Chemistry for Non-Majors Question Bank - 2734 Verified Questions

Chemistry for Non-Majors Question Bank

Course Introduction

Chemistry for Non-Majors provides a comprehensive introduction to the fundamental principles and applications of chemistry for students without a strong science background. The course explores essential topics such as atomic and molecular structure, chemical bonding, states of matter, and basic chemical reactions, all within the context of real-world phenomena and everyday life. Emphasis is placed on the relevance of chemistry in environmental issues, health, and technology, helping students develop scientific literacy and an appreciation for the role of chemistry in society. Laboratory sessions are designed to reinforce theoretical concepts through hands-on experiments and observations.

Recommended Textbook Chemistry 10th Edition by Raymond Chang

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25 Chapters

2734 Verified Questions

2734 Flashcards

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Chapter 1: Chemistry: The Study of Change

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Sample Questions

Q1) Name two types of mixtures.

Answer: Homogeneous mixture and heterogeneous mixture

Q2) An object will float at the surface of a liquid if the mass of the object is less than the mass of the liquid that it displaces. A spherical vessel (diameter = 5.00 cm)when empty has a mass of 12.00 g. What is the greatest volume of water that can be placed in the vessel and still have the vessel float at the surface of benzene? (Given: density of water = 1.00 g/cm³; density of benzene = 0.879 g/cm³)

A)45.5 mL

B)448 mL

C)53.4 mL

D)57.5 mL

E)65.4 mL

Answer: A

Q3) Classify the following as a physical or chemical change: Food spoils.

Answer: Chemical

Q4) Classify the following as an element, a compound, or a mixture: Table salt (non-iodized).

Answer: Compound

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Chapter 2: Atoms, Molecules, and Ions

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Sample Questions

Q1) Atoms of the same element with different mass numbers are called A)ions.

B)neutrons.

C)allotropes.

D)chemical families.

E)isotopes.

Answer: E

Q2) The mineral hausmannite is a compound of manganese-55 and oxygen-16. If 72% of the mass of hausmannite is due to manganese, what is the empirical formula of hausmannite?

A)MnO

B)Mn₃O

C)Mn₃O₄

D)Mn₄O₃

E)MnO₃

Answer: C

Q3) Name the straight chain hydrocarbon that contains eight carbon atoms.

Answer: octane

Q4) Name the following ternary compound: Al(NO₃)₃.

Answer: aluminum nitrate

Page 4

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Chapter 3: Mass Relationships in Chemical Reactions

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Sample Questions

Q1) In the Haber process, hydrogen gas reacts with nitrogen gas to produce ammonia.How many kilograms of hydrogen would be required to react completely with 1.0 kg of nitrogen, and how many kilograms of ammonia would be formed?

Answer: 0.22 kg hydrogen required, 1.2 kg ammonia produced

Q2) A 1.375 g sample of mannitol, a sugar found in seaweed, is burned completely in oxygen to give 1.993 g of carbon dioxide and 0.9519 g of water. The empirical formula of mannitol is A)CHO

B)CH₇O₃

C)C₃H₂O

D)C₃H₇O₃

E)CH₂O

Answer: D

Q3) Calculate the mass of sodium chlorate that must be decomposed to form 6.5 g of oxygen.

2NaClO₃(s)\(\rarr\)2NaCl(s)+ 3O₂(g)

Answer: 14 g

Q4) Calculate the mass of 3.7 moles of Br₂. Answer: 590 g

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Chapter 4: Reactions in Aqueous Solution

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Sample Questions

Q1) Give an example of a monoprotic acid.

Q2) Sugar dissolves in water, therefore it is a strong electrolyte. A)True

B)False

Q3) Zinc dissolves in hydrochloric acid to yield hydrogen gas: Zn(s)+ 2HCl(aq)\(\rarr\)ZnCl₂(aq)+ H₂(g)

When a 12.7 g chunk of zinc dissolves in 500.mL of 1.450M HCl, what is the concentration of hydrogen ions remaining in the final solution?

A)0.776 M

B)0.388 M

C)0.674 M

D)1.06 M

E)0 M

Q4) Identify the following compound as an electrolyte or nonelectrolyte: H₂SO₄.

Q5) Identify the following as either a good or poor conductor of electricity: an aqueous solution of Na₂SO₄.

Q6) Define solution, solute, and solvent.

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Chapter 5: Gases

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Sample Questions

Q1) A gas evolved during the fermentation of sugar was collected.After purification its volume was found to be 25.0 L at 22.5°C and 702 mmHg.How many moles of gas were collected?

