Fundamentals of General Organic and Biological Chemistry 8th Edition By McMurray - Peterson - Test Bank

Fundamentals of General Organic and Biological Chemistry 8th Edition By McMurray – Peterson – Test Bank

 

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Fundamentals of General, Organic, and Biological Chemistry, 8e (McMurry)

Chapter 5   Classification and Balancing of Chemical Reactions

 

1) In a balanced chemical equation

1. A) there are equal numbers of atoms on each side of the reaction arrow.
2. B) there are equal numbers of molecules on each side of the reaction arrow.
3. C) there are always the same number of products as there are reactants.
4. D) the number of atoms present in a reaction can vary when the conditions change during the reaction.
5. E) none of the above

Answer:  A

Diff: 2

Section:  5.1

LO:  5.1

Global LO:  G2

 

2) Consider the balanced equation shown and identify the statement that is not true.

 

Na2SO4(aq) + BaCl2(aq) → 2 NaCl(aq) + BaSO4(s)

 

1. A) The coefficient of sodium sulfate is one.
2. B) Barium sulfate is produced in solid form.
3. C) Barium chloride is dissolved in water.
4. D) The products are barium sulfate and sodium chloride.
5. E) 2 NaCl (aq) could also be correctly written as Na2Cl2(aq).

Answer:  E

Diff: 1

Section:  5.1

LO:  5.1

Global LO:  G7

 

3) In a precipitation reaction the insoluble product can be identified by the symbol

1. A) (aq).
2. B) (l).
3. C) (g).
4. D) (s).
5. E) none of the above

Answer:  D

Diff: 1

Section:  5.1

LO:  5.1

Global LO:  G2

 

4) Consider the reaction shown and identify the statement that is not true.

 

CaCO3(s)  CaO(s) + CO2(g)

 

1. A) This reaction is balanced as written.
2. B) The reactant must be heated for this reaction to occur.
3. C) The products are a solid and a gas.
4. D) Water must be present for this reaction to occur.
5. E) There are no solutions used in this reaction.

Answer:  D

Diff: 1

Section:  5.1

LO:  5.1

Global LO:  G2

 

5) The scientific principle which is the basis for balancing chemical equations is

1. A) the Law of Conservation of Energy.
2. B) the Law of Conservation of Mass.
3. C) the Law of Conservation of Mass and Energy.
4. D) the Law of Definite Proportions.
5. E) Avogadro’s Law.

Answer:  B

Diff: 2

Section:  5.1

LO:  5.1

Global LO:  G6

 

6) Which statement regarding balanced chemical equations is not true?

1. A) The number of each kind of atom must be the same on each side.
2. B) Coefficients are used in front of formulas to balance the equation.
3. C) Subscripts may be changed to make an equation simpler to balance.
4. D) When no coefficient is written in front of a formula, the number “one” is assumed.
5. E) Reactants are written to the left of the arrow.

Answer:  C

Diff: 2

Section:  5.2

LO:  5.2

Global LO:  G2, G4

 

 

7) Which is the correct equation for the reaction of magnesium with hydrochloric acid to produce hydrogen and magnesium chloride?

1. A) Mg + 2 HCl → H2+ MgCl2
2. B) Mg + HCl → H + MgCl
3. C) 2 Mg + 6 HCl → 3 H2+ 2 MgCl2
4. D) Mg + 2 HCl → 2 H + MgCl2
5. E) Mg + 3 HCl → 3 H + MgCl2

Answer:  A

Diff: 2

Section:  5.2

LO:  5.2

Global LO:  G2, G4

8) Which of the following equations is not balanced?

1. A) 2 Na + 2 H2O → 2 NaOH + H2
2. B) C3H8+ 5 O2→ 3 CO2 + 4 H2O
3. C) 2 H2+ O2→ 2 H2O
4. D) SO2+ O2→ SO3
5. E) 2 Al + 6 HCl → 2 AlCl3+ 3 H2

Answer:  D

Diff: 2

Section:  5.2

LO:  5.2

Global LO:  G2, G4

 

9) Which of the following equations is not balanced?

