Course Introduction
Chemistry for Engineers Practice
Questions
Chemistry for Engineers provides engineering students with a foundational understanding of chemical principles and their practical applications in engineering contexts. The course covers essential topics such as atomic structure, chemical bonding, thermodynamics, chemical kinetics, equilibrium, and materials science. Special emphasis is placed on the relevance of chemistry in areas like corrosion, energy production, environmental engineering, and the selection of construction materials. Through lectures and laboratory experiments, students learn to apply chemical concepts to solve real-world engineering problems and gain skills needed for innovation in various engineering fields.
Recommended Textbook Chemistry 6th Edition by John E. McMurry
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Page 2
Chapter 1: Chemistry: Matter and Measurement
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Sample Questions
Q1) Which of the following volumes is equal to 40 mL?
A)40 cm<sup>3</sup>
B)40 dm<sup>3</sup>
C)0)40 L
D)0)000 40 kL
Answer: A
Q2) The factor 10<sup>-2</sup> corresponds to which prefix?
A)deka
B)deci
C)centi
D)milli
Answer: C
Q3) If hitting the bull's-eye is the desired result,Figure (a)represents
A)good accuracy and good precision.
B)good accuracy and poor precision.
C)poor accuracy and good precision.
D)poor accuracy and poor precision.
Answer: C
Q4) Stored energy is ________ energy,and energy of motion is ________ energy.
Answer: potential,kinetic
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Chapter 2: Atoms, molecules, and Ions
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Sample Questions
Q1) Which of the following statements concerning ionic compounds is true?
A)Essentially all ionic compounds are solids at room temperature and pressure.
B)Ionic compounds do not contain any covalent bonds.
C)Ionic compounds contain the same number of positive ions as negative ions.
D)The chemical formula for an ionic compound must show a nonzero net charge.
Answer: A
Q2) 10% saline solution (sodium chloride dissolved in water)is an example of a ________ mixture.
Answer: homogeneous
Q3) Which of the above drawings represents a Cl<sup>-</sup> ion?
A)drawing (a)
B)drawing (b)
C)drawing (c)
D)drawing (d)
Answer: A
Q4) The subatomic particles contained in the nucleus of an atom are ________ and ________.
Answer: protons,neutrons
Q5) The number of neutrons in a neutral atom of uranium-238 is ________.
Answer: 146
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Chapter 3: Formulas, equations, and Moles
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Sample Questions
Q1) If the percent yield for the following reaction is 75.0%,and 45.0 g of NO<sub>2</sub> are consumed in the reaction,how many grams of nitric acid,HNO<sub>3</sub>(aq)are produced?
3 NO<sub>2</sub>(g)+ H<sub>2</sub>O(l) 2 HNO<sub>3</sub>(aq)+ NO(g)
A)30.8 g
B)41.1 g
C)54.8 g
D)69.3 g
Answer: A
Q2) Combustion analysis of 1.200 g of an unknown compound containing carbon,hydrogen,and oxygen produced 2.086 g of CO<sub>2</sub> and 1.134 g of H<sub>2</sub>O.What is the empirical formula of the compound?
A)C<sub>2</sub>H<sub>5</sub>O
B)C<sub>2</sub>H<sub>5</sub>O<sub>2</sub>
C)C<sub>2</sub>H<sub>10</sub>O<sub>3</sub>
D)C<sub>3</sub>H<sub>8</sub>O<sub>2</sub>
Answer: D
Q3) The fundamental SI unit for measuring matter is the ________. Answer: mole
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Page 5
Chapter 4: Reactions in Aqueous Solutions
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Sample Questions
Q1) What reagent could be used to separate Br<sup>-</sup> from CH<sub>3</sub>CO<sub>2</sub><sup>- </sup>when added to an aqueous solution containing both?
A)AgNO<sub>3 </sub>(aq)
B)Ba(OH)<sub>2 </sub>(aq)
C)CuSO<sub>4 </sub>(aq)
D)NaI <sub>(</sub><sub>aq</sub><sub>)</sub>
Q2) Which pair of compounds is insoluble in water?
