Chem 2 final

Write the formula of the conjugate acid of the Brønsted-Lowry base, (CH₃)₃N

(CH3)3NH+

What is the rate of reaction in terms of C in the following reaction: A + B → 2 C.

+0.5∆[C]/∆t

The pH of a 0.0040 M solution of HNO₃ is

2.4

For which of the following equations would the value of Kp = Kc(RT)? A) A (g) + 2 B (s) ⇌ C (s) + 2 D (g) B) 2 NO₂ (g) ⇌ N₂O₄ (g) C) 2 NBr₃ (g) ⇌ N₂ (g) + 3 Br₂ (g) D) 2 HI (g) ⇌ H₂ (g) + I₂ (g)

A (g) + 2 B (s) ⇌ C (s) + 2 D (g)

Which of the following occurs during positron emission? A) Atomic number decreases B) Atomic mass increases C) Number of neutrons decreases D) All of the above E) None of the above

Atomic number decreases

Which of the following is described by the following characteristics? a very hard, colorless substance melting at about 3000 °C A) BN B) P₄S₃ C) Pb D) CaCl₂ E) C₆H₁₂O₆

BN

In the reaction below, the Lewis base is BeCl₂ + 2 Cl⁻ → BeCl₄²⁻

Cl-

Which of the following substances contains MOSTLY ionic bonding? A) LiF B) CO₂ C) AlCl₃ D) BeCl₂ E) Cu

LiF

a high Ka has a lower

pKa

The rate of a reaction increases when a catalyst has been added to the reaction mixture. The catalyst _____

provides a new mechanism for the reaction to proceed by

Heavy nuclides with too few neutrons to be in the band of stability are most likely to decay by what mode? A) α-particle production B) fission C) positron production D) β⁻ production E) none of these

α-particle production

The isotope ⁶⁹Zn undergoes what mode of radioactive decay? A) α emission B) β⁻ emission C) electron capture D) γ emission E) positron emission

β⁻ emission

Complete the following nuclear bombardment equation by filling in the nuclear symbol for the missing species. ²³⁵₉₂U + ¹₀n → ? + ¹³⁹₅₄Xe + 3 ¹₀n A) ⁹⁴₄₈Cd B) ⁹⁶₃₈Cm C) ⁹⁴₃₈Pu D) ⁹⁴₃₈Sr E) ⁹⁶₃₈Sr

⁹⁴₃₈Sr

Which of the following is always true for an equilibrium? A) ∆S = 0 B) ∆H = 0 C) ∆G = 0 D) T = 298 K E) K = 0

∆G = 0

Which of the following is true for a reaction when K is much less than one? A) ∆G° = K B) ∆G° = large negative number C) ∆G° = large positive number D) ∆G° = small negative number E) ∆G° = small positive number

∆G° = large positive number

As E°(cell) increases: A) ∆G° increases B) ∆G° decreases C) ∆G° remains the same D) Not enough info

∆G° decreases

For the reaction 2 A + 3 B → 4 D + 5 E, how is the rate of reaction expressed in terms of rate of disappearance of B? A) ∆[B]/∆t B) -∆B/∆t C) +1/3∆[B]/∆t D) -1/3∆[B]/∆t E) +3∆[B]/∆t

-1/3∆[B]/∆t

The decay constant for the element X is 6.931 yr⁻¹. What is the half-life? A) 0.6931 years B) 6.931 years C) 10 years D) 1 year E) 0.1 years

0.1 years

Which of the following combinations can be used to make a buffer? (Assume equal volumes are used.) A) 0.30 M HCN and 0.30 M HBr B) 0.30 M HCN and 0.15 M HBr C) 0.30 M HCN and 0.30 M NaOH D) 0.30 M HCN and 0.15 M NaOH

0.30 M HCN and 0.15 M NaOH

How many atoms are there in a simple cubic unit cell? A) 1 B) 4 C) 6 D) 8 E) 12

1

Which of the following are spontaneous processes? 1. Ice melting at 273 K (assume only ice is initially present). 2. Heat flowing from a hot object to a cold object. 3. An iron bar rusting. A) 1 only B) 2 only C) 3 only D) 1 and 3 only E) 1, 2, and 3

1, 2, 3

Which statements describes why ethyl methyl ether (b.p. 7.9°C) and 1-propanol (b.p. 97.2°C) have such different boiling points despite identical molar masses?

