Chemistry for Engineering Pre-Test Questions - 929 Verified Questions

Chemistry for Engineering

Pre-Test Questions

Course Introduction

Chemistry for Engineering introduces the fundamental principles of chemistry with a focus on their application in engineering contexts. The course covers essential topics such as atomic and molecular structure, chemical bonding, stoichiometry, states of matter, thermodynamics, and chemical kinetics. Special emphasis is placed on material properties, corrosion, electrochemistry, and environmental considerations relevant to engineering disciplines. Through lectures, laboratory experiments, and problem-solving sessions, students develop a solid understanding of how chemical processes influence the design, operation, and optimization of engineering systems. This foundation prepares students to address real-world challenges in various engineering fields, including civil, mechanical, chemical, and electrical engineering.

Recommended Textbook

Introductory Chemistry An Atoms First Approach 1st Edition by Julia Burdge

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17 Chapters

929 Verified Questions

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Page 2

Chapter 1: Atoms and Elements

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Sample Questions

Q1) The alkali metal elements are found in _______ of the periodic table.

A)Group 1A

B)Group 2A

C)Group 3A

D)Period 7

E)Period 1

Answer: A

Q2) Lead (Pb) is a main group element.

A)True

B)False

Answer: True

Q3) What is the term used for findings that are summarized based on a pattern or trend?

A)Law

B)Hypothesis

C)Theory

D)Phenomena

E)Prediction

Answer: A

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Chapter 2: Electrons and the Periodic Table

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Sample Questions

Q1) Arrange these ions in order of increasing ionic radius: K⁺ , P³ , S² , Cl.

A)K⁺ < Cl < S² < P³

B)K⁺ < P³< S² < Cl

C)P³ < S² < Cl < K⁺

D)Cl < S² < P³ < K⁺

E)Cl < S² < K⁺ < P³

Answer: A

Q2) Visible light, radio waves, microwave radiation, infrared, ultraviolet radiation, X-rays, and gamma rays all constitute the electromagnetic spectrum.Which of the following characteristics do all of these kinds of radiation share?

A)They all have the ability to generate heat in objects.

B)They all have the same frequencies.

C)They are all the transmission of energy in the form of waves.

D)They have equal energies.

E)They have the same electron spin state.

Answer: C

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Page 4

Chapter 3: Compounds and Chemical Bonds

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Sample Questions

Q1) The formula for sodium sulfide is A)NaS

B)K₂S

C)NaS₂

D)Na₂S E)SeS

Answer: D

Q2) What is the formula for the ionic compound formed by calcium and selenium?

A)CaSe

B)Ca₂Se

C)CaSe₂

D)Ca₃Se

E)CaSe₃

Answer: A

Q3) A scoop of vanilla ice cream is a pure substance. A)True

B)False

Answer: False

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Chapter 4: How Chemists Use Numbers

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Sample Questions

Q1) The distance between carbon atoms in ethylene is 134 picometers.Which of the following expresses that distance in meters?

A)1.34 × 10¹³ m

B)1.34 × 10¹² m

C)1.34 × 10¹⁰ m

D)1.34 × 10⁷ m

E)1.34 × 10⁶ m

Q2) If a patient in the hospital is running a temperature of 39.5°C, what is this in degrees Fahrenheit?

A)99°F

B)101.3°F

C)102.4°F

D)103.1°F

E)104°F

Q3) The diameter of Earth is 12.7 Mm.Express this diameter in centimeters.

A)1.27 × 10⁵ cm

B)1.27 × 10⁶ cm

C)1.27 × 10⁷ cm

D)1.27 × 10⁸ cm

E)1.27 × 10⁹ cm

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Chapter 5: The Mole and Chemical Formulas

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Sample Questions

Q1) Calculate the formula mass of (NH₄)₃AsO₄.

A)417.80 amu

B)193.05 amu

C)165.02 amu

D)156.96 amu

E)108.96 amu

Q2) Five vials each contain 12 grams of a solid metal sample.The samples include calcium, platinum, barium, gold, and silver.Which vial has the fewest moles of metal atoms?

A)Calcium

B)Barium

C)Gold

D)Silver

E)Platinum

Q3) How many moles of ammonia, NH₃, are in 13.81 g of NH₃?

