CO3 c)23.90% NaHCO3, 50.20% Na2CO3 b) 10.38% NaHCO3, 50.20% Na2CO3 d)18.94% NaHCO3, 62.70% Na2CO3 97) The phosphate in a 3000 mg sample of industrial detergent was precipitated by the addition of 1 gram AgNO3. The solution was filtered and the filtrate required 18.23 mL of 0.1377 M KSCN. Calculate the percentage of phosphate in the detergent. AgNO3 (169.87 g/mol) PO4–3 (94.97 g/mol) a)3.56% b) 7.12% c) 5.35% d) 10.69% 98) Calculate the weight of primary standard Na2C2O4 (134 g/mol) necessary to react with 25 mL of 0.2005 M KMnO4 in acidic medium. a)0.671 gram b) 1.343 grams c) 1.679 grams d) 2.687 grams 99) Which of the following types of precipitimetry is used as a direct method for halide determination? a)Mohr method b) Volhard method c) Fajans method d) none of these 100) A 0.0722 M acid has pH of 3.11, what is the Ka of the acid? a)4.2 x 10-6 b) 8.35 x 10-6 c)8.35 x 10-7 d) 4.2 x 10-7
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PREPARED BY: KENSOR ^.^
PREBOARD EXAM (PHYSICALAND CHEMICAL PRINCIPLES) 9) _______ is a rather disagreeable-smelling preservative for laboratory specimens. a) Acetaldehyde c) Methanal b) Methanol d) Valeraldehyde
liquid
used
10) Reactions proceeds spontaneously at low temperatures. temperatures, the reverse reaction becomes spontaneous. a) + Δ H and + ΔS c) - Δ H and + ΔS b) - Δ H and – ΔS d) + Δ H and - ΔS
as
At
a
high
11) Geometrically, ________ is the most symmetrical molecule known. a) Buckminsterfullerene c) fullerenes b) Graphite d) Buckytubes 12) Alcohol boils t 79oC and H2O boils at 100oC at 1atm pressure. A mixture of the two will have a boiling point a) lower than 79oC c) higher than 79oC b) higher than 100oC d) between 79oC and 100oC 13) What determines the degree of completeness of a reaction? a) catalyst c) rate of reaction b) intimacy of d) equilibrium constant 14) What is the substance called that causes an alteration of the speed of a chemical reaction? a) variable c) catalyst b) gas d) equilibrium constant 15) What substance does not have catalytic capability, but does increase the effectiveness of a catalyst? a) enzyme c) anti-catalyst b) promoter d) true constant 16) Who first proposed the atomic theory? a) John Dalton c) Lord Kelvin b) Julius Robert d) William Thomson 17) What is the temperature at which slightly exceeds the pressure of a) absolute zero c) b) boiling point d) 18) What theory states that equal same number of molecules when a) Quantum Theory b) Kinetic Theory
PREPARED BY: KENSOR ^.^
the vapor pressure of a liquid the atmosphere above the liquid? Kelvin melting point
volumes of different gases contain the compared under the same conditions. c) Molecular Law d) Avogadro's Law
PREBOARD EXAM (PHYSICALAND CHEMICAL PRINCIPLES) 19) Who first came up with the periodic table? a) Amedeo Avogadro c) Charles Darwin b) Dmitri Mendeleev d) Isaac Newton 20) What is the number of the element on the Periodic Table called? a) periodic number c) quantum number b) element number d) atomic number 21) Who invented the X-ray? a) Wilhelm Conrad Roentgen b) Marie Curie
c) Pierre Curie d) Ernest Rutherford