1-propanol has more hydrogen bonding than ethyl methyl ether

Which of the following would have the greatest amount (in moles) of the original isotope remaining? A) 1.0 g of Fe-59 after 100 days (half life = 44.5 days) B) 1.0 g of S-35 after 100 days (half life = 87 days) C) 1.0 g of P-32 after 100 days (half life = 14.3 days) D) 1.0 g of Cu-64 after 100 days (half life = 12.7 hours) E) 1.0 g of I-131 after 100 days (half life = 8.0 days)

1.0 g of S-35 after 100 days (half life = 87 days)

What is the balanced reaction for the cell diagram below? Al(s) | Al³⁺(aq) || Cd²⁺(aq) | Cd(s) A) Al³⁺(aq) + Cd(s) → Al(s) + Cd²⁺(aq) B) 2 Al(s) + 3 Cd²⁺(aq) → 2 Al³⁺(aq) + 3 Cd(s) C) 3 Al³⁺(aq) + 2 Cd(s) → 3 Al(s) + 2 Cd²⁺(aq) D) Al(s) + Cd²⁺(aq) → Al³⁺(aq) + Cd(s) E) 2 Al³⁺(aq) + 3 Cd(s) → 2 Al(s) + 3 Cd²⁺(aq)

2 Al(s) + 3 Cd²⁺(aq) → 2 Al³⁺(aq) + 3 Cd(s)

During the electrolysis of molten NaI, what reaction occurs at the anode? A) I⁻(l) + e⁻ → I₂⁻(l) B) 2 I⁻(l) → I₂(g) + 2e⁻ C) NaI(l) → NaI₂(l) D) 2 I⁻(l) + e⁻ → I₂(g) E) Na⁺(l) + e⁻ → Na(l)

2 I⁻(l) → I₂(g) + 2e⁻

For the reaction 2 H₂(g) + O₂(g) → 2 H₂O(g), which equation would be used to determine the entropy change? (H2= A, O2= B, H2O= C) A) (2A + B) - 2C B) C - (A + B) C) 2C - (2A + B) D) 2A + B + 2C E) 2C - (A + B)

2C-(2A+B)

A uranium-235 nucleus decays by a series of alpha and beta emissions until it reaches lead-207. How many alpha emissions and how many beta emissions occur in this series of decays? A) 7 α and 4 β⁻ decays B) 4 α and 7 β⁻ decays C) 5 α and 5 β⁻ decays D) 7 α and 10 β⁻ decays E) Cannot be determined

7 α and 4 β⁻ decays

Which of the following is the cell diagram for the reaction 3 Pb²⁺+(aq) + 2 Al(s) → 3 Pb(s) + 2 Al³⁺(aq)? A) Pb(s) | Pb²⁺(aq) || Al³⁺(aq) | Al(s) B) Pb²⁺(aq) | Pb(s) || Al³⁺(aq) | Al(s) C) Pb(s) | Pb²⁺(aq) || Al(s) | Al³⁺(aq) D) Al(s) | Al³⁺(aq) || Pb²⁺(aq) | Pb(s) E) Al³⁺(aq) | Al(s) || Pb(s) | Pb²⁺(aq)

Al(s) | Al³⁺(aq) || Pb²⁺(aq) | Pb(s)

When two He atoms undergo fusion in a star, the resulting element is: A) H B) Li C) Be D) He E) All of the above

Be

Which of the following has the lowest boiling point?

C5H12 (smaller compounds)

Which of the following pairs of substances has the higher vapor pressure at 298 K given first? A) H₂O, H₂Se B) CF₄, CBr₄ C) Kr, Ne D) C₆H₁₄, C₄H₁₀ E) CH₃OH, CH₃OCH₃

CF4, CBr4

Which one of the following correctly ranks the compounds in order of lowest boiling point to highest boiling point based only in intermolecular forces? A) CH₃CH₂OH < CH₃OCH₃ < CH₃CH₂CH₃ B) CH₃OCH₃ < CH₃CH₂CH₃ < CH₃CH₂OH C) CH₃CH₂CH₃ < CH₃CH₂OH < CH₃OCH₃ D) CH₃CH₂CH₃ < CH₃OCH₃ < CH₃CH₂OH

CH₃CH₂CH₃ < CH₃OCH₃ < CH₃CH₂OH

Which one of the following correctly ranks the compounds in order of lowest vapor pressure to highest vapor pressure based only in intermolecular forces? A) CH₃CH₂OH < CH₃OCH₃ < CH₃CH₂CH₃ B) CH₃OCH₃ < CH₃CH₂CH₃ < CH₃CH₂OH C) CH₃CH₂CH₃ < CH₃CH₂OH < CH₃OCH₃ D) CH₃CH₂CH₃ < CH₃OCH₃ < CH₃CH₂OH

CH₃CH₂OH < CH₃OCH₃ < CH₃CH₂CH₃

Which of the following reactions would have the most positive ∆S° value? A) SO₂(g) + Na₂O(s) ⟶ Na₂SO₃(s) B) CO₂(s) ⟶ CO₂(g) C) Fe³⁺(aq) + SCN⁻(aq) ⟶ FeSCN²⁺(aq) D) N₂(g) + 3 H₂(g) ⟶ 2 NH₃(g) E) 2 NO(g) + Cl₂(g) ⟶ 2 NOCl(g)

CO₂(s) ⟶ CO₂(g) (goes from a high solid to a disordered gas)

Which one of the following is a strong base? A) Mg(OH)₂ B) Ca(OH)₂ C) NH₃ D) CH₃OH