A)0.95 mol

B)1.05 mol

C)12.5 mol

D)22.4 mol

E)724 mol

Q2) A pressure that will support a column of Hg to a height of 256 mm would support a column of water to what height? The density of mercury is 13.6 g/cm³; the density of water is 1.00 g/cm³.

A)1.00 * 10² ft

B)18.8 mm

C)33.8 ft

D)76.0 cm

E)348 cm

Q3) At standard temperature and pressure, a given sample of water vapor occupies a volume of 2.80 L. How many moles of water vapor are present?

Q4) What is the definition of a "gas"?

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Chapter 6: Thermo-Chemistry

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Sample Questions

Q1) The total heat of hydration of 1 mol of gas phase Li⁺ ions and Cl^- ions is -865 kJ. The lattice energy of LiCl(s)is 828 kJ/mol. Calculate the heat of solution of LiCl.

A)37 kJ/mol

B)1,693 kJ/mol

C)-1,693 kJ/mol

D)-37 kJ/mol

E)None of these.

Q2) Given H₂(g)+ (1/2)O₂(g)\(\rarr\) H₂O(l),

\(\Delta\)0H° = -286 kJ/mol, determine the standard enthalpy change for the reaction 2H₂O(l)\(\rarr\)2H₂(g)+ O₂(g).

A)(\(\Delta\)H° = -286 kJ/mol)

B)(\(\Delta\)H° = +286 kJ/mol)

C)(\(\Delta\)H° = -572 kJ/mol)

D)(\(\Delta\)H° = +572 kJ/mol)

E)(\(\Delta\)H° = -143 kJ/mol)

Q3) What is the standard enthalpy of formation of H₂(g)at 25°C?

Q4) The specific heat of silver is 0.235 J/g·°C. How many joules of heat are required to heat a 75 g silver spoon from 20°C to 35°C?

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Chapter 7: Quantum Theory and the Electronic Structure of Atoms

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Sample Questions

Q1) The scattering of helium atoms by a solid can be used to gain information about the lattice of atoms, provided the wavelength of the helium atoms is comparable to the dimensions of the lattice.What is the wavelength, in picometers, of a helium-4 atom with a kinetic energy of 0.10 eV.(mass of ⁴He = 4.0026 amu; 1 amu = 1.67 * 10^-24 g; 1 eV = 1.602 * 10^-19 J; h = 6.626 * 10^-34 J.s)

Q2) Calculate the frequency of the light emitted by a hydrogen atom during a transition of its electron from the n = 6 to the n = 3 principal energy level. Recall that for hydrogen E_n = -2.18 * 10^-18 J(1/n²).

A)1.64 * 10¹⁵/s

B)9.13 * 10¹³/s

C)3.65 * 10¹⁴/s

D)1.82 * 10^-19/s

E)2.74 * 10¹⁴/s

Q3) An AM radio station broadcasts at a frequency of 1270 kHz.Calculate the wavelength of the broadcast signal in meters.(c = 2.9979 * 10⁸ m/s)

Q4) What is the total number of electrons possible in the 2p orbitals?

Q5) Write the ground state electron configuration for the selenium atom.

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Chapter 8: Periodic Relationships Among the Elements

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Sample Questions

Q1) The cobalt(III)ion, Co³⁺, has how many 3d electrons?

A)0

B)7

C)6

D)5

E)4

Q2) The general electron configuration for noble gas atoms is

A)ns²np⁶

B)ns²np⁵

C)ns²np⁴

D)ns²np³

E)ns²

Q3) Which of the following make an isoelectronic pair: Cl^-, O^2-, F, Ca²⁺, Fe³⁺?

A)Ca²⁺ and Fe³⁺

B)O^2- and F

C)F and Cl^-

D)Cl^- and Ca²⁺

E)None of the above.

Q4) Write the ground-state electron configuration for S^2-.

Page 10

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Chapter 9: Chemical Bonding I: Basic Concepts

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Sample Questions

Q1) The bond in which of the following pairs of atoms would have the greatest percent ionic character (i.e., most polar)?

A)C - O

B)S - O

C)Na - I

D)Na - Br

E)F - F

Q2) Write a Lewis structure for the chlorate ion, ClO₃^-, that obeys the octet rule, showing all non-zero formal charges, and give the total number of resonance structures for ClO₃^- that obey the octet rule.

Q3) Which one of these polar covalent bonds would have the greatest percent ionic character?

A)H -Br

B)H - Cl

C)H - F

D)H- I

Q4) Write the Lewis structure of boron trifluoride.

Q5) Write the chemical equation for which the enthalpy of reaction is the lattice energy of KCl(s).

