FINAL PREBOARD EXAMINATION Day 1- Physical and Chemical Principles

What is the maximum number of electrons that can occupy a 5f sublevel?
A. 5 B. 7 C. 14 D. 50

C. 14

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Hydrogen is collected in a 250-milliliter container over water at 30°C. The total pressure is 101.246 kPa. What is the pressure of the
“dry” hydrogen gas?
A. 97 kPa B. 92 kPa C. 88 kPa D. 85 kPa

A. 97 kPa

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From the data in Problem #2, what is the volume occupied by the water vapor?
A. 250 mL B. 220 mL C. 200 mL D. 180 mL

A. 250 mL

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What is the empirical formula of an ion whose composition by mass is 57.14% sulfur, 42.86% oxygen?
A. SO2^-2
B. SO3^-2
C. S2O3^2-
D. SO4^2-

C. S2O3^2-

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Given the reaction: 2C8 H18(g )+25O2 (g)⟶16C O2 (g)+18 H2O(g)
. What is the total number of liters of O2
required for the complete combustion of 4.00 liters of C8H18?
A. 25 B. 50 C. 100 D. 200

B. 50

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Given the reaction: A+B⟶AB+50kJ. If the activation energy of 5 kJ is required for the forward reaction, the activation
energy of the reverse reaction is
A. 5 kJ B. 45 kJ C. 50 kJ D. 55 kJ

D. 55 kJ

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volume is
A. increased and the temperature is increased
B. increased and the temperature is decreased
C. decreased and the temperature is increased
D. decreased and the temperature is decreased

C. decreased and the temperature is increased

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According to the Bronsted-Lowry theory, an acid is any species that can
A. donate a proton C. accept a proton
B. donate an electron D. accept an electron

A. donate a proton

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. The ionization constants (Ka values) of four acids are shown below. Which Ka represents the weakest of these acids?
A.Ka=1.0E-5 B. Ka=1E-4 C. 7.1E-3 D. 1.7E-2

A.Ka=1.0E-5

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Oxides of nonmetals react with water to form
A.acids B. bases C. salts D. anhydrides

A.acids

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The cracking of dicyclopentadiene to give cyclopentadiene is represented by the equation below: C10 H12(l)⟶2C5 H6 (l)

The densities of dicyclopentadiene and cyclopentadiene are 0.982 g/mL and 0.802 g/mL, respectively. How many mL of
cyclopentadiene can be obtained from 20.0 mL of dicyclopentadiene?
A. 20.0 mL B. 16.3 mL C. 24.5 mL D. 10.0 mL

C. 24.5 mL

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What volume of 0.125 M H2SO4 is required to neutralize 2.50 g of Ca(OH)2?
A. 54 mL B. 270 mL C. 135 mL D. 0.170 mL

B. 270 mL

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What is the mass of the precipitate formed when 12.0 mL of 0.150 M NaCl is added to 25.0 mL of a 0.0500 M AgNO3 solution?
A. 258 g B. 0.179 g C. 36.0 g D. 0.258 g

B. 0.179 g

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Vinegar is an aqueous solution of acetic acid. A 5 mL sample of particular vinegar requires 26.90 mL of 0.175 M NaOH for its
titration. What is the molarity of acetic acid in the vinegar?
A. 0.52 B. 1.04 C. 0.94 D. 0.47

C. 0.94

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What is the energy in J of a photon of electromagnetic radiation that has a wavelength of 9.0 m?
A. 6E-23 B. 2.2E-26 C. 2.7E9 D. 4.5E25

B. 2.2E-26

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Which of the following has the largest first ionization energy?
A. Fe B. Cu C. Ge D. S

D. S

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Which of the following species is the largest?
A. Br B. Kr C. Sr2+ D. Rb

A. Br

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In which of the following molecule do we find bond angles of 109.5°?
A. BF3 B. CCl4 C. SF4 D. NH3

B. CCl4

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Which hybrid orbital set and molecular geometry are incorrect?
A. sp2
– trigonal planar C. sp – linear
B. sp3
– tetrahedral D. sp2
– trigonal bipyramida

