Chemistry for Engineers Review Questions - 2610 Verified Questions

Chemistry for Engineers Review

Questions

Course Introduction

Chemistry for Engineers is a foundational course designed to introduce engineering students to the essential principles of chemistry and their practical applications in the engineering field. The course covers core topics such as atomic and molecular structure, chemical bonding, thermodynamics, equilibrium, kinetics, and materials chemistry, emphasizing their relevance to real-world engineering problems and industrial processes. Through a combination of lectures, laboratory experiments, and problem-solving sessions, students develop an understanding of how chemical principles influence the design, optimization, and functioning of engineering systems, enabling them to make informed decisions related to materials selection, environmental considerations, and process safety.

Recommended Textbook

General Chemistry 11th Edition by Darrell D. Ebbing

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Page 2

Chapter 1: Chemistry and Measurement

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Sample Questions

Q1) How many liters are in 15.1 fluid ounces of a soft drink? (1 fl oz = 28.35 mL)

A)5 × 10^-4 L

B)5 × 10² L

C)4 × 10⁵ L

D)4 × 10² L

E)0.428 L

Answer: E

Q2) How many cubic millimeters equal one cubic meter?

A)10⁴

B)10^-9

C)10³

D)10⁹

E)10^-3

Answer: D

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Chapter 2: Atoms, molecules, and Ions

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Sample Questions

Q1) Which of the following is not a correct name-symbol combination?

A)gallium,Ga

B)iron,Fe

C)nitrogen,N

D)argon,Ar

E)sodium,He

Answer: E

Q2) Chemical reactions between nonmetals and nonmetals primarily involve

A)sharing of electrons.

B)interactions between protons.

C)transfer of electrons.

D)interactions among protons,electrons,and neutrons.

E)interactions between protons and electrons.

Answer: A

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Chapter 3: Calculations With Chemical Formulas and Equations

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Sample Questions

Q1) Which is a reasonable mass corresponding to 10²⁶ molecules of a substance?

A)100 ng

B)100 g

C)100 mg

D)100 kg

E)100 µg

Answer: D

Q2) A 15-g sample of lithium is reacted with 15 g of fluorine to form lithium fluoride: 2Li + F₂ 2LiF.After the reaction is complete,what will be present?

A)0.789 mol of lithium fluoride only

B)2.16 mol of lithium fluoride only

C)2.16 mol of lithium fluoride and 0.395 mol of fluorine

D)0.789 mol of lithium fluoride and 1.37 mol of lithium

E)none of these

Answer: D

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Chapter 4: Chemical Reactions

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Sample Questions

Q1) The net ionic equation for the reaction between aqueous ammonia and hydrobromic acid is

A)HBr(aq)+ NH₃(aq) NH₄Br(aq).

B)H⁺(aq)+ OH^-(aq) H₂O(l).

C)HBr(aq)+ OH^-(aq) Br^-(aq)+ H₂O(l).

D)H⁺(aq)+ NH₃(aq) NH₄⁺(aq).

E)H⁺(aq)+ Br^-(aq)+ NH₃(aq) NH₄⁺(aq)+ Br^-(aq).

Q2) Aqueous solutions of sodium sulfide and copper(II)chloride are mixed together.Which statement is correct?

A)CuS will precipitate from solution.

B)NaCl will precipitate from solution.

C)No precipitate will form.

D)Both NaCl and CuS will precipitate from solution.

E)No reaction will occur.

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6

Chapter 5: The Gaseous State

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Sample Questions

Q1) A 15.6-g mixture of nitrogen and carbon dioxide is found to occupy a volume of 9.9 L when measured at 940.2 mmHg and 54.9°C.What is the mole fraction of carbon dioxide in this mixture?

A)0.486

B)0.5

C)0.513

D)0.597

E)0.402

Q2) The density of ethane,C₂H₆ (30.1 g/mol),at 25°C and 1.13 atm pressure is

A)1.39 g/L.

B)16.6 g/L.

C)1.34 g/L.

D)0.719 g/L.

E)0.136 g/L.

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Chapter 6: Thermochemistry

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Sample Questions

Q1) The enthalpy change at 1 atm of which reaction corresponds to the standard enthalpy of formation of solid calcium nitrate,Ca(NO₃)₂?

A)Ca²⁺(g)+ 2NO₃^-(g)

Ca(NO₃)₂(s)

B)Ca(s)+ N₂(g)+ 3O₂(g) Ca(NO₃)₂(s)

C)Ca(g)+ 2N(g)+ 6O(g) Ca(NO₃)₂(s)

D)Ca(s)+ N₂(g)+ 2O₃(g) Ca(NO₃)₂(s)

E)Ca²⁺(aq)+ 2NO₃^-(aq)

Ca(NO₃)₂(s)

Q2) The quantity of heat required to raise the temperature of a sample of a substance by 1°C is the sample's

A)work.