1. A) C7H16+ O2→ 7 CO2 + 8 H2O
2. B) K2CrO4+ Pb(NO3)2→ 2 KNO3 + PbCrO4
3. C) 4 Fe3O4+ O2→ 6 Fe2O3
4. D) 3 AgNO3+ (NH4)3PO4→ Ag3PO4 + 3 NH4NO3
5. E) 2 Al2O3→ 4 Al + 3 O2

Answer:  A

Diff: 2

Section:  5.2

LO:  5.2

Global LO:  G2, G4

 

 

10) When the reaction shown is correctly balanced, the coefficients are:

 

________ KClO3 → ________ KCl + ________ O2

 

1. A) 1; 1; 1
2. B) 2; 2; 2
3. C) 2; 2; 3
4. D) 2; 2; 1
5. E) 4; 4; 6

Answer:  C

Diff: 2

Section:  5.2

LO:  5.2

Global LO:  G2, G4

11) When the reaction shown is correctly balanced, the coefficients are:

 

________ C6H14(l) + ________ O2(g) → ________ CO2(g) + ________ H2O(g)

 

1. A) 1; 6; 6; 7
2. B) 2; 19; 12; 14
3. C) 1; 3.5; 6; 7
4. D) 1; 9.5; 6; 7
5. E) 2; 16.5; 12; 7

Answer:  B

Diff: 2

Section:  5.2

LO:  5.2

Global LO:  G2, G4

 

12) When the following reaction is balanced, the coefficient in front of carbon dioxide is:

 

________ C5H12 + ________ O2 → ________ CO2 + ________ H2O

 

1. A) 5
2. B) 6
3. C) 12
4. D) 10
5. E) 11

Answer:  A

Diff: 1

Section:  5.2

LO:  5.2

Global LO:  G2, G4

 

 

13) When the following reaction is balanced, the coefficient in front of oxygen is:

 

________ C8H18 + ________ O2 → ________ CO2 + ________ H2O

 

1. A) 25
2. B) 12
3. C) 18
4. D) 9
5. E) 17

Answer:  A

Diff: 3

Section:  5.2

LO:  5.2

Global LO:  G2, G4

14) In the correctly balanced reaction, the coefficient for H2O is:

 

________ Al(OH)3 + ________ H2SO4 → ________ Al2(SO4)3 + ________ H2O

 

1. A) 1
2. B) 2
3. C) 3
4. D) 6
5. E) 8

Answer:  D

Diff: 2

Section:  5.2

LO:  5.2

Global LO:  G2, G4

 

15) When the reaction shown is correctly balanced, the coefficients are:

 

________ HBr + ________ Ca(OH)2 → ________ CaBr2 + ________ H2O

 

1. A) 2; 1; 1; 1
2. B) 1; 1; 1; 2
3. C) 2; 1; 1; 2
4. D) 2; 2; 1; 1
5. E) 2; 1; 2; 2

Answer:  C

Diff: 2

Section:  5.2

LO:  5.2

Global LO:  G2, G4

 

 

16) When the reaction shown is correctly balanced, the coefficients are:

 

________ Li + ________ Br2 → ________ LiBr

 

1. A) 1; 1; 1
2. B) 1; 2; 2
3. C) 1; 2; 1
4. D) 2; 2; 1
5. E) 2; 1; 2

Answer:  E

Diff: 2

Section:  5.2

LO:  5.2

Global LO:  G2, G4

17) When the reaction shown is correctly balanced, the coefficients are:

 

________ HNO3 + ________ KOH → ________ KNO3 + ________ H2O

 

1. A) 0; 0; 0; 0
2. B) 1; 1; 1; 1
3. C) 2; 2; 2; 2
4. D) 3; 1; 1; 3
5. E) 2; 1; 2; 1

Answer:  B

Diff: 2

Section:  5.2

LO:  5.2

Global LO:  G2, G4

 

18) When the reaction shown is balanced, there are ________ atoms of oxygen and ________ atoms of hydrogen on each side.