A. sp2– trigonal planar

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What is the total vapor pressure in torr of a mixture of H2O(l) and 0.123 mol of CH4(g) at T=30°C and a total vapor volume of 20.0 L?
A. 31.9 torr B. 43.3 torr C. 116 torr D. 148 torr

D. 148 torr

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The gas CF6 is in a container with a volume of 19.0 L, a temperature of 29.3°C, and a pressure of 1.82 atm. A mixture is formed by
adding the CF6 to a container with C3H8 gas. The mixture has a pressure of 4.23 atm, a temperature of 29.3°C, and a volume of 48.9
L. What is the partial pressure of C3H8 in the mixture? What is the mole fraction of CF6 in the mixture?
A. 2.41 atm, 0.43 B. 2.41 atm, 0.57 C. 3.52 atm, 0.17 D. 3.52 atm, 0.83

C. 3.52 atm, 0.17

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A mixture of the gases He and Ar, whose mole fraction He is 0.40, is collected over water at 29°C. If the total pressure exerted by
the gas mixture is 760 mmHg, what is the partial pressure of Ar in mmHg?
A. 316 B. 456 C. 292 D. 438

D. 438

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Freon-11, which has the chemical formula CCl3F, has a normal boiling point of 23.8°C. The specific heats of CCl3F(l) and CCl3F(g) are
0.87 J/kg·K and 0.59 J/kg·K, repectively. The heat of vaporization is 24.75 kJ/mol. Calculate the heat required to convert 10.0 g of
Freon-11 from a liquid at -50°C to a gas at 50.0°C.
A. 0.15 kJ B. 0.64 kJ C. 1.8 kJ D. 2.6 kJ

D. 2.6 kJ

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Nickel metal crystallizes in a cubic close-packed structure (face-centered cubic cell). What is the coordination number of each nickel
atom?
A. 4 B. 6 C. 8 D. 12

D. 12

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What is the difference between low- and high-density polyethylene (LDPE and HDPE)? A. LDPE has less chain branching than HDPE B. LDPE is less crystalline than HDPE C. LDPE has an average molecular mass in the range of 1

B. LDPE is less crystalline than HDPE

Sintering is A. placing in the middle C. sieving to achieve uniform particle size B. heating to high temperature under pressure D. finely dividing

B. heating to high temperature under pressure

The solubility of Cr(NO3)3·9H2O in water at 15°C is 208 g per 100 mL of solution. Is a 1.22 M solution of Cr(NO3)3·9H2O in water at 20°C saturated, supersaturated or unsaturated? A. unsaturated B. supersaturated C. needs more data D. saturated

A. unsaturated

The Henry’s Law constant for CO2 IS 3.1E-2 mol/L·atm at 25°C. What pressure would be necessary in order to have a 0.25 M solution? A. 0.12 atm B. 8.1 atm C. 81 atm D. 12 atm

B. 8.1 atm

Lysozome is an enzyme that breaks bacterial cell walls. A solution containing 0.15 g of this enzyme in 210 mL of solution has an osmotic pressure of 0.953 torr at 25°C. What is the molar mass of this substance? A. 13.9 g/mol B. 18.3 g/mol C. 1.17E3 g/mol D. 1.39E6 g/mol

D. 1.39E6 g/mol

What is the freezing point (in °C) of a solution prepared by dissolving 11.3 g Ca(NO3)3 in 115 g water? A. 3.34°C B. 1.11°C C. -1.11°C D. -3.34°C

D. -3.34°C

Determine the mg of mercury in a piece of swordfish of mass = 150 g that has a mercury concentration of 0.20 ppb by mass. A. 3E-5 B. 3.0 C. 3E-2 D. 3E-8

A. 3E-5

What is the freezing point in °C of a 0.10 M solution of NaCl? A. -0.19 B. +0.37 C. -1.86 D. -0.37

D. -0.37

The first-order rate constant for the decomposition of N2O5 to NO2 and O2 at 70°C is 6.82E-3/s. Suppose we start with 0.30 mol of N2O5(g) in a 0.50 L container. How many moles of N2O5 will remain after 1.5 min? A. 0.555 mol B. 0.081 mol C. 0.297 mol D. 0.162 mol