B)calorimetry.

C)heat capacity.

D)specific heat.

E)enthalpy.

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Chapter 7: Quantum Theory of the Atom

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Sample Questions

Q1) In Bohr's atomic theory,when an electron moves from one energy level to another energy level more distant from the nucleus,

A)energy is absorbed.

B)light is emitted.

C)energy is emitted.

D)no change in energy occurs.

E)none of these

Q2) The contribution for which de Broglie is best remembered in modern science is

A)his statement that no electron can have identical values for all four quantum numbers.

B)his proposal that particles of matter should be associated with wavelike behavior.

C)his statement that an electron can exist in an atom only in discrete energy levels.

D)his statement that elements show periodic repetition of properties.

E)his statement that electrons occupy all the orbitals of a given sublevel singly before pairing begins.

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Chapter 8: Electron Configurations and Periodicity

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Sample Questions

Q1) The change in energy for which of the following processes represents the first ionization energy of iodine?

A)I(g) I²⁺(g)+ 2e^-

B)I(g)+ e ^- I^-(g)

C)2I^-(g) I₂(s)+ 2e^-

D)I(g) I⁺(g)+ e^-

E)I^-(g) I⁺(g)+ 2e^-

Q2) All of the following ground-state electron configurations are correct except A)Fe:[Ar]4s²4d⁶.

B)Ca:[Ar]4s².

C)In:[Kr]4d¹⁰5s25p¹.

D)Cu:[Ar]3d¹⁰4s¹.

E)Xe:[Kr]4d¹⁰5s25p⁶.

Q3) An atom of which of the following elements has the largest atomic radius?

A)Ca

B)Sr

C)Mg

D)Ba

E)Be

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Chapter 9: Ionic and Covalent Bonding

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Sample Questions

Q1) In which of the following lists do the ions not appear in order of increasing ionic radius?

A)S^2- < Cl^- < K⁺

B)Na⁺ < F^- < O^2-

C)Cl^- < Br^- < I^-

D)Li⁺ < Na⁺ < K⁺

E)Al³⁺ < Mg²⁺ < Na⁺

Q2) The Lewis structure for each of the following except ____contains at least one double bond.

A)O₂

B)CS₂

C)C₂H₄

D)NO⁺

E)N₂H₂

Q3) Which of the following species would you expect to have the largest radius?

A)S^2-

B)P

C)Na⁺

D)Se^2-

E)Ca²⁺

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Chapter 10: Molecular Geometry and Chemical Bonding Theory

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Sample Questions

Q1) Which molecule or ion has a trigonal pyramidal molecular geometry?

A)H₂CO

B)H₂CCO

C)CH₃⁺

D)CH₃^-

E)C₂H₄

Q2) Which of the following statements is incorrect regarding the water molecule?

A)There are two lone pairs and two bonding pairs on the central atom.

B)The molecule is polar.

C)The hybridization of oxygen is sp³.

D)The hybridization of hydrogen is sp.

E)The molecular geometry is bent.

Q3) When an atom in a molecule or ion is described as sp³d¹ hybridized,its molecular geometry is

A)trigonal bipyramidal.

B)trigonal planar.

C)linear.

D)tetrahedral.

E)octahedral.

Page 12

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Chapter 11: States of Matter; Liquids and Solids

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Sample Questions

Q1) A low melting solid readily dissolves in water to give a nonconducting solution.The solid is most likely a

A)molecular solid.

B)ionic solid.

C)covalent network solid.

D)weak base.

E)metallic solid.

Q2) Assume 12,500 J of energy is added to 2.0 moles (36 grams)of H₂O as an ice sample at 0°C.The molar heat of fusion is 6.02 kJ/mol.The specific heat of liquid water is 4.18 J/g °C.The molar heat of vaporization is 40.6 kJ/mol.The resulting sample contains which of the following?

A)water and water vapor

B)ice and water

C)only water

D)only water vapor

E)only ice

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Chapter 12: Solutions

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Sample Questions

Q1) Which of the following solutes,dissolved in 1000 g of water,would provide a solution with the lowest freezing point?

A)0.030 mol of barium chloride,BaCl₂

B)0.030 mol of urea,CO(NH₂)₂

C)0.030 mol of calcium sulfate,CaSO₄

D)0.030 mol of acetic acid,CH₃COOH

E)0.030 mol of ammonium nitrate,NH₄NO₃

Q2) If 11.2 g of naphthalene,C₁₀H₈,is dissolved in 107.8 g of chloroform,CHCl₃,what is the molality of the solution?