A)AgNO<sub>3</sub> and KNO<sub>3</sub>
B)Na<sub>2</sub>S and CuS
C)(NH<sub>4</sub>)<sub>2</sub>SO<sub>4</sub> and AgI
D)PbSO<sub>4</sub> and Pb<sub>3</sub>(PO<sub>4</sub>)<sub>2</sub>
Q3) How many H<sup>+</sup> ions can the acid H<sub>3</sub>PO<sub>4</sub> donate per molecule?
A)0
B)1
C)2
D)3
Q4) Metals that do not react with hydrochloric acid to produce hydrogen gas are found ________ H<sub>2</sub> in the activity series.
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Chapter 5: Periodicity and the Atomic Structure of Atoms
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Sample Questions
Q1) What are the possible values of l if n = 3?
A)3
B)0,1,or 2
C)-4,-3,-2,-1,0,+1,+2,+3,or +4
D)-5,-4,-3,-2,-1,0,+1,+2,+3,+4,or +5
Q2) What is the first ionization energy for a hydrogen atom in the ground state? The Rydberg constant is
1)097 × 10<sup>-2</sup> nm<sup>-1</sup>.
A)7)27 × 10<sup>-36</sup> J
B)1)63 × 10<sup>-27</sup> J
C)2)18 × 10<sup>-18</sup> J
D)0)00823 J
Q3) Wave (b)has the
A)higher frequency and higher energy than wave (a).
B)higher frequency and lower energy than wave (a).
C)lower frequency and higher energy than wave (a).
D)lower frequency and lower energy than wave (a).
Q4) In a representation of an orbital,a region having zero probability of finding an electron is called a ________.
Q5) Copper has the anomalous electron configuration ________.
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Chapter 6: Ionic Bonds and Some Main-Group Chemistry
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Sample Questions
Q1) Of the following,which element has the highest first ionization energy?
A)Ca
B)K
C)Li
D)Mg
Q2) Which contains covalent bonds?
A)NaH and HCl
B)only HCl
C)only NaCl
D)only NaH
Q3) Predict the product(s)when the reactants Be(s)+ Br<sub>2</sub>(l)are mixed.
A)BeBr(s)
B)BeBr<sub>2</sub>(s)
C)Be<sub>2</sub>Br(s)
D)BeBr<sub>3</sub>(s)
Q4) Using shorthand notation,the ground-state electron configuration for C<sup>4-</sup> is predicted to be ________.
Q5) Potassium reacts with oxygen to form a superoxide with the formula ________.
Q6) Using shorthand notation,the ground-state electron configuration for Tl<sup>+</sup> is predicted to be ________.
Page 8
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Chapter 7: Covalent Bonds and Molecular Structure
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Sample Questions
Q1) What is the hybridization of the nitrogen atom?
A)sp
B)sp<sup>2</sup>
C)sp<sup>3</sup>
D)None of these
Q2) Which type of bond produces a charge cloud with a nodal plane containing the bond axis?
A)
B)
C) and D)neither nor
Q3) The orbital hybridization on the carbon atom in HCN is A)sp.
B)sp<sup>2</sup>.
C)sp<sup>3</sup>.
D)None of these
Q4) Of H<sub>2</sub>CO and CO and CO<sub>2</sub>,the compound having the strongest C-O bond is ________.
Q5) Of NH<sub>4</sub><sup>+</sup><sub> </sub>and NH<sub>4</sub><sup>-</sup><sub> </sub>the one with the smaller bond angles is
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Chapter 8: Thermochemistry: Chemical Energy
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Sample Questions
Q1) At 253 K the sign of G for the physical change shown below is ________. H<sub>2</sub>O(s) H<sub>2</sub>O(l)
Q2) 10.0 g of a metal,initially at 25°C,are placed into 10.0 g of water,initially at 100°C.Which metal will have the highest final temperature? Shown after each metal is its specific heat in J/(g°C).