22) Who's theory proposed that electrons are arranged in shells, or quantum levels, at a distance from the nucleus? a) Rutherford c) Bohr b) Newton d) Davis 23) What was Melvin Calvin was known for his study of? a) x-rays c) magnetics b) photosythesis d) boiling point 24) What are chemical changes in organic substances caused by the action of enzymes called? a) reaction c) enzymiphication b) oxidation d) fermentation 25) What compounds are formed by the reaction of acids and alcohols? a) ethers c) esters b) enzymes d) bases 26) Who was key to developing the valence theory? a) Melvin Calvin c) Sir Edward Franklin b) Henry Dow d) Humphry David 27) Who invented vulcanization for the rubber industry? a) Charles Goodyear c) Robert Michelin b) James Firestone d) Albert Brookstone 28) What process combines rubber and sulfur at a high temperature? a) fulmination c) fermentation b) vulcanization d) distillation 29) Who won the 1944 Nobel Prize in chemistry for his work in nuclear fission? a) Fritz Straussmann c) Otto Hahn b) Joseph Lussac d) Johann Glauber 30) Who invented the Carbon-14 dating method? a) Irving Langmuir c) August Hofmann b) Williard Libby d) Otto Hahn
PREPARED BY: KENSOR ^.^
PREBOARD EXAM (PHYSICALAND CHEMICAL PRINCIPLES)
31) What is the ability of a solid substance to resist abrasion and surface deformation called? a) hardness c) conductivity b) softness d) tensile strength 32) What is the resistance to breakage called? a) hardness c) malleability b) elasticity d) tensile strength 33) What is the ability to return to the original shape after being deformed called? a) hardness c) malleability b) elasticity d) tensile strength 34) What is the ability to be shaped called? a) hardness c) malleability b) elasticity d) tensile strength 35) A 0.8040-g sample of an iron ore is dissolved in acid. The iron is then reduced to Fe+2 and titrated with 47.22 mL of 0.02242 M KMnO4 (158.04g/mol) solution. Calculate the results of this analysis in of %Fe (55.847g/mol). a) 22.06% b)36.77% c)14.71% d)44.12% 36) A 0.992-g sample of canned tuna was analyzed by the Kjeldahl method; 22.66 mL of 0.1224 M HCl were required to titrate the liberated ammonia. Calculate the percentage of Nitrogen in the sample. a) 11.74% b)7.83% c)3.91% d)0.28% 37) Calculate the pH of a buffer prepared by adding 10 mL of a 0.10 M acetic acid to 20 mL of 0.10 M sodium acetate. (Ka = 1.75^-5) a) 5.06 b)4.46 c)9.54 d)6.02 38) What is the pH of an aqueous solution that is 14.0% HCl (36.46g/mol) by weight and has a density of 1.054 g/mL? a) -0.573 b)-0.507 c)-0.673 d)-0.607 39) What is the pH of the resulting solution made by mixing 25 mL of 0.1 M HCl and 15 mL of 0.1 M NaOH? a) 1.40 b)1.60 c)1.00 d)0.40 40) The Zn in a 0.7556-gram sample of foot powder was titrated with 21.27 mL of 0.01645 M EDTA. Calculate the percent Zn (65.37g/mol) in this sample. a) 2.87% b)2.95% c)3.03% d)3.18%
PREPARED BY: KENSOR ^.^
PREBOARD EXAM (PHYSICALAND CHEMICAL PRINCIPLES) 41) A 0.7121 g sample of wheat flour was analyzed by the Kjeldahl method. The ammonia formed by addition of concentrated base after digestion with H2SO4 was distilled into 25.00 mL of 0.04977 M HCl. The excess HCl was then back titrated with 3.97 mL of 0.04012 M NaOH. Calculate the percent protein in the flour (f = 5.70) a) 12.16% b)24.32% c)12.79 d)6.40% 42) Calculate the pH of a 0.010 M solution of NaCN. (Ka = 7.2^-10) a) 11.57 b)10.57 c)12.57 d)9.57 43) Using the equilibrium constants given for reactions (1) and (2), what is the equilibrium constant for reaction (3)? (1) 2NO(g) + O2(g) → N2O4(g) Kp = 1.49 × 10^13 (2) 2NO(g) + O2(g) → 2NO2(g) Kp = 1.66 × 10^12 (3) N2O4(g) → 2NO2(g) a) 0.0123 b) 0.111 c) 8.98 d) 80.3 44) Calculate the difference in calories between G and A at 25C the reaction: H2 (g, 1atm) + 1/2 O2 (g, 1 atm) H2O(l) a. –256 cal
b. –888 cal
c. –904 cal
for
d. –1058 cal