D. 0.162 mol

36. A certain first-order reaction has a rate constant of 1.75E-1/s at 20°C. What is the value of k at 60°C if activation energy is 121 kJ/mol? A. 68.3/s B. 5.6/s C. 0.175/s D. 0.525/s

A. 68.3/s

The decomposition of NOBr is second-order with respect to NOBr and second-order overall. If the initial concentration of NOBr is 0.102 M and the rate constant is 25/M·min, what is the half-life of the reaction? A. 4.1E-3 min B. 2.8E-2 min C. 4.0E-2 min D. 3.9E-1 min

D. 3.9E-1 min

From the data in problem #36, what is the concentration of NOBr after 1.0 min? A. 1.4E-12 M B. 2.9E-2 M C. 4.0E-2 M D. 9.8 M

B. 2.9E-2 M

The half-life for the radioactive decay of cesium-130 is 30 min. What percentage of the initial activity will be present after 2.0 hours? A. 3.13 B. 6.25 C. 25 D. 12.5

B. 6.25

A mixture of 0.10 mol of NO, 0.50 mol of H2 and 0.10 mol of H2O is placed in a 1.00 L vessel. The following equilibrium is established: 2 N O(g)+2 H2(g )⇌ N2(g )+2H2 O( g) . At equilibrium [NO] = 0.062 M. Calculate the concentrations of H2, N2 and H2O. A. [H2]=0.012M, [N2]=0.019M, [H2O]=0.138M B. [H2]=0.012M, [N2]=0.038M, [H2O]=0.138M C. [H2]=0.031M, [N2]=0.019M, [H2O]=0.119M D. [H2]=0.05M, [N2]=0.062M, [H2O]=0.100M

A. [H2]=0.012M, [N2]=0.019M, [H2O]=0.138M

For the equilibrium:2 I Br(g)⇌ I 2 (g)+Br2 (g) , KC = 8.5E-3 at 150°C. If 0.04 mol of IBr is placed in a 1.0 L container, what is the concentration of this substance after equilibrium is reached? A. 0.016M B. 0.020M C. 0.025M D. 0.034M

D. 0.034M

From the data in problem #40, if 0.01 mol of I2 and 0.01 mol Br2 are placed in a 1.0 L container, what is the concentration of IBr after equilibrium is reached? A. 5.4E-3M B. 5.9E-3M C. 0.017M D. 0.020M

C. 0.017M

The production of sulfur dioxide follows the equation 2 SO2 (g)+O2 (g)⇌2 SO3 (g) with Kp = 3.40 at 1000K. What is the concentration of sulfur trioxide if we begin with 0.0050 atm of sulfur dioxide and the reaction occurs in 1.00 atm air, which is 20% oxygen? Assume that the loss of oxygen is small compared to its concentration. A. 1.65 atm B. 0.117 atm C. 0.00292 atm D. 0.00146 atm

C. 0.00292 atm

The active ingredient in aspirin is acetylsalicylic acid, HC9H7O4, a monoprotic acid with Ka = 3.3E-4 at 25°C. What is the pH of a solution obtained by dissolving two aspirin tablets, each containing 325 mg of acetylsalicylic acid in 100 mL of water? A. 1.44 B. 2.48 C. 1.34 D. 1.74

B. 2.48

Calculate the percent ionization of 0.10 M butanoic acid (Ka=1.5E-5) in a solution containing 0.05 M sodium butanoate. A. 3.0E-5 B. 3.0E-4 C. 3.0E-2 D. 4.52

C. 3.0E-2

What is the ratio of [HCO3] to [H2CO3] in blood at pH 7.40 (Ka=4.3E-7)? A. 1.7E-14 B. 7.0E-4 C. 9.3E-2 D. 11

D. 11

Lead sulfate has a solubility of 4.25 mg per 100 mL of solution. What is its Ksp? A.1.4E-4 B. 1.81E-3 C. 1.96E-8 D. 1.96E-10

C. 1.96E-8

What is the final pH if 0.20 mol HCl is added to 0.50 L of a 0.28 M NH3 and 0.11 M NH4Cl buffer solution? A. 4.64 B. 11.32 C. 4.78 D. 9.2