A)aluminum (0.902)
B)copper (0.385)
C)Gold (0.129)
D)iron (0.450)
Q3) For the reaction,NH<sub>3</sub>(g) N(g)+ 3 H(g),one would expect
A) H° to be negative and S° to be negative.
B) H° to be negative and S° to be positive.
C) H° to be positive and S° to be negative.
D) H° to be positive and S° to be positive.
Q4) At a given temperature and pressure,which of the following would be expected to have the greatest molar entropy?
A)Br<sub>2</sub>(s)
B)Br<sub>2</sub>(l)
C)Br<sub>2</sub>(g)
D)All of these would be expected to have the same molar entropy.
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Chapter 9: Gases: Their Properties and Behavior
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Sample Questions
Q1) How many liters of SO<sub>3</sub>(g)are produced at 25°C and 1.00 atm from the combustion of 1.00 kg of coal which is 1.00% S by weight? Assume all the sulfur in the coal ends up as SO<sub>3</sub>.
A)0)640 L
B)5)08 L
C)7)63 L
D)11.4 L
Q2) Each of three identical 15.0-L gas cylinders contains 7.50 mol of gas at 295 K.Cylinder A contains Ar,cylinder B contains Cl<sub>2</sub>,and cylinder C contains N<sub>2</sub>.According to the kinetic molecular theory,which gas has the highest pressure?
A)Ar
B)Cl<sub>2</sub>
C)N<sub>2</sub>
D)All have identical pressures
Q3) According to the kinetic molecular theory of gases,what is the force of attraction of one N<sub>2</sub> molecule for another N<sub>2</sub> molecule?
Q4) If one mole of gas occupies 22.4 L at STP the same gas would occupy ________ than 22.4 L at 25°C and 738 mm Hg.
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Chapter 10: Liquids,solids,and Phase Changes
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Sample Questions
Q1) The coordination number of each atom in a simple cubic unit cell is ________.
Q2) The Br-Cl bond has 5.05% ionic character and a dipole moment of 0.518 D.What is the distance between atoms in BrCl?
Q3) Manganese crystallizes in a body-centered cubic structure.What is the coordination number of each atom?
A)4
B)6
C)8
D)12
Q4) In the drawing of acetaldehyde,CH<sub>3</sub>CHO,the largest partial negative charge ( -)occurs on
A)atom (a).
B)atom (b).
C)atom (c).
D)atom (d).
Q5) What is the empirical formula of the mineral?
A)MM'A
B)MM'A<sub>3</sub>
C)M<sub>2</sub>M'A<sub>3</sub>
D)M<sub>8</sub>M'A<sub>6</sub>
Page 12
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Chapter 11: Solutions and Their Properties
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Sample Questions
Q1) What is the approximate boiling temperature of a mixture that is 0.70 X<sub>A</sub> and 0.30 X<sub>B</sub>?
A)50°C
B)75°C
C)95°C
D)100°C
Q2) Substances with high lattice energies tend to be less soluble than substances with low lattice energies.On that basis predict the relative aqueous solubility at 20°C,from highest to lowest,of the following ionic compounds:
Ce<sub>2</sub>(SO<sub>4</sub>)<sub>3</sub>,K<sub>2</sub>SO<sub>4</sub>,KBr,Na Cl.
A)Ce<sub>2</sub>(SO<sub>4</sub>)<sub>3</sub> > K<sub>2</sub>SO<sub>4</sub> > KBr > NaCl
B)Ce<sub>2</sub>(SO<sub>4</sub>)<sub>3</sub> > K<sub>2</sub>SO<sub>4</sub> > NaCl > KBr
C)KBr > NaCl > K<sub>2</sub>SO<sub>4 </sub>>
Ce<sub>2</sub>(SO<sub>4</sub>)<sub>3</sub>
D)NaCl > KBr > K<sub>2</sub>SO<sub>4 </sub>> Ce<sub>2</sub>(SO<sub>4</sub>)<sub>3</sub>
Q3) Molarity is defined as ________,whereas molality is defined as ________.