 

_______ (NH4)2SO4(aq) + _______ Ba(C2H3O2)2(aq) → _______ BaSO4(s) + _______ NH4C2H3O2(aq)

 

1. A) 6; 11
2. B) 16; 18
3. C) 8; 14
4. D) 4; 7
5. E) 16; 28

Answer:  C

Diff: 3

Section:  5.2

LO:  5.2

Global LO:  G2, G4

 

 

19) The balanced equation for the reaction occurring when calcium nitrate solution is mixed with sodium phosphate solution is

1. A) 3 Ca(NO3)2(aq) + 2 Na3PO4(aq) → Ca3(PO4)2(aq) + 6 NaNO3(aq).
2. B) 2 Ca(NO3)2(aq) + 3 Na3PO4(aq) → 2 Ca3(PO4)2(s) + 6 NaNO3(aq).
3. C) 3 CaNO3(aq) + Na3PO4(aq) → Ca3PO4(aq) + 3 NaNO3(s).
4. D) 3 Ca(NO3)2(aq) + 2 Na3PO4(aq) → Ca3(PO4)2(s) + 6 NaNO3(aq).
5. E) Ca(NO3)2(aq) + 2 NaPO4(aq) → Ca(PO4)2(s) + 2 NaNO3(aq).

Answer:  D

Diff: 3

Section:  5.3

LO:  5.3

Global LO:  G2, G4

20) The balanced equation for the reaction occurring when iron(III) oxide, a solid, is reduced with pure carbon to produce carbon dioxide and molten iron is

1. A) 2 Fe3O(s) + C(s) → 6 Fe(l) + CO2(g).
2. B) 2 FeO3(s) + 3 C(s) → 2 Fe(l) + 3 CO2(g).
3. C) 4 Fe2O3(s)+ 6 C s) → 8 Fe l) + 6 CO2(g).
4. D) 2 FeO(s) + C s) → 2 Fe l) + CO2(g).
5. E) 2 Fe2O3(s)+ 3 C(s) → 4 Fe l) + 3 CO2(g).

Answer:  E

Diff: 3

Section:  5.3

LO:  5.3

Global LO:  G2, G4

 

21) The balanced equation for the reaction between aqueous ammonium sulfate and aqueous barium acetate is

1. A) (NH4)2SO4(aq) + Ba(C2H3O2)2(aq) → BaSO4(s) + NH4C2H3O2(aq).
2. B) (NH4)2SO4(aq) + Ba(C2H3O2)2(aq) → BaSO4(s) + 2 NH4C2H3O2(aq).
3. C) NH4SO4(aq) + BaC2H3O2(aq) → BaSO4(s) + NH4C2H3O2(aq).
4. D) (NH4)2SO4(aq) + Ba(C2H3O2)2(aq) → BaSO4(aq) + 2 NH4C2H3O2(s).
5. E) (NH4)2SO3(aq) + Ba(C2H3O2)2(aq) → BaSO3(aq) + NH4C2H3O2(aq).

Answer:  B

Diff: 3

Section:  5.3

LO:  5.3

Global LO:  G2, G4

 

 

22) The reaction 2 AgNO3(aq) + K2SO4(aq) → 2 KNO3(aq) + Ag2SO4(s) is an example of a(an) ________ reaction.

1. A) acid-base
2. B) oxidation-reduction
3. C) precipitation
4. D) combustion
5. E) none of the above

Answer:  C

Diff: 1

Section:  5.3

LO:  5.3

Global LO:  G2

 

23) Which reaction is an example of a precipitation reaction?