A)1.234 moles

B)0.8107 moles

C)8.316 × 10²⁴ moles

D)4.881 × 10²³ moles

E)235.3 moles

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Chapter 6: Molecular Shape

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Sample Questions

Q1) Which of the following atoms does not participate in hydrogen bonding?

A)S

B)O

C)F

D)N

E)H

Q2) The total number of bonding electrons in a molecule of formaldehyde (H₂CO) is

A)3.

B)4.

C)6.

D)8.

E)18.

Q3) Which one of the following pure substance has both dispersion forces and dipole-dipole forces?

A)HCl

B)BCl₃

C)Br₂

D)H₂

E)CO₂

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Chapter 7: Solids, Liquids, and Phase Changes

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Sample Questions

Q1) Which substance has the highest vapor pressure at room temperature?

A)HF

B)HCl

C)HBr

D)HI

E)All of these substances have the same vapor pressure at room temperature.

Q2) What is the process in which molecules undergo a phase change from the liquid phase to the solid phase?

A)vaporization

B)condensation

C)freezing

D)melting

E)sublimation

Q3) What is the process in which molecules undergo a phase change directly from the gas phase to the solid phase?

A)deposition

B)sublimation

C)freezing

D)condensation

E)melting

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Chapter 8: Gases

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Sample Questions

Q1) The pressure of hydrogen sulfide gas in a container is 3.565 ×10⁴ Pa.What is this pressure in torr? (1 atm = 101,325 Pa = 760 torr)?

A)46.91 torr

B)267.4 torr

C)351.8 torr

D)3612 torr

E)2.709 ×10⁴ torr

Q2) Determine the molar mass of Freon-11 gas if a sample weighing 0.597 g occupies 100 cm³ at 95°C and 1000 mmHg (R = 0.08206 L atm/K mol, 1 atm = 760 mmHg).

A)0.19 g/mol

B)35.3 g/mol

C)70.9 g/mol

D)137 g/mol

E)384 g/mol

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Chapter 9: Physical Properties of Solutions

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Sample Questions

Q1) The distinguishing characteristic of all electrolyte solutions is that they A)contain molecules.

B)conduct electricity.

C)react with other solutions.

D)always contain acids.

E)conduct heat.

Q2) The distinguishing characteristic of all nonelectrolyte solutions is that they A)contain ions.

B)do not conduct electricity.

C)react with other solutions.

D)always contain acids.

E)conducts heat.

Q3) What volume of a 2.75 M solution of NaOH is required to make 500.0 mL of a 1.27 M solution of NaOH?

A)231 mL

B)1.72 L

C)1.10 L

D)440 mL

E)909 mL

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Chapter 10: Chemical Reactions and Chemical Equations

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Sample Questions

Q1) If aqueous solutions of KMnO₄, FeSO₄ and H₂SO_4, are mixed, which ions are spectator ions?

2KMnO₄(aq) + 10FeSO₄(aq) + 8H₂SO₄(aq) K₂SO₄(aq) + 2MnSO₄(aq) + 5Fe₂(SO₄)₃(aq) + 8H₂O(l)

A)only K⁺

B)only SO₄²

C)only K⁺and SO₄²

D)only K⁺, SO₄²_, and Fe²⁺

E)only K⁺, SO₄², Fe²⁺, and Mn²⁺

Q2) Which of these chemical equations describes a metal displacement reaction?

A)2NaN₃(s) 2Na(s) + 3N₂(g)

B)Fe₂O₃(s) + 2Al(s) 2Fe(s) + Al₂O₃(s)

C)3NO₂(g) + H₂O(l) 2HNO₃(aq) + NO(g)

D)2P(s) + 3Cl₂(g) 2PCl₃(g)

E)2ZnS(s) + 3O₂(g) 2ZnO(s) + 2SO₂(g)

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Page 12

Chapter 11: Using Balanced Chemical Equations

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Sample Questions

Q1) What volume of 0.200 M H₂SO₄ solution is required to react exactly with 50.0 mL of 0.100 M KOH? H₂SO₄(aq) + 2KOH(aq) 2H₂O(l) + K₂SO₄(aq)

A)62.5 mL

B)12.5 mL

C)50.0 mL

D)25.0 mL

E)75.0 mL

Q2) How much heat is released if 35.0 g of ethanol (C₂H₅OH) burns in excess oxygen? C₂H₅OH(l) + 3O₂(g) 2CO₂(g) + 3H₂O(l) heat of reaction = 1367 kJ/mol

A)1797 kJ

B)1367 kJ

C)9.61 × 10⁴ kJ

D)4.78 × 10⁴ kJ

E)1040 kJ

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Chapter 12: Acids and Bases

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Sample Questions

Q1) Which solution is the most acidic?