D. 9.2

Which of the noble gas is present in the highest concentration in dry air at sea level? A. Kr B. Ar C. Xe D. Ne

B. Ar

The depression in freezing point of a dilute aqueous solution of a non-electrolytic solute is 0.65oC. What is its relative lowering of vapor pressure? ( Kf = 1.8 K.kg.mol-1) A. 0.0067 B. 0.042 C. 0.21 D. 0.42

A. 0.0067

Use the van der Waals equation of state to calculate the pressure exerted by exactly 1 mol of gaseous ammonia, NH3, held at a temperature of 1000K in a vessel of a volume 2.50 dm3 . The value of the van der Waals parameters for ammonia area, a=4.225 atm dm6mol-2 and b=3.71 x10-2 dm3 mol-1 . A. 3.33 kPa B. 3.31 MPa C. 1970 Pa D. 224 kPa

B. 3.31 MPa

50. The complementary strand of m-RNA formed over the single stranded DNA of sequence 5’-A-T-C-A-G-T-3’) is A. 5’-T-G-A-C-T-A-3’ C. 5’-A-C-T-G-A-T-3’ B. 5’-A-C-U-G-A-U-3’ D. 5’-U-G-U-C-A-3

B. 5’-A-C-U-G-A-U-3

A calorimeter was calibrated by passing an electrical current through a heater and measuring the rise in temperature that resulted. When a current of 113 mA from a 24.1V source was passed through the heater for 254 s, the temperature of the calorimeter rose by 2.61oC. Determine the heat capacity of the calorimeter. A.1.04 J/K B. 24.9 J/K C. 50.2 J/K D. 265 J/K

D. 265 J/K

Calculate the difference between the molar internal energy and the molar enthalpy for a perfect gas at 298.15 K. A. 0.5425 kJ/mol B. 765 J/mol C. 2.4790 kJ/m D. 10.432 kJ/mol

C. 2.4790 kJ/m

Calculate the standard enthalpy of combustion of phenol, C6H5OH, at 298.15 K given that, at this temperature, the standard enthalpy of formation of phenol is -165.0 kJ mol-1, of liquid water, H2O is 385.8 kJ mol-1 and gaseous carbon dioxide, CO2, is -393.52 kJ mol-1. A. -340 kJ/mol B. -524.3 kJ/mol C. -1240 kJ/mol D. -3053.5 kJ/mol

D. -3053.5 kJ/mol

The equilibrium constant for the reaction:CO(g)+H 2O(g) CO2(g)+H 2(g) is K=1.03 x105 at 298.15 K. Calculate the standard reaction Gibbs energy at this temperature. A. -28.6 kJ/mol B. -14.2 kJ/mol C. -2.40 kJ/mol D. 4.12 kJ/mol

A. -28.6 kJ/mol

Calculate the equilibrium constant at 25oC for the reaction:2 NO(g)+O 2(g) 2NO2(g) given that Δ f G o=−69.8 kJ mol−1 A. 1.2 E-5 B. 1.7E-3 C. 1.03 D .1.7E12

D .1.7E12

For many substance, the variation with temperature of the molar heat capacity at constant pressure of is given by the expression Cp ,m=a−bT− c T 2 For copper, a = 22.64 J K-1 mol-1, b= 6.28 x10-3 J K-2mol-1 with the value of c being negligible estimate the change in the molar enthalpy of copper when it is heated from 293 to 323 K. A. +210 J/mol B. 437 J/mol C. +737 J/mol D. 1200 J/mol

C. +737 J/mol

Calculate the pH of a solution prepared by mixing 25 mL of 0.1 NaOH and 25 mL of 0.1 N HAc. A. 2.46 B. 12.96 C. 4.57 D. 8.75

D. 8.75

Calculate the pH of a solution prepared by mixing 10 mL of 0.1 NaOH and 25 mL of 0.1 N HAc. A. 2.46 B. 12.96 C. 4.57 D. 8.75

C. 4.57

Calculate the pH of a solution prepared by mixing 30 mL of 0.1 NaOH and 25 mL of 0.1 N HAc. A. 2.46 B. 12.96 C. 4.57 D. 8.75