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Chapter 12: Chemical Kinetics
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Sample Questions
Q1) The decomposition of ozone in the stratosphere can occur by the following two-step mechanism:
Br + O<sub>3</sub> BrO + O<sub>2</sub>
BrO + O Br + O<sub>2</sub>
Which species is a catalyst in this mechanism?
A)Br
B)BrO
C)O
D)O<sub>3</sub>
Q2) An aqueous reaction occurs by a two-step mechanism,shown below.
Step 1: A<sub>2</sub>X<sub>2</sub> + Y A<sub>2</sub>X + XY
Step 2: A<sub>2</sub>X<sub>2</sub> + XY A<sub>2</sub>X + X<sub>2</sub> + Y
What is the catalyst in this reaction?
A)A<sub>2</sub>X
B)X<sub>2</sub>
C)XY
D)Y
Q3) Platinum in the catalytic converter of an automobile catalyzes the conversion of CO to CO<sub>2</sub> is an example of a ________ (heterogeneous,homogeneous)catalyst.
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Chapter 13: Chemical Equilibrium
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Sample Questions
Q1) The decomposition of ammonia is: 2 NH<sub>3</sub>(g)= N<sub>2</sub>(g)+ 3 H<sub>2</sub>(g).If K<sub>p</sub> is 1.5 × 10<sup>3</sup> at 400°C,what is the partial pressure of ammonia at equilibrium when N<sub>2</sub> is 0.10 atm and H<sub>2</sub> is 0.15 atm?
A)2)2 × 10<sup>-7</sup> atm
B)4)7 × 10<sup>-4</sup> atm
C)2)1 × 10<sup>3</sup> atm
D)4)4 × 10<sup>6</sup> atm
Q2) What is the value of the equilibrium constant K<sub>c</sub> for the reaction A B?
A)K<sub>c</sub> = 0.33
B)K<sub>c</sub> = 3.0
C)K<sub>c</sub> = 12
D)K<sub>c</sub> = 27
Q3) What is the best balanced chemical equation for the reaction?
A)A<sub>2</sub> + B A<sub>2</sub>B
B)A<sub>2</sub> + 2 B A<sub>2</sub>B<sub>2</sub>
C)A<sub>2</sub> + 2 B 2 AB
D)6 A<sub>2</sub> + 9 B 3 A<sub>2</sub> + 3B + 6 AB
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Chapter 14: Aqueous Equilibria: Acids and Bases
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Sample Questions
Q1) Which acid,if any,is a strong acid?
A)All are strong acids.
B)HX and HZ
C)HY
D)None are strong acids.
Q2) Identify the Br nsted-Lowry acid/base conjugate pairs.
A)(1)/(2)and (3)/(4)
B)(1)/(3)and (2)/(4)
C)(1)/(4)and (2)/(3)
Q3) Which is not a hydrate of a proton?
A)H<sub>3</sub>O<sup>+</sup>
B)H<sub>9</sub>O<sub>4</sub><sup>+</sup>
C)H<sub>25</sub>O<sub>11</sub><sup>+</sup>
D)H<sub>43</sub>O<sub>21</sub><sup>+</sup>
Q4) Calculate the pH for an aqueous solution of pyridine that contains 2.15 × 10<sup>-4</sup> M hydroxide ion.
A)4)65 × 10<sup>-11</sup>
B)2)15 × 10<sup>-4 </sup>
C)3)67
D)10.33
Page 16
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Chapter 15: Applications of Aqueous Equilibria
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Sample Questions
Q1) If solution (1)is a saturated solution of CuS,which of solutions (2)-(4)are saturated?
A)(2)
B)(3)
C)(4)
D)None of these
Q2) A buffer prepared by mixing equal moles of an acid having K<sub>a</sub> = 4.5 × 10<sup>-4</sup> and a salt of its conjugate base has a pH = ________.