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Chapter 10: Chemical Bonding Ii: Molecular Geometry and Hybridization

of Atomic Orbitals

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Sample Questions

Q1) Use VSEPR theory to predict the geometry of the PCl₃ molecule.

A)linear

B)bent

C)trigonal planar

D)trigonal pyramidal

E)tetrahedral

Q2) The bond angles in SF₅⁺ are expected to be

A)90°.

B)120°.

C)90° and 120°.

D)90° and 180°.

E)90°, 120°, and 180°.

Q3) According to VSEPR theory, which one of the following molecules should have a geometry that is trigonal bipyramidal?

A)SF₄

B)XeF₄

C)NF₃

D)SF₆

E)PF₅

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Q4) According to the VSEPR theory, the geometrical structure of PF₅ is

Chapter 11: Intermolecular Forces and Liquids and Solids

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Sample Questions

Q1) The normal boiling point of methanol (CH₃OH)is 64.6°C. Given that the vapor pressure of methanol is 75.0 torr at 15.2°C, calculate the molar enthalpy of vaporization of methanol.

A)0.383 kJ/mol

B)3.00 kJ/mol

C)38.0 kJ/mol

D)27.5 kJ/mol

E)74.7 kJ/mol

Q2) Which one of the following crystallizes in a metallic lattice?

A)C

B)NaMnO₄

C)K

D)LiClO₄

E)K₂Cr₂O₇

Q3) Ethanol and dimethyl ether have the same molecular formula, C₂H₆O.Ethanol boils at 78.4°C.Dimethyl ether boils at -23.7°C.Their structural formulas are, respectively, CH₃CH₂OH and CH₃OCH₃. Explain why the boiling point of the ether is so much lower than the boiling point of ethanol.

Q4) Indicate all the types of intermolecular forces of attraction in HCl(g).

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Chapter 12: Physical Properties of Solutions

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Sample Questions

Q1) What is the molarity and molality of a solution that is 10.00 % by mass potassium hydrogen carbonate (KHCO₃, 100.11 g/mol)and has a density of 1.0650 g/mL?

Q2) For dilute aqueous solutions, the concentration units molarity and molality have almost the same values.

A)True

B)False

Q3) Oxygen gas makes up 21 % of the atmosphere by volume.What is the solubility of O₂(g)in water at 25°C if the atmospheric pressure is 741 mmHg? The Henry's law constant for oxygen gas at 25°C is 1.3 * 10^-³ mol/L·atm.

A)2.7 * 10^-4 M

B)1.3 * 10^-3 M

C)6.2 * 10^-3 M

D)9.6 * 10^-3 M

E)0.96 M

Q4) Define solvation.

Q5) The solubility of oxygen in water is about 4.5 * 10^-2 g/L.The water portion of an adult's total blood supply is about 5 liters.How many grams of oxygen could dissolve in 5 liters of water?

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Chapter 13: Chemical Kinetics

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Sample Questions

Q1) The activation energy for the following reaction is 60.kJ/mol. Sn²⁺ + 2Co³⁺ F1F1F1S1 F1F1F10 Sn⁴⁺ + 2Co²⁺ By what factor (how many times)will the rate constant increase when the temperature is raised from 10°C to 28°C?

A)1.002

B)4.6

C)5.6

D)2.8

E)696

Q2) At 25°C, by what factor is the reaction rate increased by a catalyst that reduces the activation energy of the reaction by 1.00 kJ/mol?

A)1.63

B)123

C)1.04

D)1.50

E)2.53

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Chapter 14: Chemical Equilibrium

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Sample Questions

Q1) What conditions are used in the Haber process to enhance the yield of ammonia? Explain why each condition affects the yield in terms of the Le Châtelier principle.

Q2) Describe why addition of a catalyst does not affect the equilibrium constant for a reaction.

Q3) The dissociation of solid silver chloride in water to produce silver ions and chloride ions has an equilibrium constant of 1.8 * 10^-18.Based on the magnitude of the equilibrium constant, is silver chloride very soluble in water? Why?

Q4) Which of these statements is true about chemical equilibria in general?

A)At equilibrium the total concentration of products equals the total concentration of reactants, that is, [products] = [reactants].

B)Equilibrium is the result of the cessation of all chemical change.

C)There is only one set of equilibrium concentrations that equals the K_c value.

D)At equilibrium, the rate constant of the forward reaction is equal to the rate constant for the reverse reaction.

E)At equilibrium, the rate of the forward reaction is equal to as the rate of the reverse reaction.

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Chapter 15: Acids and Bases

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Sample Questions

Q1) A solution with a pH of 8 has a hydrogen ion concentration [H⁺] that is 30 times greater than that of a solution of pH 11.