Ca(OH)2

For which of the following aqueous solutions will a decrease of pH increase the solubility? A) CaCO₃ B) PbCl₂ C) CuBr D) AgCl

CaCO3

Which of the following might be best described by the following set of properties? 1. white solid melting at 772 °C 2. solid does not conduct electricity 3. solid dissolves in water to form a conducting solution

CaCl2

In the reaction below, which reactant is the Lewis acid? Cr³⁺ + 6 H₂O → Cr(H₂O)₆³⁺

Cr3+

A galvanic cell is represented by the shorthand Cu | Cu²⁺ || Ag⁺ | Ag. Which reaction occurs at the anode? A) Cu(s) → Cu²⁺(aq) + 2e⁻ B) Ag⁺(aq) + e⁻ → Ag(s) C) Cu²⁺(aq) + 2e⁻ → Cu(s) D) Ag(s) → Ag⁺(aq) + e⁻

Cu(s) → Cu²⁺(aq) + 2e⁻

Which of the following aqueous solutions will not be more soluble under acidic conditions? A) Ag₂SO₄ B) ZnF₂ C) Mg(OH)₂ D) CuBr

CuBr (does not contain a base)

Write the basic equilibrium equation for C₆H₅NH₂

C₆H₅NH₂(aq) + H₂O(l) ⇌ OH⁻(aq) + C₆H₅NH₃⁺(aq)

What intermolecular forces are present in both molecules of CH₃CH₂OH and CH₃CH₂NH₂?

Dispersion forces, dipole-dipole forces, and hydrogen bonding.

An electrolytic cell converts: A) Chemical energy into electrical energy B) Chemical energy into mechanical energy C) Mechanical energy into electrical energy D) Electrical energy into chemical energy

Electrical energy into chemical energy

Which of these terms describes the following process? ²³⁹₉₄Pu → ²³⁵₉₂U + ⁴₂He²⁺ A) Chemical B) Fusion C) Exothermic

Exothermic

Which of the following reactions accurately shows how Fe³⁺ acts as an acid in water? A) Fe(OH)₃ (s) ⇌ Fe³⁺ (aq) + 3 OH⁻ (aq) B) Fe³⁺ (aq) + 5 H₂O (l) ⇌ Fe(H₂O)₅³⁺ (aq) C) Fe(H₂O)₆³⁺ (aq) ⇌ Fe(H₂O)₅(OH)²⁺ (aq) + H⁺ (aq) D) Fe³⁺ (aq) + 3 OH⁻ (aq) ⇌ Fe(OH)₃ (s)

Fe(H₂O)₆³⁺ (aq) ⇌ Fe(H₂O)₅(OH)²⁺ (aq) + H⁺ (aq)

Which of the following is a Lewis acid? A) Fe³⁺ B) CN⁻ C) NH₃ D) SCN⁻

Fe^3+

What type of nuclear process requires extremely high temperatures to occur? A) Fission B) Fusion C) Transmutation D) Neutron emission E) Gamma ray emission

Fusion

What unit represents the 1 Joule of radiation absorbed by one kilogram of matter? A) Rad B) Rem C) Gray D) Curie E) Becquerel

Gray

what is a hydronium ion

H+

Which one of the following 1.0 M solutions would have the highest pH? A) C₅H₅N= 1.7x10^-9 B) HONH₂= 1.1x10^-8 C) C₆H₅NH₂= 4.3x10^-10 D) H₂NNH₂= 1.3x10^-6

H2NNH2

Which is expected to have the lowest vapor pressure? CH3, SiH4, NH3, PH3, H2O

H2O

Which of the following phase changes is not spontaneous at room temperature? Assume only the first phase is initially present. A) H₂O(g) → H₂O(l) B) H₂O(s) → H₂O(g) C) H₂O(s) → H₂O(l) D) H₂O(g) → H₂O(s) E) They are all spontaneous.

H2O (g) -> H2O (s)

Write the formula of the conjugate acid of the Brønsted-Lowry base, H₂PO₄⁻

H3PO4

Write the acidic equilibrium equation for HC₂H₃O₂

HC₂H₃O₂(aq) + H₂O(l) ⇌ H₃O⁺(aq) + C₂H₃O₂⁻(aq)

Which of the following will be the strongest acid? A) HIO B) HIO₂ C) HIO₃ D) HIO₄

HIO4 (the more oxygen, the stronger the acid)

Rank the following solutions in order from most acidic to least acidic. A) HNO₃ > HNO₂ > NaNO₃ > NaNO₂ B) NaNO₂ > NaNO₃ > HNO₂ > HNO₃ C) HNO₃ > NaNO₃ > NaNO₂ > HNO₂ D) HNO₃ > HNO₂ > NaNO₂ > NaNO₃

HNO₃ > HNO₂ > NaNO₃ > NaNO₂

Which of the following should exhibit the highest viscosity at 298 K?

