Deck 4: Reactions in Aqueous Solution

Question 1

Based on the solubility rules, which one of the following compounds should be insoluble in water?

A)NaCl
B)MgBr₂
C)FeCl₂
D)AgBr
E)ZnCl₂

Answer 1

AgBr

Question 2

Based on the solubility rules, which one of the following should be soluble in water?

A)CaSO₄
B)BaSO₄
C)PbSO₄
D)K₂SO₄
E)AgCl

Answer 2

K₂SO₄

Question 3

Which of the following compounds is a weak electrolyte?

A)HCl
B)CH₃COOH (acetic acid)
C)C₆H₁₂O₆ (glucose)
D)O₂
E)NaCl

Answer 3

CH₃COOH (acetic acid)

Question 4

Based on the solubility rules, which one of the following should be soluble in water?

A)AgBr
B)AgCl
C)Ag₂CO₃
D)AgNO₃
E)Ag₂S

Question 5

Which of the following compounds is a weak electrolyte?

A)HCl
B)NH₃
C)C₆H₁₂O₆ (glucose)
D)N₂
E)KCl

Question 6

Based on the solubility rules, which of the following will occur when a solution containing about 0.1 g of Pb(NO₃)₂(aq)is mixed with a solution containing 0.1 g of KI(aq)/100 mL?

A)KNO₃ will precipitate; Pb²⁺ and I^- are spectator ions.
B)No precipitate will form.
C)Pb(NO₃)₂ will precipitate; K⁺ and I^- are spectator ions.
D)PbI₂ will precipitate; K⁺ and NO₃^- are spectator ions.
E)Pb²⁺ and I^- are spectator ions, and PbI₂ will precipitate.

Question 7

Identify the major ionic species present in an aqueous solution of K₂SO₄.

A)K²⁺, S⁶⁺, O₄^8-
B)K²⁺, S⁶⁺, 4O^2-
C)2K⁺, S⁶⁺, O₄^8-
D)2K⁺, S⁶⁺, 4O^2-
E)2K⁺, SO₄^2-

Question 8

Which of the following compounds is a nonelectrolyte?

A)NaF
B)HNO₃
C)CH₃COOH (acetic acid)
D)NaOH
E)C₆H₁₂O₆ (glucose)

Question 9

Which of the following compounds is a strong electrolyte?

A)H₂O
B)N₂
C)CH₃COOH (acetic acid)
D)CH₃CH₂OH (ethanol)
E)KOH

Question 10

Based on the solubility rules, which one of the following should be soluble in water?

A)Hg₂Cl₂
B)Na₂S
C)Ag₂CO₃
D)Ag₂S
E)BaSO₄

Question 11

Based on the solubility rules, which of the following will occur if solutions of CuSO₄(aq)and BaCl₂(aq)are mixed?

A)CuCl₂ will precipitate; Ba²⁺ and SO₄^2- are spectator ions.
B)CuSO₄ will precipitate; Ba²⁺ and Cl^- are spectator ions.
C)BaSO₄ will precipitate; Cu²⁺ and Cl^- are spectator ions.
D)BaCl₂ will precipitate; Cu²⁺ and SO₄^2- are spectator ions.
E)No precipitate will form.

Question 12

Based on the solubility rules, which one of the following should be soluble in water?

A)(NH₄)₃PO₄
B)Ca₃(PO₄)₂
C)AlPO₄
D)Ag₃PO₄
E)Mg₃(PO₄)₂

Question 13

Based on the solubility rules, which of the following will occur when solutions of ZnSO₄(aq)and MgCl₂(aq)are mixed?

A)ZnCl₂ will precipitate; Mg²⁺ and SO₄^2- will be spectator ions.
B)ZnSO₄ will precipitate; Mg²⁺ and Cl^- will be spectator ions.
C)MgSO₄ will precipitate; Zn²⁺ and Cl^- will be spectator ions.
D)MgCl₂ will precipitate; Zn²⁺ and SO₄^2- will be spectator ions.
E)No precipitate will form.

Question 14

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.

Question 15

Identify the major ionic species present in an aqueous solution of Na₂CO₃.

A)Na₂⁺, CO₃^2-
B)Na₂⁺, C^{2 -}, O₃
C)Na⁺, C⁴⁺, O₃^2-
D)Na⁺, C⁺, O^2-
E)Na⁺, CO₃^2-

Question 16

Which of the following compounds is a nonelectrolyte?

A)NaOH
B)HNO₃
C)C₂H₆O (ethanol)
D)KF
E)CH₃COOH (acetic acid)

Question 17

Which of the following compounds is a weak electrolyte?

A)HNO₃
B)NaNO₃
C)HNO₂
D)NaNO₂
E)NaOH

Question 18

Based on the solubility rules, which one of the following compounds should be insoluble in water?

A)Na₂SO₄
B)BaSO₄
C)CuSO₄
D)MgSO₄
E)Rb₂SO₄

Question 19

Which of the following compounds is a strong electrolyte?

A)H₂O
B)CH₃OH
C)CH₃CH₂OH
D)HF
E)NaF

Question 20

Based on the solubility rules, which one of the following compounds should be insoluble in water?