1. A) H2CO3(aq) → H2O(l) + CO2(g)
2. B) H2SO4(aq) + Ca(OH)2(aq) → CaSO4(aq) + 2 H2O(l)
3. C) 6 HCl(aq) + 2 Al(s) → 2 AlCl3(aq) + 3 H2(g)
4. D) FeCl3(aq) + 3 KOH(aq) → Fe(OH)3(s) + 3 KCl(aq)
5. E) 2 Hg(l) + O2(g) → 2 HgO(s)

Answer:  D

Diff: 1

Section:  5.3

LO:  5.3

Global LO:  G2

24) The combination of ions most likely to produce a precipitate is

1. A) Li+and PO43-.
2. B) Pb2+and NO3-.
3. C) NH4+and SO42-.
4. D) Fe3+and OH-.
5. E) Mg2+and C2H3O2-.

Answer:  D

Diff: 2

Section:  5.3

LO:  5.3

Global LO:  G2

 

 

25) The combination of ions least likely to produce a precipitate is

1. A) Ba2+and SO42-.
2. B) Pb+and Cl-.
3. C) Ca2+and PO43-.
4. D) Fe3+and OH-.
5. E) Mg2+and C2H3O2-.

Answer:  E

Diff: 2

Section:  5.3

LO:  5.3

Global LO:  G2

 

26) Which of the following is not soluble in water?

1. A) potassium sulfide
2. B) iron(II) bromide
3. C) iron(III) hydroxide
4. D) iron(III) nitrate
5. E) ammonium sulfate

Answer:  C

Diff: 2

Section:  5.3

LO:  5.3

Global LO:  G2

 

27) When a solution of iron(III) nitrate is mixed with a solution of sodium hydroxide, a rust colored precipitate forms. This precipitate is probably

1. A) iron(III) nitrate.
2. B) sodium hydroxide.
3. C) sodium nitrate.
4. D) iron(III) hydroxide.
5. E) none of the above

Answer:  D

Diff: 3

Section:  5.3

LO:  5.3

Global LO:  G2

 

28) Which reaction is an example of both a precipitation and a neutralization?

1. A) H3PO4(aq) + 3 KOH(aq) → K3PO4(aq) + 3 H2O(l)
2. B) FeCl3(aq) + 3 KOH(aq) → Fe(OH)3(s) + 3 KCl(aq)
3. C) (NH4)2CO3(s) → 2 NH3(g) + CO2(g) + H2O(l)
4. D) H2SO4(aq) + Ba(OH)2(aq) → BaSO4(s) + 2 H2O(l)
5. E) 2 C(s) + O2(g) → 2 CO(g)

Answer:  D

Diff: 2

Section:  5.3, 5.4

LO:  5.3

Global LO:  G2

 

29) The following reaction can be classified as what type(s) of reaction(s)?

 

2 Al(OH)3(aq) + 3 H2SO4(aq) → Al2(SO4)3(s) + 6 H2O(l)

 

1. A) precipitation
2. B) acid-base neutralization
3. C) redox reaction
4. D) combustion
5. E) both A and B

Answer:  E

Diff: 2

Section:  5.3, 5.4

LO:  5.3, 5.4

Global LO:  G2

 

30) Write and balance the following acid-base neutralization reaction:

 

HBr(aq) + Li2CO3(aq) →

Answer:  2 HBr(aq) + Li2CO3(aq) → 2 LiBr(aq) + H2O(l) + CO2(g)

Diff: 1

Section:  5.3, 5.4

LO:  5.4

Global LO:  G7

 

 

31) The formation of which one of the compounds below will act as the driving force for an acid-base reaction?

1. A) H2O
2. B) MgCl2
3. C) NaNO3
4. D) KOH
5. E) all of these

Answer:  A

Diff: 2

Section:  5.4

LO:  5.4

Global LO:  G2

32) Which reaction is an example of an acid-base reaction?