HOCH₂CH₂OH

Which of the following is a conjugate acid/base pair? A) H₃PO₄, PO₄³⁻ B) H₂PO₄⁻, PO₄³⁻ C) HPO₄²⁻, PO₄³⁻ D) H₃PO₄, HPO₄²⁻

HPO4^2-, PO4^3-

Which of the following processes has a negative ∆S? A) CaCO₃(s) → CaO(s) + CO₂(g) B) H₂O(g) → H₂O(s) C) CO₂(s) → CO₂(g) D) C₆H₁₂O₆(s) → C₆H₁₂O₆(aq) E) ∆S cannot be negative

H₂O(g) → H₂O(s)

Which types of processes are likely when the neutron-to-proton ratio in a nucleus is too large? I. α decay II. β⁻ decay III. positron production IV. electron capture

II only

Which of the following statements regarding a gamma ray is true? A) It is less penetrating than a beta ray. B) It is not deflected by an electric field. C) It is composed of neutrons. D) It is less penetrating than an alpha ray. E) None of these statements are true.

It is not deflected by an electric field.

Which of the following indicates a spontaneous reaction under standard conditions? A) K = 8.6 x 10⁻² B) K = 7.9 x 10⁻⁸ C) K = 2.2 x 10² D) K = 9.2 x 10⁻⁴⁵ E) K = 0.14

K = 2.2 x 10²

Which of the following is a Lewis base? A) CO₂ B) BF₃ C) NH₃ D) NO₂

NH3

Write the formula of the conjugate base of the Brønsted-Lowry acid, NH₄⁺

NH3

which of the following exhibits dipole-dipole intermolecular forces in a pure substance

NH3

Which of the following reactions results in an increase in the entropy of the system? A) CH₄(g) + 2O₂(g) → CO₂(g) + 2H₂O(g) B) BaO(s) + CO₂(g) → BaCO₃(s) C) NH₄Cl(s) → HCl(g) + NH₃(g) D) 2HCl(g) + F₂(g) → 2HF(g) + Cl₂(g) E) 4Co(s) + 3O₂(g) → 2Co₂O₃(s)

NH₄Cl(s) → HCl(g) + NH₃(g)

Electrolyzing molten NaCl produces what products at the cathode and anode, respectively? A) Na(l), Cl₂(g) B) Cl₂(g), Na(l) C) Na⁺(aq), Cl⁻(aq) D) Cl⁻(aq), Na⁺(aq) E) Na(l), Cl(l)

Na(l), Cl₂(g)

Which of the following substances has the highest melting point? A) NaCl B) Cl₂ C) NO₂ D) CH₄ E) H₂S

NaCl

In an electron capture process, which of the following occurs? A) Number of electrons increases B) Number of protons increases C) Number of neutrons increases D) All of the above E) None of the above

Number of neutrons increases

for the reaction mechanism show, idenify the intermediates (s). A. O B. O2 C. O3 D. O and O2 E. O2 and O3

O

what is a hydroxide ion

OH-

Consider the reaction in a lead storage battery below. Which of the following statements is correct? PbO₂(s) + Pb(s) + 2 H₂SO₄(aq) ⇌ 2 PbSO₄(s) + 2 H₂O(l) A) Pb is formed at the anode during use of the battery. B) Pb²⁺ is formed at the cathode during use of the battery. C) The mass of Pb decreases during recharging. D) The concentration of H₂SO₄ increases during use of the battery. E) The mass of PbSO₄ remains constant during use and recharging of the battery.

Pb²⁺ is formed at the cathode during use of the battery.

What is ionizing radiation? A) Radiation that exists as a plasma. B) Radiation required to initiate a fission reaction. C) Radiation that can cause ionization processes to occur. D) Radiation that occurs as charged ions. E) Radiation that is required to initiate a fusion reaction.

Radiation that can cause ionization processes to occur.

Which species has the greatest rate of appearance in the reaction below? 2 H₂S + O₂ → 2 S + 2 H₂O

S and H₂O have identical rates

Which of the compounds below is an example of a network solid? A) C₂₅H₂₅(s) B) NaCl(s) C) SiO₂(s) D) S₈(s) E) MgO(s) +

SiO2

Which of the following best describes the third law of thermodynamics? A) ∆U(univ) = ∆U(sys) + ∆U(surr) B) S° = 0 for perfect Li(s) at 0 K C) ∆S(univ) > 0 (spontaneous process) D) ∆S = ∆H(rev)/T at constant T E) ∆G = ∆H - T∆S

S° = 0 for perfect Li(s) at 0 K

A decrease of pH by 3 implies

The OH⁻ concentration decreases by a factor of 1000.

Which of the following describes the entropy change in the given reaction? 2 Cl₂O₇(g) → 2 Cl₂(g) + 7 O₂(g) A) The entropy change is negative because a larger molecule (Cl₂O₇) is converted into two smaller molecules (Cl₂ and O₂). B) The entropy change is zero because the reactants and products are all gases. C) The entropy change cannot be determined because the temperature is not specified. D) The entropy change is negative because there are more moles of products than reactants. E) The entropy change is positive because there are more moles of products than reactants.