A)True

B)False

Q2) A 0.14 M HNO₂ solution is 5.7% ionized. Calculate the H⁺ ion concentration.

A)8.0 * 10^-3 M

B)0.057 M

C)0.13 M

D)0.14 M

E)0.80 M

Q3) A 8.0 M solution of formic acid (HCOOH)is 0.47% ionized.What is the K_a of formic acid?

Q4) Write the chemical formula for phosphoric acid.

Q5) In aqueous solutions at 25°C, the sum of the ion concentrations ([H⁺] + [OH^-])equals

1 * 10^{- 14}.

A)True

B)False

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Chapter 16: Acid-Base Equilibria and Solubility Equilibria

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Sample Questions

Q1) Will a precipitate (ppt)form when 300.mL of 2.0 * 10^-5 M AgNO₃ are added to 200.mL of 2.5 * 10^-9 M NaI? Answer yes or no, and identify the precipitate if there is one.

A)Yes, the ppt is AgNO₃(s).

B)Yes, the ppt is NaNO₃(s).

C)Yes, the ppt is NaI(s).

D)Yes, the ppt is AgI(s).

E)No, a precipitate will not form.

Q2) Write an equation showing the net reaction that occurs when a strong base is added to a CO₃^2-/HCO₃^- buffer solution (for carbonic acid, K_a1 = 4.2 * 10^-7, K_a2 = 2.4 * 10^-8):

Q3) All indicators are weak acids that are one color in acidic solution and another color in basic solution.

A)True

B)False

Q4) The solubility of a salt increases as its K_sp increases.

A)True

B)False

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Chapter 17: Chemistry in the Atmosphere

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Sample Questions

Q1) Which one of the following indoor air pollutants has adverse health effects because it is radioactive?

A)formaldehyde

B)carbon monoxide

C)carbon dioxide

D)radon

Q2) Which one of the following would slow the rate of increase of atmospheric CO₂?

A)Building and operating more coal-fired power plants.

B)More use of catalytic converters in cars to produce complete combustion.

C)Use of hydrogen fuel produced using solar or nuclear energy.

D)Conversion of nuclear power plants to methane-burning power plants.

E)Clearing and burning the tropical rain forests.

Q3) Which region of the atmosphere contains the ozone layer?

A)thermosphere

B)mesosphere

C)stratosphere

D)troposphere

Q4) List three primary pollutants removed from automobile exhaust by catalytic converters.

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Chapter 18: Entropy, Free Energy, and Equilibrium

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Sample Questions

Q1) Which of these species would you expect to have the lowest standard entropy (S°)?

A)Br₂(l)

B)Cl₂(g)

C)F₂(g)

D)H₂(g)

E)I₂(s)

Q2) Aluminum forms a layer of aluminum oxide when exposed to air which protects the bulk metal from further corrosion. 4Al(s)+ 3O₂(g)\(\to\)2Al₂O₃(s)

Calculate \(\Delta\)G° for this reaction, given that \(\Delta\)G°_f of aluminum oxide is -1576.4 kJ/mol.

A)-3152.8 kJ/mol

B)-1576.4 kJ/mol

C)-788.2 kJ/mol

D)1576.4 kJ/mol

E)3152.8 kJ/mol

Q3) How does the entropy change when a gas is converted to a liquid?

Q4) Predict the sign of \(\Delta\)S for the process N₂(g, 10 atm)\(\to\) N₂(g, 1atm).

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Chapter 19: Electrochemistry

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Sample Questions

Q1) Using a table of standard reduction potentials, determine which of these reactions (if any)is/are nonspontaneous in the direction indicated at 25°C.

A)2Fe³⁺ + 2Cl^- \(\to\) 2Fe²⁺ + Cl₂(g)

B)2Fe³⁺ + 2Br^- \(\to\) 2Fe²⁺ + Br₂(l) C)2Fe³⁺ + 2I^- \(\to\) 2Fe²⁺ + I₂(s)

D)A and B

E)All are spontaneous.

Q2) Complete and balance the following redox equation using the smallest whole-number coefficients. What is the coefficient of Sn in the balanced equation? Sn + HNO₃ \(\to\) SnO₂ + NO₂ + H₂O (acidic solution)

A)1

B)2

C)3

D)4

E)5

Q3) Will H₂(g)form when Fe is placed in 1.0 M HCl?

Q4) Will H₂(g)form when Cu is placed in 1.0 M HCl?

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Chapter 20: Metallurgy and the Chemistry of Metals

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Sample Questions

Q1) Write the chemical formula of fluorite.

Q2) Volatile impurities are removed from ores by means of A)roasting.