45) A liquid is observed to boil at 120C under a pressure of 725 mm Hg. Its molar heat of vaporization is 8200 cal/mol. Calculate the normal boiling point of the liquid. a. 121.76C b. 120.80C c. 118.16C d. 112.54C 46) A 0.01 molal solution of K3Fe(CN)6 freezes at –0.062C. What is its apparent degree of dissociation? d. 78% a. 25.9% b. 47.2% c. 67.2% 47) How many grams of urea must be added to 4000 grams of water to make the solution boil at 100.32C? b. 150.5 grams a. 75.3 grams c. 185.4 grams d. 205.6 grams 48) What is the solubility of CaF2 in water in mols of CaF2 per L of solution? Ksp for CaF2 is 1.7 × 10^10. a. 9.2×10^—6 M b. 1.3×10^—5 M c. 3.5×10^—4 M d. 5.5×10^—4 M 49) What is the solubility in mol/L of BaF2 in 0.10M MgF2? Ksp for BaF2 = 1.7 × 10^-6. a. 1.7×10^-4 M b. 1.7×10^-5 M c. 4.3×10^-5 M d. 8.5×10^-6 M 50) Oxidation of which of the following compounds can lead to an aldehyde? a. primary alcohol b. secondary alcohol c. tertiary alcohol d. ether 51) Oxidation of which of the following compounds can lead to ketone? a. primary alcohol b. secondary alcohol c. tertiary alcohol d. ether
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PREBOARD EXAM (PHYSICALAND CHEMICAL PRINCIPLES) 52) Hydrolysis of an ester leads to two compounds. Which of the following pairs compounds is formed from such a hydrolysis? a. An alcohol and an aldehyde c. An alcohol and a carboxylic acid b. Two alcohols d. A ketone and a carboxylic acid 53) Which of the following compounds would you expect to be the most soluble in water? a. CH3CH2CH2CH2CH2CH2CH2CH3 c. CH3CH2CH2CH2CH2CH2CH2OH b. CH3CH2CH2OH d. CH3CH2CH2-O-CH2CH2CH3 54)
Which of nature of a. A soap b. A soap c. A soap d. A soap
the following is the best definition of the chemical soap? is a very long molecule. is a long chain carboxylic acid. is an ester of glycerol and a long chain carboxylic acid. is a salt of a long chain carboxylic acid.
55) The molecule among those in the following list that can be classified as an amide is a. CH3NH2 b. CH3CONH2 c. CH3CHO d. CH3COOH 56) Which of the following amino acids has sulfur in the R group? a. Serine b. Cysteine c. Asparagine d. Tyrosine 57) Triglycerides which are solids or semisolids at room temperature are called: a. oil b. Fat c. Steroid d. Cholesterol 58) One ml of a bacterial culture was pipetted into a 9 ml dilution blank. One-tenth ml of this dilution was pipetted into a 9.9 ml dilution blank. From this dilution, one-tenth ml was plated with 25 ml of culture medium. 220 colonies arose after incubation. How many colony-forming units were present per ml of the original culture? a. 2.2 x 10^6 b. 2.2 x 10^5
c. 2.2 x 10^4
d. 2.2 x 10^7
59) The Philippine cornstarch Corporation prepares pharmaceutical glucose from cornstarch by enzyme hydrolysis. It was observed that when the starch concentration of the slurry was 5%, the rate of conversion of starch to glucose was 0.04 kg/s. When the starch concentration was made 10%, the turnover rate was 0.07 kg/s. The maximum production level of glucose that can reasonably be attained per shift of 8 hours is a. 6084 kg
b. 8064 kg
c. 1008 kg
d. 0.28 kg
60) An act to Control Toxic Substances and Hazardous and Nuclear Wastes providing penalties for violation thereof a. RA 8749
b. RA 9003
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c. RA 9275
d. RA 6969
PREBOARD EXAM (PHYSICALAND CHEMICAL PRINCIPLES) 61) The difference between the actual property value of a solution and the value it would have as an ideal solution at the same T and P and composition is called a. Residual
b. Excess
c. Partial property
d. Gibbs free energy