The entropy change is positive because there are more moles of products than reactants.

Considering the rate law, rate = k[A]²[B], which of the following statements is correct?

The reaction is first order in B and third order overall

The stable nuclide ²⁰⁶₈₂Pb is formed from ²³⁸₉₂U by a long series of α and β⁻ decays. Which of the following nuclides could NOT be involved in this decay series? A) Th-234 B) U-239 C) Po-218 D) Bi-214 E) Rn-222

U-239

Given the standard electrode reduction potentials, which reaction will occur spontaneously? A) V²⁺ + 2Cu⁺ → V + 2Cu²⁺ B) Mg²⁺ + V → V²⁺ + Mg C) Mg²⁺ + 2Cu⁺ → 2Cu²⁺ + Mg D) Mg²⁺ + V²⁺→ Mg + V E) V + 2Cu²⁺ → V²⁺ + 2Cu⁺

V + 2Cu²⁺ → V²⁺ + 2Cu⁺

Considering the activity series of increasing reactivities (Cu < Sn < Fe < Zn < Mg), which metal(s) could be used to protect steel (Fe)? A) Cu or Sn B) Cu only C) Sn only D) Mg only E) Zn or Mg

Zn or Mg

Which of the following equations describes the calculation for the half-life of a zero-order reaction?

[A]₀/2k

Consider the following rate law: Rate = k[B] Which of the following equations could be used to find the concentration of B at some time (t) in the reaction?

[B] = [B]₀ × e^(-kt)

Which of the following is the correct expression for the concentration based equilibrium constant for the reaction: Mg(OH)₂ (s) ⇌ Mg²⁺ (aq) + 2 OH⁻ (aq)

[MG2+][OH]2

Which of the following is the correct expression for Ksp for Zn₃(PO₄)₂?

[Zn2+]^3[PO43-]^2

Which of the following statements is true? A) A buffer forms when any acid or base are mixed together. B) A buffer forms when a strong acid is mixed with a weak acid. C) A buffer forms when a conjugate weak acid/weak base pair are mixed together. D) A buffer forms when a weak acid is mixed with a weak base.

a buffer forms when a conjugate weak acid/weak base pair are mixed together

Which of the following statements is false about catalysts? A) Enzymes are biological catalysts. B) A catalyst is consumed in a chemical reaction. C) A catalyst increases reaction rate by providing an alternate reaction pathway with a lower activation energy. D) A catalyst may undergo change during a reaction but is unchanged at the end of a reaction. E) Catalysts may be homogeneous or heterogeneous.

a catalyst is consumed in a chemical reaction

The conversion of CO(g) to CO₂(g) is sped up by introducing CO(g) to solid platinum. This makes platinum: A) A homogeneous inhibitor B) A heterogeneous inhibitor C) A homogeneous catalyst D) A heterogeneous catalyst E) None of the above

a heterogeneous catalyst

If the Gibbs free energy for an equilibrium is a large, negative number, the equilibrium constant is expected to be _____ A) a large, negative value B) a large, positive value C) a small, negative value D) a small, positive value E) Zero

a large, positive value

pOH>7 implies what

a solution is acidic

Which one of the following statements is true? A) A solution with a pH of 3.40 will have a higher concentration of hydroxide ions than hydronium ions. B) A solution with a pOH of 2.10 is very acidic. C) A solution with a pH of 8.20 is only slightly basic. D) A solution with a pOH of 13.20 is very basic.

a solution with a pH of 8.20 is only slightly basic.

Which of the following is not true about a spontaneous process? A) A spontaneous process is one that continues on its own once begun. B) Spontaneous processes occur naturally. C) A nonspontaneous process does not occur unless some external action is applied. D) A nonspontaneous process does not mean it cannot ever occur under any conditions. E) A spontaneous process is also spontaneous in the reverse direction.

a spontaneous process is also spontaneous in the reverse direction

Which of the following would decrease the solubility of a 0.10 M solution of Ag₂CO₃ the most? (Ksp of Ag₂CO₃ is 8.1 × 10⁻¹²)

adding 0.10 M Ag+

The second law of thermodynamics states that _____ A) no engine can be 100% efficient. B) transferring energy from a cold to a hot bath requires work. C) the entropy of the universe increases with a spontaneous process. D) all of these are true.

all of these are true

Which of the following will decrease the rate of a reaction? A) Removing a catalyst from the reaction. B) Decreasing the temperature. C) Decreasing the surface area of a solid reactant. D) Decreasing the concentration of the reactants. E) All of these will decrease the rate of a reaction.

all of these will decrease the rate of a reaction

Which of the following liquid substances has the highest vapor pressure at its normal boiling point?