B)amalgamation.

C)electrolysis.

D)flotation.

E)zone refining.

Q3) Which of these elements when doped into silicon would give an n-type semiconductor?

A)C

B)Ga

C)P

D)Ge

E)B

Q4) In p-type semiconductors,

A)the semiconductors are "ultra purified" to increase conductivity.

B)the valence and conduction bands are formed exclusively from "p orbitals."

C)the semiconductors are "patented" for use in commercial applications.

D)acceptor impurities are added to provide "positive holes" that increase the electrical conductivity of the semiconductor.

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Chapter 21: Nonmetallic Elements and Their Compounds

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Sample Questions

Q1) Write the formula for the binary hydride you would expect calcium to form.

Q2) Which of these industrial chemicals is produced in the greatest amount annually?

A)HNO₃

B)H₃PO₄

C)H₂

D)H₂SO₄

E)HClO₃

Q3) The bond energy of F₂ is anomalously low, in comparison with the other halogens, due to the small size of the fluorine atom. Which of the following periodic properties is also anomalously low in the case of fluorine?

A)first ionization energy

B)electron affinity

C)electronegativity

D)diatomic bond length

E)ionic radius

Q4) Write an equation for a laboratory preparation of nitrogen gas.

Q5) P₄O₆ and P₄O₁₀ are allotropes of phosphorus.

A)True

B)False

Page 23

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Chapter 22: Transition Metal Chemistry and Coordination Compounds

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Q1) The numbers of geometrical isomers and optical isomers of the complex ion [Co(en)₃]³⁺ are, respectively, A)2 and 2.

B)1 and 1.

C)3 and 2.

D)1 and 2.

E)2 and 4.

Q2) The electron configuration of a Co³⁺ion is

A)[Ar]3d⁶.

B)[Ar]4s¹3d⁵.

C)[Ar] 4s²3d⁴.

D)[Ar]3d⁵.

E)[Ar]3d⁴.

Q3) How many 3d electrons does a Mn²⁺ ion have?

A)1 B)2 C)3 D)4

E)5

Q4) Write the chemical formula of triammineaquodichlorochromium(III)chloride.

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Chapter 23: Nuclear Chemistry

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Sample Questions

Q1) What fraction of radioactive atoms remains in a sample after six half-lives?

A)zero

B)1/6

C)1/16

D)1/32

E)1/64

Q2) Lead-209 undergoes beta decay.Write a balanced equation for this reaction.

Q3) On a plot of the number of neutrons versus the number of protons, a nucleus of aluminum-28 lies above the belt of stability. Write an equation for radioactive decay of aluminum-28.

Q4) A typical radius of an atomic nucleus is about

A)100 µm

B)5000 mm

C)100 nm

D)5 \(\times\) 10^-3 pm

E)500 pm

Q5) Tritium is a radioisotope of hydrogen having a half-life of 12.3 years.If you initially had 1.0 \(\times\) 10^-7 mole of tritium, how many moles of tritium would be left after 78 years?

Page 25

Q6) What nuclear fuel is produced in a breeder reactor?

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Chapter 24: Organic Chemistry

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Sample Questions

Q1) The reaction of ethylene and water yields

A)an aldehyde.

B)an ester.

C)an alcohol.

D)an ether.

E)an organic acid.

Q2) Cycloalkanes have the general formula

A)C_nH_2n-4

B)C_nH_2n-2

C)C_nH_2n

D)C_nH_2n+2

E)C_nH_2n+4

Q3) The reaction of hydrogen chloride gas with propene will yield 1-chloropropane as the main product.

A)True

B)False

Q4) A compound with the formula C₆H₁₂ may or may not be a saturated hydrocarbon.Explain.

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Chapter 25: Synthetic and Natural Organic Polymers

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Q1) An amino acid is a compound that contains at least

A)one amino group and one amide group.

B)two amino groups and one carboxylic acid group.

C)one hydroxyl group and one methyl group.

D)one carboxylic acid group and one amino group.

E)one methyl group and one amide group.

Q2) The secondary structure of a protein is the

A)configuration of those parts of the chain stabilized by a regular pattern of covalent bonds between C and O groups of the backbone of the chain.

B)configuration of those parts of the chain stabilized by a regular pattern of hydrogen bonds between CO and NH groups of the backbone of the chain.

C)specific order of amino acids in the chain.

D)overall three-dimensional structure of the molecule.

E)overall arrangement of several polypeptide chains into one functional unit.

Q3) Hydrogen bonding, dispersion forces, ionic forces, and dipole-dipole forces all affect the structure of a protein?

A)True

B)False

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