A)0.0875 m

B)12.4 m

C)0.811 m

D)0.0941 m

E)0.0969 m

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Page 14

Chapter 13: Rates of Reaction

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Sample Questions

Q1) The balanced chemical equation and rate law for the reaction between NO(g)and H₂(g)at a particular temperature are 2NO(g)+ 2H₂(g) N₂(g)+ 2H₂O(g)

Rate = k[NO]²[H₂]

What is the reaction order with respect to nitric oxide?

A)4

B)0

C)1

D)3

E)2

Q2) For a certain reaction of the general form aA products,a plot of the experimental data as [A] versus time is linear.What is the reaction order with respect to reactant A?

A)zero

B)first

C)second

D)fourth

E)third

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15

Chapter 14: Chemical Equilibrium

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Sample Questions

Q1) A(n)_____ is a substance that increases the rate of a reaction but is not consumed by it.

A)antimatter

B)dark matter

C)beta particle

D)pansmer

E)catalyst

Q2) Which of the following statements is true in a reaction system at equilibrium?

A)The equilibrium constant is zero.

B)The number of collisions per unit time between reactants is equal to the number of collisions per unit time between products.

C)Reactants are reacting to form products at the same rate as products are reacting to form reactants.

D)Reactants and products are present in equimolar amounts.

E)The product of the concentrations of the products divided by the product of the concentrations of the reactants is always a constant.

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Chapter 15: Acids and Bases

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Sample Questions

Q1) What is the pH of a solution prepared by dissolving 0.195 g of NaOH(s)in 9.00 L of water?

A)2.312

B)11.688

C)7.000

D)10.734

E)3.266

Q2) The acid strength decreases in the series HBr > HSO₄^- > CH₃COOH > HCN > HCO₃^-.Which of the following is the strongest base?

A)SO₄^2-

B)CO₃^2-

C)CH₃COO^-

D)Br^-

E)CN^-

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Chapter 16: Acid-Base Equilibria

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Sample Questions

Q1) The K_a for hydrofluoric acid is 6.8 × 10^-4.What is K_b for the fluoride ion?

A)1.5 × 10^-11

B)6.8 × 10^-4

C)1.5 × 10³

D)6.8 × 10¹⁰

E)6.8 × 10^-18

Q2) What will happen if a small amount of sodium hydroxide is added to a 0.1 M solution of ammonia?

A)K_b for ammonia will decrease.

B)The percent ionization of ammonia will increase.

C)K_b for ammonia will increase.

D)The percent ionization of ammonia will decrease.

E)The percent ionization of ammonia will remain unchanged.

Q3) Which of the following combinations is not suitable for making a buffer?

A)HClO₄ and NaClO₄

B)NaH₂PO₄ and Na₂HPO₄

C)NH₄Cl and NH₃

D)H₃PO₄ and NaH₂PO₄

E)Na₂CO₃ and NaHCO₃

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Chapter 17: Solubility and Complex-Ion Equilibria

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Sample Questions

Q1) Which of the following substances will increase the molar solubility of nickel(II)phosphate in a saturated solution?

A)AgCl

B)HNO₃

C)KOH

D)AlPO₄

E)Na₃PO₄

Q2) Which of the following salts has the highest molar solubility in water?

A)CaCO₃ (K_sp = 3.8 × 10^-9)

B)Ni(OH)₂ (K_sp = 2.0 × 10^-15)

C)Fe(OH)₂ (K_sp = 8 × 10^-16)

D)AgBr (K_sp = 5.0 × 10^-13)

E)PbI₂ (K_sp = 6.5 × 10^-9)

Q3) A saturated solution of which of the following salts will have the greatest molar concentration of silver ion?

A)Ag₂S (K_sp = 8 × 10^-51)

B)AgCl (K_sp = 1.8 × 10^-10)

C)Ag₂CrO₄ (K_sp = 1.2 × 10^-12)

D)Ag₂CO₃ (K_sp = 8.1 × 10^-12)

E)Ag₄Fe(CN)₆ (K_sp = 8.5 × 10^-45)

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Chapter 18: Thermodynamics and Equilibrium

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Sample Questions

Q1) For which of the following reactions is S° at 25°C closest to zero?

A)N₂(g)+ O₂(g) 2NO(g)

B)H₂(g)+ I₂(s) 2HI(g)

C)CH₃CHO(g)+ ⁵/₂O₂(g) 2CO₂(g)+ 2H₂O(g)

D)2NO(g)+ O₂(g) 2NO₂(g)

E)C₂H₄(g)+

C₂H₄Br₂(l)

Br₂(l)

Q2) _____ is a thermodynamic quantity that is a measure of how dispersed the energy of a system is among the different possible ways that system can contain energy.