62) A certain quantity of nitrogen gas collected over water at 20C and at a total pressure of 745 mm Hg has a volume of 200 mL. What will be the volume of the nitrogen in a completely dry state at 780 mm Hg pressure and at 48C. The vapor pressure of water at 20C is 17.54 mm Hg. d) 204.34 mL a) 211.45 mL b) 209.27 mL c) 206.75 mL 63) Among the following processes, all of the following will produce an alkane from an alkyl halide except a) Wurtz Synthesis c) Reduction with Zn b) Hydrogenation d) Corey-House Synthesis 64) The following are correctly named except a) 3-ethylpentane c) N-methylbutanamide b) p-dichlorobenzene d) 5-hexanone 65) Aromatic compounds are characteristics of a) Electrophilic substitution c) Nucleophilic substitution b) Electrophilic addition d) Electrophilic addition 66) Delocalization of pi electrons a) Rearrangement c)hyperconjugation b) isomerism d)resonance 67) Hydration of alkynes yields a) epoxide b) ketone c) alcohol
d) ether
68) The sequence of steps to produce o-nitrobenzoic acid from benzene is (1) Friedel-Crafts Alkylation (2) Nitration (3) Oxidation a) 123 b) 132 c) 213 d) 231 69) Markovnikoff’s addition of HBr to alkynes dominantly produces a) Geminal dihalide c) tetrahalide b) Vicinal dihalide d) halohydrin 70) Ozonolysis of alkenes gives a/an a) aldehydes b) alcohol c) ether
d) ester
71) Which of the following reactions will yield an alcohol from alkenes? a) Oxymercuration-Demercuration c) Hydroxylation b) Hydroboration-Oxidation d) all of the above
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PREBOARD EXAM (PHYSICALAND CHEMICAL PRINCIPLES) 72) Which of the following compounds has the highest boiling point? a) N-pentane b) isopentane c) neopentane d) isobutene 73) A sequence in which a C=C double bond is oxidatively converted to two carbonyl groups through sequential treatment with O3, followed by Zn in acetic acid a) Oxidation c) Oxymercuration-Demercuration b) Ozonolysis d) Hydroboration-Oxidation
74) An addition reaction initiated by attack by an electron-deficient reagent (an electrophile), often a proton from a hydronium ion a) Electrophilic Addition c) Oxidation b) Nucleophilic Addition d) Ozonolysis 75) A reaction sequence used to alkene; initiated by concerted syn with basic hydrogen peroxide a) Oxidation b) Ozonolysis
achieve anti-Markovnikov hydration of an addition of borane, followed by oxidation c) Oxymercuration-Demercuration d) Hydroboration-Oxidation
76) What is the common name of this compound – C6H5OCH3? a) Aniline b) Styrene
c) Cumene d) Anisole
77) The influence of mixing of s and p s character of the hybrid orbital, the a) Hybridization c) b) Hybrid Orbitals d)
orbitals; the greater the fraction of more electronegative is the atom Hybridization Effect Hybrid
78) Name the Alkane CH3 CH3
H 2C
CH H 3C
CH CH
CH3
a) b) c) d)
2-ethyl-3,4-dimethylpentane c) 3,4,5-trimethylhexane 4-ethyl-2,3-dimethylpentane 2,3,4-trimethylhexane
CH3
79) Name the Alkane CH3 CH3
CH H 3C
CH
a) b) c) d)
2-methyl-3-bromobutane 2-methyl-2-bromobutane 2-bromo-3-methylbutane 3-bromo-2-methylbutane
Br
80)A homolytic substitution of halogen for hydrogen, often in an alkane a) Nucleophilic substitution c) Electrophilic aromatic substitution b) Free radical substitution d) Electrophilic addition
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PREBOARD EXAM (PHYSICALAND CHEMICAL PRINCIPLES) 81) Name the Alkene H C H 3C
a) b) c) d)
CH3 C
2-methyl-2-butene 1,2-dimethylpropene 3-methyl-2-butene none of the above
CH3
82) Name the Alkene CH3 H2 C
C
H 3C H 2C
C
CH3
a) b) c) d)
Z-3,4-dimethyl-3-hexene Z-3,4-diethyl-3-hexene E-3,4-dimethyl-3-hexene E-3,4-diethyl-3-hexene
CH3
83) The alkene formed is the one that is more alkyl substituted. a) Markovnikoff’s Rule c) Saitsev’s Rule b) Hoffman’s Rule d) Huckel’s Rule 84) What is the IUPAC name of this compound? H2 C
F
H 3C
a) b) c) d)
4-ethyl-2-fluoroaniline 4-ethyl-2-fluoroanisole 4-ethyl-6-fluoroaniline 4-ethyl-6-fluoroanisole
NH2
85)What is the major product of the reaction?