1. A) H2CO3(aq) → H2O(l) + CO2(g)
2. B) H2SO4(aq) + Ca(OH)2(aq) → CaSO4(aq) + 2 H2O(l)
3. C) 6 HCl(aq) + 2 Al(s) → 2 AlCl3(aq) + 3 H2(g)
4. D) FeCl3(aq) + 3 KOH(aq) → Fe(OH)3(s) + 3 KCl(aq)
5. E) 2 Hg(l) + O2(g) →2 HgO(s)

Answer:  B

Diff: 2

Section:  5.4

LO:  5.4

Global LO:  G2

 

33) Which one of the following substances is produced during an acid/base (or neutralization) reaction?

1. A) H2
2. B) H2O
3. C) CO2
4. D) NaOH
5. E) NaCl

Answer:  B

Diff: 2

Section:  5.4

LO:  5.4

Global LO:  G2

 

34) Write and balance the following acid-base neutralization reaction:

 

KOH(aq) + H2SO4 aq) →

Answer:  2 KOH(aq) + H2SO4(aq) → K2SO4(aq) + 2 H2O(l)

Diff: 1

Section:  5.4

LO:  5.4

Global LO:  G7

 

35) When potassium hydroxide and hydrobromic acid are combined the products are

1. A) potassium bromide and water.
2. B) potasium bromate and water.
3. C) potassium bromide and hydrogen gas.
4. D) potassium hypobromite and water.
5. E) potassium bromite and hydrogen gas.

Answer:  A

Diff: 2

Section:  5.4

LO:  5.4

Global LO:  G7

36) In order to form the salt calcium sulfate, which acid and base combination should you choose?

1. A) H2SO3 and CaOH
2. B) H2SO4and CaOH
3. C) H2SO3and Ca(OH)2
4. D) H2SO4and Ca(OH)2
5. E) none of the above

Answer:  D

Diff: 2

Section:  5.4

LO:  5.4

Global LO:  G7

 

37) All of the statements regarding redox reactions are true except

1. A) a reducing agent causes another substance to be reduced.
2. B) halogens usually behave as oxidizing agents because they readily gain electrons.
3. C) metal ions are produced when pure metals are oxidized.
4. D) when a substance is oxidized its charge (or oxidation number) decreases.
5. E) alkali metals often behave as reducing agents because they readily lose electrons.

Answer:  D

Diff: 2

Section:  5.5

LO:  5.5

Global LO:  G2

 

38) In a typical oxidation-reduction reaction the electrons are transferred

1. A) from the oxidizing agent to the reducing agent.
2. B) from what is being oxidized to the substance being reduced.
3. C) from what is being reduced to the substance being oxidized.
4. D) from what is being oxidized to the reducing agent.
5. E) none of these.

Answer:  B

Diff: 2

Section:  5.5

LO:  5.5

Global LO:  G2

 

39) Which reaction is not an example of a redox reaction?

1. A) 2 Hg(l) + O2(g) → 2 HgO(s)
2. B) 2 (NH4)3PO4(aq) + 3 Ba(NO3)2(aq) → Ba3(PO4)2(s) + 6 NH4NO3(aq)
3. C) CH4(g) + 2 O2(g) → CO2(g) + 2 H2O(g)
4. D) 6 HCl(aq) + 2 Al(s) → 2 AlCl3(aq) + 3 H2(g)
5. E) 2 Al2O3(s) → 4 Al(s) + 3 O(g)

Answer:  B

Diff: 2

Section:  5.5

LO:  5.5

Global LO:  G2

40) All of the reactions shown are oxidation-reduction reactions except

1. A) N2(g) + O2(g) → 2 NO(g).
2. B) 2 Fe2O3(s) → 4 Fe(s) + 3 O2(g).
3. C) Zn(s) + 2 HCl(aq) → ZnCl2(aq) + H2(g).
4. D) 2 NaI(aq) + Cl2(g) → 2 NaCl(aq) + I2.
5. E) K2SO4(aq) + BaCl2(aq) → BaSO4(s) + 2 KCl(aq).