B. 12.96

In a titration, 2.7 cm3 of 0.100 mol dm-3 sodium hydroxide, NaOH, solution is added to 25.0 cm3 of 0.125 moldm-3benzoic acid, C6H5COOH, solution. Calculate the pH of the resulting solution given that the pKaof benzoic acid is 4.19 A. 3.13 B. 4.12 C. 7.45 D. 9.12

A. 3.13

Calculate the ionic strength of a solution iron(III)carbonate, Fe2(CO3)3 of concentration 0.020 mol dm-3 . A. 0.25 B. 0.30 C. 0.40 D. 0.50

B. 0.30

The rate constant for the substitution reaction C 4 H 9Cl+H 2O C 4 H 9OH +HCl increases by a factor of 10.6 when temperature is increased from 298 K to 308 K. Calculate the activation energy of the reaction. A. 180 kJ/mol B. 78.2 kJ/mol C. 43.9 kJ/mol D. 12.1 kJ/mol

A. 180 kJ/mol

A liquid that has percolated through solid waste and has extracted dissolved suspended materials from it A. permeate B. leachate C. filtrate D. seepage

B. leachate

What usually happen to the surrounding when water vapor condenses A. it warms the surrounding B. it neither warm nor cold the surrounding C. the surrounding temperature decreases D. the surrounding will be dehumidified

A. it warms the surrounding

Calculate the pH of a buffer solution containing 0.01 M acetic acid and 0.01 M sodium acetate. A. 2.42 B. 4.74 C. 3.76 D. 6.23

B. 4.74

Which of the following is a unit of radiation exposure? A. grays B. roentgen C. curie D. rads

B. roentgen

A device commonly used to create measure and photograph emission spectra. A. tachometer B. spectrometer C. manometer D. hydrometer

B. spectrometer

Which of the following graphs is linear for A products? A. ln[A] versus t if second order inA C. 1/[A] versus t if first order in A B. [A]2 versus t if second order in A D. ln[A] versus t if first order in A

D. ln[A] versus t if first order in A

For a certain reaction plot 1/[A} versus time is linear, where A is one of the reactants. What is the order of the reaction? A. zero-order B. first-order C. second-order D. third-order

C. second-order

Which of the following would have the lowest vapor pressure at 0oC? A. CH3OH B. CH4 C. H2O D. CH2Cl2

C. H2O

The reason that some insects can walk on water is due to A. surface tension B. adhesive forces C. vaporization D. capillary action

A. surface tension

Which of the following plastic is used in making Styrofoam, disposable cups, forks, spoons and food containers? A. polyethylene B. polyvinyl chloride C. polypropylene D. polystyrene

D. polystyrene

The color of bromine is A. white B. violet C. black D. brown reddish

D. brown reddish

Which of the following generates the most ions in dilute aqueous solution? A. C2H5OH B. MgCl2 C. NaCl D. NaHSO4

B. MgCl2

Which of the following is a weak base? A. NaOH B. Ca(OH)2 C. NH3 D. RbOH

C. NH3

Which of the following is themost reactive? A. propene B. propyne C. propane D. cyclopropane

B. propyne

Which of the following are soluble? I)BaSO4 II) AgBr III) Sr3(NO3)2 IV)PbS V) Na2CO3 A. all are soluble B. III only C. II and V D. I, II, and IV only

C. II and V

What is the name of the following alkane? CH3---CH---CH---CH3 l l CH3 CH3 A. 2,3-dimethyl butane B. 1-isopropyl-1-methyl ethane C. 1,1,2-trimethyl propane D. 1,3-dimethyl butane

A. 2,3-dimethyl butane

Pentane and isopentane are what type of isomers? A. aldehydes B. chiral C. structural D. enantiomers

C. structural

What is the hybridization of the oxygen atom in an aldehyde A. sp B. sp3 C. d2 sp3 D. sp^2

D. sp^2

Which of the following are monosaccharides? (I)glucose, (II) fructose, (III) lactose, (IV) sucrose A. III and IV B. I and II C. I D. II