A)pH = 1.00

B)pH = 10.00

C)pH = 5.00

D)pH = 3.00

E)pH = 4.00

Q2) Which is a strong base?

A)LiOH

B)CH₃COOH

C)NH₃

D)H₃PO₄

E)HClO₂

Q3) A solution with a pH of 8.15 is

A)slightly acidic.

B)very basic.

C)neutral.

D)very acidic.

E)slightly basic.

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Chapter 13: Equilibrium

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Sample Questions

Q1) If, in a particular process, reactants are able to form products, and products are also able to form reactants, then this process may be described as

A)a reversible process.

B)an elementary process.

C)at equilibrium.

D)forbidden.

E)a forward process.

Q2) Which substances are included in the equilibrium constant expression, K_c?

A)Only pure solids

B)Only pure liquids

C)Only pure solids and liquids

D)Only gases and dissolved substances

E)All participating substances

Q3) At equilibrium, the rate of the forward reaction is equal to the rate of the reverse reaction.

A)True

B)False

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15

Chapter 14: Organic Chemistry

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Sample Questions

Q1) Which type of organic compound does not contain a carbonyl group?

A)Ethers

B)Carboxylic acids

C)Ketones

D)Aldehydes

E)Esters

Q2) How are aromatic compounds defined?

A)Organic compounds that contain the benzene ring

B)Organic compounds that do not contain the benzene ring

C)Inorganic compounds that do not contain the benzene ring

D)Inorganic compounds that contain the benzene ring

E)Compounds containing double bonds

Q3) What name is given to a compound containing a COOH group?

A)Aldehyde

B)Ketone

C)Alcohol

D)Carboxylic acid

E)Ester

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Chapter 15: Biochemistry

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Sample Questions

Q1) Which of the following describes a protein?

A)A molecules composed of three small sugar molecules.

B)A relatively small, water-soluble molecule that contains either a ketone or an aldehyde functional group.

C)A large biological polymer composed of amino acids.

D)And ester of phosphoric acid where one or more of the ionizable hydrogen atoms has been replaced by an R group.

E)A tri-ester of glycerol where each of the hydroxyl-group hydrogen atoms in glycerol has been replaced by the alkyl group of a relatively long hydrocarbon chain carboxylic acid.

Q2) 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.

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Chapter 16: Nuclear Chemistry

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Sample Questions

Q1) Cesium-134 is a emitter with a half-life of 2.0 years.How much of a 2.50-g sample of cesium-134 will remain after 10 years?

A)0.0024 g

B)0.078 g

C)0.25 g

D)0.50 g

E)80.0 g

Q2) Uranium-235 decays by alpha emission.What isotope is also produced by this transformation?

A)Pa-234

B)Th-237

C)Pu-237

D)Th-231

E)Pu-239

Q3) Beta particles are identical to A)protons.

B)helium atoms.

C)hydrogen atoms.

D)helium nuclei.

E)electrons.

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Chapter 17: Electrochemistry

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Sample Questions

Q1) Consider the following balanced redox reaction.3CuO(s) + 2NH₃(aq) N₂(g) + 3H₂O(l) + 3Cu(s) Which of the following statements is ?

A)CuO(s) is the oxidizing agent and copper is reduced.

B)CuO(s) is the oxidizing agent and copper is oxidized.

C)CuO(s) is the reducing agent and copper is oxidized.

D)CuO(s) is the reducing agent and copper is reduced.

E)CuO(s) is the oxidizing agent and N₂(g) is the reducing agent.

Q2) When the following redox equation is balanced with the smallest whole number coefficients, what is the coefficient for nitrogen dioxide? I₂(s) + HNO₃(aq) HIO₃(aq) + NO₂(g) + H₂O(l)

A)1

B)2

C)4

D)5

E)10

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