Answer:  E

Diff: 3

Section:  5.5

LO:  5.5

Global LO:  G2

 

41) The element chlorine is very reactive as a(an) ________ agent because it readily ________ electrons to form the chloride ion.

1. A) oxidizing; loses
2. B) oxidizing; gains
3. C) reducing; loses
4. D) reducing; gains
5. E) none of the above

Answer:  B

Diff: 3

Section:  5.5

LO:  5.5

Global LO:  G2

 

 

42) When a substance loses electrons it is ________; the substance itself is acting as a(an) ________ agent.

1. A) oxidized; oxidizing
2. B) oxidized; reducing
3. C) reduced; oxidizing
4. D) reduced; reducing
5. E) dissolved; neutralizing

Answer:  B

Diff: 3

Section:  5.5

LO:  5.5

Global LO:  G2

 

43) In the reaction shown, ________ is the oxidizing agent because it ________.

 

Ni(s) + CuCl2(aq) → Cu(s) + NiCl2(aq)

 

1. A) Ni; causes reduction
2. B) Ni; gets reduced
3. C) CuCl2; causes reduction
4. D) CuCl2; gets reduced
5. E) NiCl2; gets reduced

Answer:  D

Diff: 3

Section:  5.5

LO:  5.5

Global LO:  G2

44) Reduction is the process of

1. A) gaining hydrogen.
2. B) losing oxygen.
3. C) gaining electrons.
4. D) forming an anion from a neutral atom.
5. E) all of the above

Answer:  E

Diff: 3

Section:  5.5

LO:  5.5

Global LO:  G2

 

 

45) In the redox reaction shown, ________ is oxidized and becomes ________.

 

Fe(s) + CuCl2 aq) → Cu(s) + FeCl2(aq)

 

1. A) Fe; Fe+
2. B) Fe; Fe2+
3. C) Cu; Cu2+
4. D) Cu2+; Cu
5. E) none of the above

Answer:  B

Diff: 2

Section:  5.5

LO:  5.5

Global LO:  G2

 

46) In the following reaction which species is being oxidized and which is being reduced?

 

2 Cr(s) + 3 Cl2(g) → 2 CrCl3(s)

 

1. A) oxidized: Cr; reduced: CrCl3
2. B) oxidized:CrCl3; reduced: Cr
3. C) oxidized: Cr; reduced: Cl2
4. D) oxidized: Cl2; reduced: Cr
5. E) oxidized: Cl2; reduced: CrCl3

Answer:  C

Diff: 3

Section:  5.5

LO:  5.5

Global LO:  G2

47) The oxidation number of iron in the compound FeBr3 is

2. A) -2.
3. B) -1.
4. C) +1.
5. D) +2.
6. E) +3.

Answer:  E

Diff: 1

Section:  5.6

LO:  5.6

Global LO:  G2

 

 

48) The oxidation number of sulfur in calcium sulfate, CaSO4, is

6. A) +6.
7. B) +4.
8. C) +2.
9. D) 0.
10. E) -2.

Answer:  A

Diff: 1

Section:  5.6

LO:  5.6

Global LO:  G2

 

49) The oxidation number of chlorine in the compound FeCl3 is

3. A) -3.
4. B) -2.
5. C) -1.
6. D) +2.
7. E) +3.

Answer:  C

Diff: 1

Section:  5.6

LO:  5.6

Global LO:  G2

 

50) As a pure element the oxidation number of zinc is ________, but in compounds such as ZnCO3 its oxidation number is ________.

1. A) 0; 0
2. B) 0; +1
3. C) +1; 0
4. D) 0; +2
5. E) none of the above

Answer:  D

Diff: 2

Section:  5.6

LO:  5.6

Global LO:  G2

51) In which of the following is the oxidation number for oxygen equal to zero?