all would have the same vapor pressure at their normal boiling points

Which of the following represents the three main types of radiation ranked by increasing penetrating ability? A) alpha < beta < gamma B) alpha < gamma < beta C) beta < alpha < gamma D) beta < gamma < alpha E) gamma < beta < alpha

alpha < beta < gamma

Which of the following has the greatest mass? A) α particle B) neutron C) proton D) β⁻ particle E) neutrino

alpha particle

Which of the following processes decreases the atomic number by two? A) gamma-ray production B) beta production C) positron-particle production D) alpha-particle production E) proton production +

alpha particle production

A reaction which is exothermic and has an overall increase in entropy is A) spontaneous only at high T B) spontaneous only at low T C) always spontaneous D) spontaneous in the reverse direction.

always spontaneous

When NO₂ dimerizes (two molecules join together to form a 'dimer') into N₂O₄, an equilibrium is reached and in the process this reaction produces heat. If you increase the temperature of the chamber in which both NO₂ and N₂O₄ reside, you would observe

an increase in NO2

In a voltaic (galvanic) cell, oxidation occurs at the _____ and is where _____ in the salt bridge moves toward. A) cathode, anions B) cathode, cations C) anode; anions D) anode, cations E) salt bridge, both cations and anions

anode; anions

Reversible processes: A) Do not conserve energy B) Do not conserve momentum C) Are impossible in real life D) Are possible only at high temperatures

are impossible in real life

Negatively charged particles of radiation emitted from the decay of radioactive substances are known as A) protons B) alpha particles C) beta particles D) neutrons E) gamma rays

beta particles

what is the molecularity of step 1 in the proposed mechanism? Step 1: Cl + O3 -> ClO + O2

bimolecular

Compared to HCO₃⁻, H₂CO₃ has a A) Higher Ka B) Lower Ka C) Lower pKa D) Higher pKa E) Both (A) and (C)

both A and C

Based on their positions in the periodic table, which of the following bonds is the most polar? A) C - O B) C - N C) C - B D) C - F

c-f

Which of the factors contributes to a low viscosity of a liquid? A) high boiling point B) hydrogen bonding C) compact molecular shape D) low temperature E) high molar mass

compact molecular shape

The formation of green patina (copper carbonate) on a copper roof protecting the underlying copper metal is an example of _____ A) corrosion B) cathodic protection C) electrolytic protection D) galvanization E) amalgamation

corrosion

What is the smallest amount of fissionable material required to sustain a chain reaction? A) limiting mass B) critical mass C) mass defect D) critical defect E) critical limit

critical mass

What is the effect on k as the activation energy for a reaction increases? A) Increases B) Decreases C) Stays the same D) Not enough info

decreases

What intermolecular forces are present between two molecules of CH₃CH₂SH?

dispersion and dipole-dipole

the predominant intermolecular force between molecules is

dispersion forces

what intermolecular forces are present in CH3F and CF4

dispersion only

Which of the following bonds is a nonpolar covalent bond? A) H - F B) N - F C) F - Cl D) F - F

f-f

Which one of the following statements is false? A) For a triprotic acid, Ka3 > Ka2. B) A triprotic acid will have three simultaneous equilibria occurring. C) For a diprotic acid, Ka1 > Ka2. D) A diprotic acid will have only one amphoteric species in its acid equilibrium series.

for a triprotic acid, Ka3 > Ka2

which one of the following phase changes would be exothermic

freezing

Which type of radiation has the greatest penetrating ability? A) alpha particle B) beta particle C) positron D) gamma ray E) all radiation has the same penetrating ability

gamma ray

What type of radiation can be used to kill bacteria in food? A) alpha particles B) beta particles C) positrons D) gamma rays E) protons

gamma rays

which of the following bonds is a polar covalent bond?

h-cl

a crystal of NaCl is

hard, high melting, and a poor electrical conductor

For the reaction: Mg(OH)₂ (s) ⇌ Mg²⁺ (aq) + 2 OH⁻ (aq) Adding Mg(OH)₂ will

have no effect because adding more solid will have no effect

Which of the following properties is not typical of metallic solids? A) High coordination number of atoms in the lattice. B) High vapor pressure. C) High electrical conductivity. D) High thermal conductivity. E) All of the above are true statements.

high vapor pressure

Ammonia and hydrogen fluoride both have unusually high boiling points due to _____

hydrogen bonding

Forming solution A from liquid B and liquid C is endothermic. Increasing the temperature of the solution will

increase the solubility of B

which best explains why the trend in noble gas boiling points increases down the group

increasing dispersion interactions

Consider the reaction below. Which of the following would increase the partial pressure of B at equilibrium? A (s) + B (g) ⇌ C (g) ΔH < 0

increasing the temperature

Which of the following changes would cause the reaction below to shift in the forward direction to reestablish equilibrium? 2 NBr₃ (g) ⇌ N₂ (g) + 3 Br₂ (g)

increasing the total volume of the container

Alpha particles interacting with matter typically lose energy by what process? A) radical formation B) ionization C) neutralization D) heat transfer E) heat absorption

ionization

Which of the following is true about the total entropy of the universe? A) It is always increasing B) It is always decreasing C) It remains constant at a given T D) It always remains constant

it is always increasing (second law of thermodynamics)