a) Aniline b) Benzonitrile
c) Benzene d) Iodobenzene
86)The final product of hydration of an alkyne is a/an __________. a) Enol
b) Alkene
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c) Ketone
d) Alcohol
PREBOARD EXAM (PHYSICALAND CHEMICAL PRINCIPLES) 87-91) Consider a continuous steady-state process in which the following reactions take place: C6H12 + 6 H2O → 6 CO + 12 H2 C6H12 + H2 → C6H14 In process 250 moles of C6H12 and 800 moles of H2O are fed into the reactor each hour. The yield of H2 is 40.0% and the selectivity of H2 relative to C6H14 is 12.0. 87) What is the limiting reactant? a) Hexane b) Water c) Hydrogen d)Hexene 88) Calculate the molar flow rate (mol/h) of water in the output stream. a) 138.39 b) 453.32 c) 346.68 d) 640
89) Calculate the extent of the first reaction, is a) 53.33
b) 57.78
c) 346.68
90) Calculate the extent of the second reaction, is a) 53.33 b) 57.78 c) 346.68
d) 138.89 d) 138.89
91) Calculate the mole fraction of carbon monoxide in the output stream a) 0.09 b) 0.28 c) 0.21 d) 0.39 92) Balance the chemical equation given K4Fe(CN)6 + H2SO4 + H2O = K2SO4 + FeSO4 + (NH4)2SO4 + CO a) 1,6,6,2,1,3,6 c) 6,3,1,2,6,6,1 b) 2,6,6,2,1,3,6 d) 1,6,6,2,1,2,6 93) ________ is a method of sequencing amino acids in a peptide.[1] In this method, the amino-terminal residue is labeled and cleaved from the peptide without disrupting the peptide bonds between other amino acid residues. a) Markovnikov Degradation c) Lewis Sequencing b) Edman Degradation d) Hall reaction
94) A 5.00 mL aliquot of bleach (density = 1.61 g/mL) was diluted and treated with excess KI to convert hypochlorite to chloride. The liberated I2 required 22.85 mL of 0.214 M Na2S2O3 for titration. Calculate the % ClO– (51.45 g/mol) in the bleach. a)4.18% b) 2.72% c) 1.56% d) 3.12% 95) Balance the chemical equation K4Fe(CN)6 + KMnO4 + H2SO4 = KHSO4 + Fe2(SO4)3 + MnSO4 + HNO3 + CO2 + H2O a) b) c) d)
60,60,188,10,122,299,162,5,122 122,299,162,5,122,60,60,188,10 188,60,60,122,5,162,299,122,10 10,122,299,162,5,122,60,60,188
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PREBOARD EXAM (PHYSICALAND CHEMICAL PRINCIPLES)
96) A base mixture sample weighing 976 mg was dissolved in sufficient water to make 100 mL solution and divided into two equal portions. The first portion was titrated with 52.05 mL of 0.1004M HCl to the methyl red end point. The other portion was titrated with 23.02 mL of the acid to the phenolphthalein endpoint. Calculate the % composition of sample. a) 50.16% NaHCO3, 50.20% Na2CO3 c)23.90% NaHCO3, 50.20% Na2CO3 b) 10.38% NaHCO3, 50.20% Na2CO3 d)18.94% NaHCO3, 62.70% Na2CO3 97) The phosphate in a 3000 mg sample of industrial detergent was precipitated by the addition of 1 gram AgNO3. The solution was filtered and the filtrate required 18.23 mL of 0.1377 M KSCN. Calculate the percentage of phosphate in the detergent. AgNO3 (169.87 g/mol) PO4–3 (94.97 g/mol) a)3.56% b) 7.12% c) 5.35% d) 10.69% 98) Calculate the weight of primary standard Na2C2O4 (134 g/mol) necessary to react with 25 mL of 0.2005 M KMnO4 in acidic medium. a)0.671 gram b) 1.343 grams c) 1.679 grams d) 2.687 grams 99) Which of the following types of precipitimetry is used as a direct method for halide determination? a)Mohr method b) Volhard method c) Fajans method d) none of these 100) A 0.0722 M acid has pH of 3.11, what is the Ka of the acid? a)4.2 x 10-6 b) 8.35 x 10-6 c)8.35 x 10-7 d) 4.2 x 10-7
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