B. I and II

Glutamic acid (C5H9O4N) is used as one of the reagents for a standard to check the BOD test. Determine the theoretical oxygen demand of 150 mg/L of glutamic acid. Assume the following reactions apply. C5 H9 O4 N+4.5O2 5CO2+3H2O+N H 3 N H3+2O2 N O3+H ++H2O A. 180 mg/L B. 190 mg/L C. 1988 mg/L D. 212 mg/L

D. 212 mg/L

If the 5-day BOD of a waste is 220 mg/L and the ultimate BOD is 320 mg/L, what is the rate constant? A. 0.142/day B. 0.178/day C. 0.210/day D. 0.233/da

D. 0.233/da

A sample of municipal sewage is diluted to 1% by volume prior to running a five-day BOD test. After 5 days, the oxygen consumption is determined to be 2 mg/L. what is the five-day BOD of the sewage? A. 200 mg/L B. 220 mg/L C. 240 mg/L D. 300 mg/L

A. 200 mg/L

Equimolar amounts of hydrogen and oxygen gas, at the same temperature, are release into a large container, the ratio of the rate of diffusion of the hydrogen molecules to that of the molecules of oxygen would be A. 256:1 B. 16:1 C. 1:16 D. 4:1

D. 4:1

At what temperature will the velocity of CO2 molecules equal to the velocity of oxygen molecules at 0oC. A. 102oC B. 632oC C. 132oC D. 125oC

A. 102oC

How much NaNO3 must be weighed out to make 50 ml of an aqueous solution containing 70 mg Na+ per ml. A. 10.5 g B. 11.0 g C. 12.9 g D. 14.2 g

C. 12.9 g

What is the equivalent weight of an acid 1.243 f of which required 31.72 cm3 of 0.1923 N standard base for neutralization? A. 180 B. 194 C. 204 D. 210

C. 204

The major components in acid rain are acids form frim _____. A. NOx and Sox B. SOx and CO2 C. NOx and CO2 D. CO and CO2

A. NOx and Sox

What volume of 0.115 M HClO4 solution is required to neutralized 50.00 mL of 0.0875 M NaOH? A. 0.115 mL B. 38.0 L C. 38.0 mL D. 50.0 mL

C. 38.0 mL

What is the pH of natural rain water? A. 5.6-6.2 B. 7.0 – 8.3 C. 4.2 – 4.4 D. 2.2 – 2.4

A. 5.6-6.2

When carbon dioxide is dissolved in water it will form ____. A. carbonic acid B. acetic acid C. nitric acid D. CaCO3

A. carbonic acid

A spoon, with a surface of 45 cm2 , is suspended in a cell filled with a 0.10 M solution of gold(III) chloride. AuCl3. A current of 0.52 A has been passed through the cell, until a coating of gold 0.10 mm thick, has plated on the spoon. How long did the current run? A. 3.6 hr B. 6.9 hr C. 11 hr D. 2.3 hr

B. 6.9 hr

Two gas storage bulbs are at the same temperature. The 1 L bulb contains 0.50 atm of helium and 2L bulb contains 1 atm nitrogen. The valves connecting the two bulbs are opened and they are conneted through a negligible volume. The pressure in the bulbs after they have pressure equilibrated and are at the initial temperature is A. 1.50 atm B. 0.67 atm C. 0.50 atm D. 0.84 atm

D. 0.84 atm

Maleic acid contains 41.4% carbon, 3.47% hydrogen, and 55.1% oxygen by weight. A 0.050-mole sample of this compound weighs 5.80 g. what is the molecular formula of the maleic acid? A. CHO B. C2H2O2 C. C3H3O D. C4H4O4

D. C4H4O4

t takes 16.6 min for a 10 mi sample of unknown gas to effuse through a pinhole. A 10 ml sample of helium required 5 min. What is the molecular weight of the unknown gas? A. 13.3 g/mol B. 44.1 g/mol C. 177 g/mol D. 7.3 g.mo

B. 44.1 g/mol

The geometry of SO3 molecule is the best describe as A. linear B. trigonal planar C. tetrahedral D. bent

B. trigonal planar

. How many secondary carbon atoms does methyl cyclopropane have? A. none B. one C. two D. three

C. two

FINAL PREBOARD EXAMINATION Day 1- Physical and Chemical Principles - Flashcards

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