HI is an Arrhenius acid because

it produces hydronium ions in solution

Which of the following is true about a spontaneous process? A) It releases energy. B) It will occur quickly. C) It will continue on its own once begun. D) It is never endothermic.

it will continue on its own once begun

Which of the following is an example of an ionic bond? A) K - F B) C - H C) Kr - H D) C - F

k-f

Which acid-base definition classifies an acid as an electron-pair acceptor?

lewis

Which of the following is a means of creating a buffer of H₂CO₃/NaHCO₃? A) Mixing 10 mL of 1 M HNO₃ with 10 mL of 1 M NaHCO₃ B) Adding 5 mL of 1 M HNO₃ to 10 mL of 1 M H₂CO₃ C) Adding 10 mL of 1 M NaOH to 10 mL of 1 M NaHCO₃ D) Mixing 5 mL of 1 M HNO₃ with 10 mL of 1 M NaHCO₃

mixing 5 mL of 1 M HNO3 with 10 mL of 1 M NaHCO3

a cathode is a ________ sided electrode

negative

The nuclide ²⁰⁰₅₀X is most likely to decay by ___ A) alpha decay. B) electron capture. C) neutron emission. D) proton emission. E) positron decay.

neutron emission.

Consider the following reaction: CH₃COOH(aq) + H₂O(l) ⇌ CH₃COO⁻(aq) + H₃O⁺(aq). An increase in the pressure of the chamber where this reaction takes place will result in

no change due to it not being a gaseous species

what does it mean when ksp > Qsp

no precipitate is formed

a anode is a __________ sided electrode

positive

A battery that cannot be recharged is classified as a _____ A) primary battery B) secondary battery C) fuel cell D) electrolytic cell

primary battery

Catalysts increase reaction rates by _____

providing an alternate reaction mechanism with a lower activation energy

If the reaction X + 2 Y → XY₂ occurs by the proposed mechanism, what is the rate law?

rate = k[X][Y]

Consider the proposed mechanism for the decomposition reaction 2 H₂O₂(aq) → 2 H₂O(l) + O₂(g) in the presence of I⁻(aq). What is the rate law for this reaction?

rate= k[H2O2][I-]

As the concentration of reactants decreases in a galvanic cell, the magnitude of E°(cell) will: A) Increase B) Decrease C) Remain the same D) Not enough info

remain the same

If a plot of 1/[A] versus time produces a straight line with a positive slope for the reaction A → B + C, what is the order of the reaction?

second

Which of the following phases does a sample of water exist in at its triple point?

solid, liquid, gas

Which of the following affects the collision rate of molecules in the gas phase?

speed, mass, and molecular diameter

A reaction which is endothermic and has an overall increase in entropy is A) spontaneous only at high T B) spontaneous only at low T C) always spontaneous as written. D) always spontaneous in the reverse direction.

spontaneous only at high T

which of the following phase changes is endothermic?

sublimation

Which term is a measure of the energy required to increase the surface area of a liquid?

surface tension

What is the molecularity of the rate-determining step in the proposed mechanism? H2 + 2NO -> N2O + H2O

termolecular

Electrons always flow in a voltaic (galvanic) cell from _____ A) the salt bridge to the anode B) the oxidizing agent through the salt bridge to the reducing agent C) the reducing agent through the salt bridge to the oxidizing agent D) the anode to cathode E) the salt bridge to the cathode

the anode to the cathode

The reason an ionic bond forms can best be described as

the energy change for electron transfer results in a large gain in stability when the ionic bond forms

Which best explains why the meniscus of mercury in a glass tube is convex?

the lower attraction of mercury to the glass than to itself

All of the following are factors that affect the rate of a reaction except _____ A) the concentration of the reactants. B) presence of a catalyst. C) the magnitude of the equilibrium constant. D) the temperature of the reaction. E) the surface area of the solid reactants.

the magnitude of the equilibrium constant

the larger the ksp ->

the more soluble the salt is in water

Which of the following is true for a reaction at equilibrium? A) The rate of the forward reaction is greater than the rate of the reverse reaction. B) The rate of the forward reaction is less than the rate of the reverse reaction. C) The rate of the forward reaction is equal to the rate of the reverse reaction. D) The rates of the forward and reverse reactions become zero because the reaction stops. E) The rates of the forward and reverse reactions can no longer be determined.

the rate of the forward reaction is equal to the rate of the reverse reaction

For the reaction below, Q = 600. What must happen for the reaction to reach equilibrium? 2 A (g) + B (s) ⇌ 2 C (s) + D (g) Kp = 8210

the reaction needs to shift in the forward directions

If the reaction quotient (Q) for a given reaction is less than the equilibrium constant (K) then A) the reaction will proceed in the forward direction. B) The reaction will proceed in the reverse direction. C) the reaction is at equilibrium.

the reaction will proceed in the forward direction

Consider the following acidic equilibrium: H₂CO₃(aq) + H₂O(l) ⇌ HCO₃⁻(aq) + H₃O⁺(aq). If you add NaHCO₃ to this solution, which of the following will occur?