Q3) A buffer solution is prepared by dissolving 0.200 mol of NaH<sub>2</sub>PO<sub>4</sub> and 0.100 mol of NaOH in enough water to make 1.00 L of solution.What is the pH of the H<sub>2</sub>PO<sub>4</sub><sup>-</sup>/HPO<sub>4</sub><sup>2-</sup> buffer if the
K<sub>a2</sub> = 6.2 × 10<sup>-8</sup>?
A)6)91
B)7)21
C)7)51
D)7)71
Q4) The artist's pigment cadmium yellow,CdS,has a water solubility of 0.13 g/L.The solubility product of CdS,K<sub>sp</sub> = ________.
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Chapter 16: Thermodynamics: Entropy, free Energy, and Equilibrium
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Sample Questions
Q1) Which electron on an atom of copper would have the highest value of W in the Boltzmann formula?
A)3s
B)3d
C)4s
D)4p
Q2) The chemical system shown below is at equilibrium.Which change in conditions will not result in a spontaneous forward reaction?
N<sub>2</sub>(g)+ 3 H<sub>2</sub>(g) 2 NH<sub>3</sub>(g)K<sub>p</sub> = 4 × 10<sup>5</sup>
A)adding a catalyst
B)adding more H<sub>2</sub>
C)adding more N<sub>2</sub>
D)reducing the volume
Q3) The standard free energy for a reaction is G° = -33.0 kJ.At 25°C the equilibrium constant for this reaction,K<sub>p</sub> = ________.
Q4) The entropy of water at 25° is ________ than the entropy of water at 35°C.
Q5) What is the entropy of 10 molecules in a system of 1000 boxes?
Q6) What is the entropy of 10 molecules in a system of 100 boxes?
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Chapter 17: Electrochemistry
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Sample Questions
Q1) Calculate the value of the reaction quotient,Q,for the galvanic cell expressed using shorthand notation below.Use the balanced chemical equation that has the smallest whole number stoichiometric coefficients.
Zn(s) Zn<sup>2+</sup>(aq,0.0100 M) Ag+(aq,1.25 M) Ag(s)
A)156
B)125
C)8)00 × 10<sup>-3</sup>
D)6)40 × 10<sup>-3</sup>
Q2) In the relationship G = -nFE°,what is the value of n for the reaction shown below?
3 Cu<sup>2+(</sup><sup>aq</sup>)+ 2 Al(s) 3 Cu(s)+ 2 Al<sup>3+</sup>(aq)
A)1
B)2
C)3
D)6
Q3) According to Table 17.1,which will reduce water but not Mg<sup>2+</sup>?
A)Al<sup>3+</sup>(aq)
B)Al(s)
C)Na<sup>+</sup>(aq)
D)Na(s)
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Chapter 18: Hydrogen, oxygen, and Water
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Sample Questions
Q1) Which oxide has the highest melting point?
A)A
B)B
C)C
D)D
Q2) A binary compound that forms when potassium reacts with oxygen has the composition 58.96% Na and 41.04% O.What is the formula of one formula unit of this compound?
A)Na<sub>2</sub>O
B)NaO
C)NaO<sub>2</sub>
D)Na<sub>2</sub>O<sub>2</sub>
Q3) What is the oxidation number of oxygen in KO<sub>2</sub>?
A)0
B)-1/2
C)-1
D)-2
Q4) At 25°C the dissociation constant K<sub>w</sub> for T<sub>2</sub>O is 0.06 × 10<sup>-14</sup>.What is the molar concentration of OT<sup>-</sup> in 0.025 M TCl?
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Chapter 19: The Main-Group Elements
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Sample Questions
Q1) White tin is the high temperature form of the metal.Given that the density of gray tin is 5.769 g/cm<sup>3</sup> and that of white tin is 7.28 g/cm<sup>3</sup> raising the pressure will favor the
A)more dense allotrope and lower the transition temperature of 13.2°C.
B)more dense allotrope and raise the transition temperature of 13.2°C.
C)less dense allotrope and lower the transition temperature of 13.2°C.
D)less dense allotrope and raise the transition temperature of 13.2°C.