1. A) Ca(OH)2
2. B) HNO3
3. C) O2
4. D) H2O2
5. E) all of the above

Answer:  C

Diff: 2

Section:  5.6

LO:  5.6

Global LO:  G2

 

52) What is the oxidation number of oxygen in hydrogen peroxide, H2O2?

1. A) 0
2. B) -1
3. C) -2
4. D) +1
5. E) +2

Answer:  B

Diff: 1

Section:  5.6

LO:  5.6

Global LO:  G2

 

53) 2 AgN(aq) + S(aq) → 2 KN(aq) + AS(s)

The net ionic reaction for the balanced equation shown above is

1. A) Ag+(aq) + NO3-(aq) → AgNO3(s)
2. B) 2 K+(aq) + SO42-(aq) → K2SO4(aq)
3. C) K+(aq) + NO3-(aq) → KNO3(aq)
4. D) 2 Ag+(aq) + SO42-(aq) → Ag2SO4(s)
5. E) H+(aq) + OH-(aq) → H2O(l)

Answer:  D

Diff: 3

Section:  5.7

LO:  5.7

Global LO:  G2

 

54) The net ionic equation for the reaction between zinc and hydrochloric acid solution is

1. A) Zn(s) + 2 H+(aq) → Zn2+(aq) + H2(g).
2. B) Zn(s) + 2 HCl(aq) → ZnCl2(aq) + H2(g).
3. C) Zn2+(aq) + H2(g) → ZnS(s) + 2 H+(aq).
4. D) ZnCl2(aq) + H2(g) → ZnS(s) + 2 HCl(aq).
5. E) none of these

Answer:  A

Diff: 3

Section:  5.7

LO:  5.7

Global LO:  G2

 

55) 2 AgNO3(aq) + K2SO4(aq) → 2 KNO3(aq) + Ag2SO4(s)

 

The spectator ions in the reaction shown are

1. A) silver ion and nitrate ion.
2. B) potassium ion and sulfate ion.
3. C) potassium ion and nitrate ion.
4. D) silver ion and sulfate ion.
5. E) hydrogen ion and hydroxide ion.

Answer:  C

Diff: 3

Section:  5.7

LO:  5.7

Global LO:  G2

 

56) What are the spectator ions in the reaction between KOH and HNO3?

1. A) K+and H+
2. B) H+and OH-
3. C) K+and NO3-
4. D) H+and NO3-
5. E) none of these

Answer:  C

Diff: 3

Section:  5.7

LO:  5.7

Global LO:  G2

 

57) Which of the following is always a spectator ion in aqueous chemical reactions?

1. A) Na+
2. B) Cl-
3. C) S2-
4. D) Mg2+
5. E) all of these ions.

Answer:  A

Diff: 3

Section:  5.7

LO:  5.7

Global LO:  G2

 

 

58) What is the typical net ionic equation for an acid-base neutralization of KOH and HCl?

1. A) HCl(aq) + KOH(aq) → H2O(l) + KCl(aq)
2. B) KOH(aq) → K+(aq) + OH-(aq)
3. C) H2O(l) → H+(aq) + OH-(aq)
4. D) K+(aq) + OH-(aq) → KOH(aq)
5. E) H+(aq) + OH-(aq) → H2O(l)

Answer:  E

Diff: 2

Section:  5.7

LO:  5.7

Global LO:  G7

Match the following.

 

1. A) redox
2. B) acid-base
3. C) precipitation

 

59) M(s) + 2 LX(aq)

→ 2 L(s) + M(aq)

Diff: 1

Section: 5.7

LO:  5.7

Global LO:  G2

 

60) LX(aq) + MY(aq)

→ LY(s) + MX(aq)

Diff: 1

Section:  5.7

LO:  5.7

Global LO:  G2

 

61) HR(aq) + XOH(aq)

→ XR(aq) + O(l)

Diff: 2

Section:  5.7

LO:  5.7

Global LO:  G2

 

Answers: 59) A 60) C 61) B