the reaction will shift in the reverse direction

A solution has a pOH of 7.84. This tells us

the solution is only slightly acidic

The higher the Kb,

the stronger the weak base

Which of the following statements about solid copper, with a face-centered cubic unit cell, is incorrect? A) It will conduct electricity. B) There are two atoms per unit cell. C) The number of atoms surrounding each copper atom is 12. D) The solid has a cubic closest-packed structure. E) The length of a face diagonal is four times the radius of copper.

there are two atoms per unit cell

The reaction rate of a reaction at 60 °C will be greater than at 30°C because _____ A) the higher temperature leads to greater surface area on solid or liquid reactants. B) the reactants at 60°C will be moving with too great of a speed to collide effectively. C) the activation energy will be lower at 60°C. D) there is a greater proportion of reactants with the necessary kinetic energy to react. E) there is a greater likelihood that the reactants will have the correct orientation to collide effectively.

there is a greater proportion of reactants with the necessary kinetic energy to react

Which law states that the entropy of a perfect crystalline substance is zero at the absolute zero of temperature? A) Zeroth law of thermodynamics B) First law of thermodynamics C) Second law of thermodynamics D) Third law of thermodynamics E) Law of conservation of energy

third law of thermodynamics

in a covalent bond

two atoms share valence electrons and those shared electrons form the chemical bond

single, double, or triple covalent bonds in a carbon atom are formed from

valence electrons

What phase change is represented by the transition from liquid to gas? A) fusion B) sublimation C) vaporization D) condensation E) solidification

vaporization

which term is a measure of the resistance to flow in a liquid

viscosity

Complete the following nuclear decay process: ²³⁵₉₂U → ⁴₂He + ___ A) ²³⁹₉₄Pu B) ²³¹₉₄Pu C) ²³¹₉₂U D) ²³¹₉₀Th E) ²³⁹₉₀Th

²³¹₉₀Th

Enriched uranium fuel used in fission reactors is that which contains a greater amount of A) ²³⁵U B) ²³⁸U C) ²⁰⁹Pb D) deuterium (²H) E) tritium (³H)

²³⁵U

²¹⁰Pb decays by emitting a β⁻ particle. What nuclide is produced? A) ²¹⁰Bi B) ²¹⁰Pb C) ²¹⁰Hg D) ²¹⁰Tl E) ²⁰⁶Hg

²¹⁰Bi

Polonium was discovered in uranium ores by Marie and Pierre Curie. Polonium-210 decays by emitting a single alpha particle. What nuclide is formed in this process? A) ²⁰⁶Pb B) ²¹⁰At C) ²⁰⁹Pb D) ²¹⁰Bi E) ²¹⁴Rn

²⁰⁶Pb

What isotope is commonly used to determine thyroid activity and treat diseases of the thyroid? A) ¹¹C B) ⁶⁰Co C) ¹³¹I D) ⁹⁹Tc E) ¹⁰B

¹³¹I

What nuclide undergoes electron capture to produce ¹⁰⁸Pd? A) ¹⁰⁸Rh B) ¹⁰⁷Ag C) ¹⁰⁷Pd D) ¹⁰⁸Ag E) ¹⁰⁷Rh

¹⁰⁸Ag

Which of the following is true for a particular reaction if ∆G° is -40.0 kJ/mol at 290 K and -20.0 kJ/mol at 390 K? A) ∆H >0 , ∆S > 0 B) ∆H < 0, ∆S < 0 C) ∆H > 0, ∆S < 0 D) ∆H < 0, ∆S > 0 E) None of these

∆H < 0, ∆S < 0

Which set of results applies to a reaction that is not spontaneous at 273 K but is spontaneous at 400 K? A) ∆H < 0 and ∆S > 0 B) ∆H > 0 and ∆S > 0 C) ∆H < 0 and ∆S < 0 D) ∆H > 0 and ∆S < 0 E) None of these

∆H > 0 and ∆S > 0

A reaction will be spontaneous at all temperatures if _____ A) ∆H and ∆S are positive B) ∆H and ∆S are negative C) ∆H is positive and ∆S is negative D) ∆H is negative and ∆S is positive

∆H is negative and ∆S is positive

Which of the following best describes the reaction? 2 H₂S(g) + 3 O₂(g) → 2 H₂O(g) + 2 SO₂(g) A) ∆S° has a large negative value. B) ∆S° has a small negative value. C) ∆S° has a large positive value. D) ∆S° has a small positive value. E) ∆S° is zero.

∆S° has a small negative value. (count number of moles, 5:4 slightly negative)

Which of the following is true for a system at equilibrium? A) ∆S°(sys) = ∆S°(surr) B) ∆S°(sys) = -∆S°(surr) C) ∆S°(sys) = ∆S°(surr) = 0 D) ∆S°(sys) = ∆S°(univ) E) ∆S°(surr) = ∆S°(univ)

∆S°(sys) = -∆S°(surr)