Q2) What statement is inconsistent about graphite?
A)Carbon sheets are separated by a distance of 335 pm and are held together by weak London dispersion forces.
B)Electrical conductivity parallel to the planar sheets is 10<sup>20</sup> times greater than the conductivity of diamond.
C)Pi electrons are delocalized and free to move perpendicular to the plane of the hexagonal sheets.
D)A two-dimensional sheetlike structure in which each C atom uses sp<sup>2</sup> hybrid orbitals.
Q3) Why is H<sub>3</sub>PO<sub>4</sub> a weak triprotic acid whereas H<sub>3</sub>PO<sub>3</sub> is a weak diprotic acid?
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21
Chapter 20: Transition Elements and Coordination Chemistry
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Sample Questions
Q1) What is the oxidation state of the Co atom in [Co(NH<sub>3</sub>)<sub>5</sub>Cl](NO<sub>3</sub>)<sub>2</sub>?
A)+2
B)+3
C)+4
D)+6
Q2) The color exhibited by coordination compounds is usually due to the absorption of light by a d-electron,resulting in the promotion of the d-electron from its ground-state d-orbital to a higher energy orbital.The first transition series element expected to have a colorless aqueous solution M<sup>2+</sup> ion is ________.
Q3) Which has the largest atomic radius?
A)Y
B)Mo
C)Rh
D)Cd
Q4) The number of diastereoisomers possible for [Co(en)<sub>2</sub>Cl<sub>2</sub>]<sup>+</sup> is ________.
Q5) The coordination number of chromium in [Cr(EDTA)]<sup>-</sup> is ________.
Q6) Copper has the anomalous short-hand electron configuration ________.
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Chapter 21: Metals and Solid-State Materials
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Sample Questions
Q1) In the reaction shown below calcium phosphate slag is formed from a reaction of calcium oxide with phosphoric anhydride.
6 CaO(s)+ P<sub>4</sub>O<sub>10</sub>(l) 2 Ca<sub>3</sub>(PO<sub>4</sub>)<sub>2</sub>(l)
CaO is a(n)________ oxide,and P<sub>4</sub>O<sub>10 </sub>is a(n)________ oxide.
A)acidic,acidic
B)acidic,basic
C)basic,acidic
D)basic,basic
Q2) According to band theory,which one of the following metals is expected to have the highest melting point?
A)Cd
B)Cr
C)Hg
D)Zn
Q3) Which of these elements is likely to be found in nature as an oxide?
A)element A
B)element B
C)element C
D)element D
Page 23
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Chapter 22: Nuclear Chemistry
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Sample Questions
Q1) What type of shielding can be used to protect against gamma rays?
A)cloth
B)lead
C)wood
D)No shielding is effective against gamma rays.
Q2) The masses of <sup>4</sup>He,<sup>6</sup>Li,and <sup>10</sup>B are 4.0015,6.0135,and 10.0102 amu respectively.The fission of a boron-10 nucleus into He-4 and Li-6 would
A)absorb energy.
B)evolve energy.
C)result in no energy change.
D)Need more information
Q3) A few sheets of ordinary paper can form an effective shield against what type of radiation?
A)alpha particles
B)cosmic rays
C)gamma rays
D)neutrons
Q4) The mass defect for the chemical reaction shown below is ________ g.
2 F F<sub>2</sub> E = -159 kJ/mol
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Chapter 23: Organic and Biological Chemistry
Available Study Resources on Quizplus for this Chatper
285 Verified Questions
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Sample Questions
Q1) "Wood alcohol" is the common name for A)methanol.
B)ethanol.
C)2-propanol.
D)1,2-ethanediol.
Q2) Which one of the following amino acids contains a polar side chain?
A)alanine
B)glycine
C)threonine
D)valine
Q3) Which one of the following amino acids contains a hydrophobic side chain?
A)leucine
B)serine
C)threonine
D)tyrosine
Q4) Which of the following amino acids contains a benzyl group?
A)glycine
B)isoleucine
C)methionine
D)phenylalanine
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