A)Enthalpy

B)Cataphoresis

C)Immovability

D)Entropy

E)Anaphoresis

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Page 20

Chapter 19: Electrochemistry

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Q1) When Au is obtained by electrolysis from NaAu(CN)₂,what is the minimum number of coulombs required to produce 1.26 mol of gold?

A)6.08 × 10⁴C

B)1.22 × 10⁵C

C)2.43 × 10⁵C

D)3.65 × 10⁵C

E)4.86 × 10⁵C

Q2) How many faradays are required to convert a mole of NO₃^- ions to NH₄⁺ ions?

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Chapter 20: Nuclear Chemistry

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Sample Questions

Q1) What is the percent activity of a radioactive sample (relative to its original activity)that has undergone four half-lives of decay?

A)6.25%

B)25%

C)12.5%

D)3.13%

E)75.0%

Q2) The rate constant for the decay of a radioactive isootope is 4.226 × 10^-3 / day.What is the half-life of of this isotope?

A)328.0 days

B)410.0 days

C)82.00 days

D)164.0 days

E)none of these

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Chapter 21: Chemistry of the Main-Group Metals

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Sample Questions

Q1) What is the gas obtained by gently heating NH₄NO₃?

A)N₂

B)NO₂

C)N₂O

D)NO₃

E)N₂O₃

Q2) The oxidation state of nitrogen (given in parentheses)is correct in all the following cases except

A)HN₃ (-1).

B)N₂O₃ (+3).

C)HNO₃ (+5).

D)NH₄⁺ (-3).

E)N₂O (+1).

Q3) In hot,basic solution,the hypochlorite ion is unstable.What are the products of its decomposition?

A)HCl(aq)and Cl₂(g)

B)ClO₃^-(aq)and ClO₄^-(aq)

C)Cl^-(aq)and Cl₂(g)

D)ClO₂^-(aq)and ClO₃^-(aq)

E)Cl^-(aq)and ClO₃^-(g)

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Chapter 22: The Transition Elements and Coordination Compounds

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Q1) How many unpaired electrons are there in the tetrahedral complex ion [FeCl₄]^-?

A)3

B)2

C)1

D)4

E)5

Q2) Which of the following statements concerning crystal field theory is incorrect?

A)In an isolated metal ion the d-orbitals have identical energies.

B)In low spin octahedral complexes the electrons are concentrated in the d_xy,d_xz,and d_yz orbitals.

C)High spin complexes have the minimum of unpaired electrons.

D)Strong bonding ligands favor a larger crystal field splitting ( )than weak bonding ligands.

E)Low spin complexes are favored when the electron pairing energy (P)is less than the crystal field splitting ( ).

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Chapter 23: Organic Chemistry

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Sample Questions

Q1) Which of the following names may represent either a cis or a trans isomer?

A)1-butene

B)1,2-dibromoethene

C)1,1,2-tribromoethene

D)1,1-dibromoethene

E)1-bromo-1-chloroethene

Q2) Which of the following best describes the bonding in ethylene,CH₂=CH₂?

A)The pi electrons are localized above and below a plane defined by the carbon and hydrogen atoms.

B)The pi electrons are localized between the two carbons.

C)Each carbon atom is sp² hybridized.

D)A and C.

E)B and C.

Q3) Which compound is a ketone?

A)(CH₃)₂C(OH)CH₃

B)(CH₃)₂CHCOOH C)(CH₃)₂CHOCH₃ D)(CH₃)₂CHCHO E)(CH₃)₂CHCOCH₃

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Chapter 24: Polymer Materials: Synthetic and Biological

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Q1) What is the significance of a "stop codon"?

A)When it appears in messenger RNA,it is a signal to stop protein biosynthesis.

B)When it appears in transfer RNA,it is a signal to stop transferring amino acids to the growing protein chain.

C)When it appears in DNA,it is a signal to stop chromosome biosynthesis.

D)When it appears in a protein,it is a signal for the protein to unfold.

E)When it appears in ribosomal RNA,it is a signal to stop catalyzing protein biosynthesis.

Q2) In an electrically conducting polymer,what is a "hole"?

A)It is a region of negative charge.

B)It is a delocalized electron.

C)It is an antibonding molecular orbital.

D)It is a molecular orbital from which a electron has been abstracted.

E)It is an ion,such as I₃^-,added to increase the conductivity of the polymer.

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