A)CaCO₃
B)(NH₄)₂CO₃
C)Na₂CO₃
D)K₂CO₃
E)KNO₃

Question 21

Identify the major ions present in an aqueous LiOH solution.

A)Li²⁺, O^-, H^-
B)Li⁺, OH^-
C)LiO^-, H⁺
D)Li⁺, O^2-, H⁺
E)Li^-, OH⁺

Question 22

What is the chemical formula of the salt produced by the complete neutralization of sodium hydroxide with sulfuric acid?

A)Na₂SO₄
B)Na₂(SO₄)₃
C)Na(SO₄)₂
D)NaSO₃
E)Na₃SO₄

Question 23

The highest possible oxidation number of nitrogen is

A)+8
B)+5
C)+3
D)+1
E)-3

Question 24

Identify the major ions present in an aqueous HNO₃ solution.

A)HN⁺, O^2-
B)OH^-, NO₃^-
C)OH^-, NO
D)H⁺, N^3-, O^2-
E)H⁺, NO₃^-

Question 25

The oxidation number of Cl in ClO₃^- is

A)-1
B)+7
C)+5
D)+3
E)None of the above.

Question 26

The oxidation number of Mn in KMnO₄ is

A)+8
B)+7
C)+5
D)-7
E)-8

Question 27

The oxidation number of Cl in ClO₄^- is

A)-1
B)+1
C)+3
D)+5
E)None of the above.

Question 28

The oxidation number of Fe in K₃Fe(CN)₆ is

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

Question 29

What is the chemical formula of the salt produced by the neutralization of nitric acid with calcium hydroxide?

A)CaNO₃
B)Ca₂(NO₃)₃
C)Ca₃(NO₃)₂
D)Ca₂NO₃
E)Ca(NO₃)₂

Question 30

Identify the major ionic species present in an aqueous solution of H₂SO₄.

A)S⁶⁺, O₃^6- (plus H₂O as a neutral species)
B)H⁺, OH^-, S⁶⁺, 3O^2-
C)2H⁺, S⁶⁺, 4O^2-
D)H⁺, HSO₄^-
E)2H⁺, SO₄^2-

Question 31

What is the chemical formula of the salt produced by the neutralization of hydrobromic acid with magnesium hydroxide?

A)MgBr
B)Mg₂Br₃
C)Mg₃Br₂
D)Mg₂Br
E)MgBr₂

Question 32

The oxidation number of S in K₂SO₄ is

A)+6
B)+4
C)+2
D)-1
E)None of the above.

Question 33

Which of the following is the correct net ionic equation for the reaction that occurs when solutions of Pb(NO₃)₂ and NH₄Cl are mixed?

A)Pb(NO₃)₂(aq)+ 2NH₄Cl(aq) $\rarr$ NH₄NO₃(aq)+ PbCl₂(s)
B)Pb²⁺(aq)+ 2Cl^-(aq) $\rarr$ PbCl₂(s)
C)Pb²⁺(aq)+ 2NO₃^- (aq)+ 2NH (aq)+ 2Cl^-(aq) $\rarr$ 2NH (aq)+ 2NO₃^- (aq)+ PbCl₂(s)
D)NH₄⁺(aq)+ NO₃^- (aq) $\rarr$ 2NH₄NO₃(s)
E)No reaction occurs when the solutions are mixed.

Question 34

The oxidation number of Cr in Cr₂O₇^2- is

A)-12
B)-7
C)-2
D)+6
E)+7

Question 35

The oxidation number of N in NaNO₃ is

A)+6
B)+5
C)+3
D)-3
E)None of the above.

Question 36

For which one of the following acids is chlorine in the +5 oxidation state?

A)HCl
B)HClO
C)HClO₂
D)HClO₃
E)HClO₄

Question 37

What is the correct formula of the salt formed in the neutralization reaction of hydrochloric acid with calcium hydroxide?

A)CaO
B)CaCl₂
C)CaH₂
D)CaCl
E)CaClH

Question 38

Which of the following compounds is a weak acid?

A)HF
B)HCl
C)HBr
D)HI
E)HClO₄

Question 39

What is the chemical formula of the salt produced by the neutralization of potassium hydroxide with sulfuric acid?

A)KSO₃
B)K₂(SO₄)₃
C)K₂SO₄
D)K(SO₄)₂
E)KSO₄

Question 40

The common constituent in all acid solutions is

A)H₂
B)H⁺
C)OH^-
D)H₂SO₄
E)Cl^-

Question 41

Which choice gives the correct oxidation numbers for all three elements in Ca(ClO)₂ in the order that the elements are shown in the formula?

A)+2, +1, -2
B)+2, -2, +1
C)+2, -3, +2
D)-2, +2, -1
E)-2, +3, -2

Question 42

In the following chemical reaction the oxidizing agent is
5H₂O₂ + 2MnO₄^- + 6H⁺ $\rarr$ 2Mn²⁺ + 8H₂O + 5O₂

A)H₂O₂
B)MnO₄^-
C)H⁺
D)Mn²⁺
E)O₂

Question 43

Identify the oxidizing agent in the following chemical reaction. 2MnO₄^- + 5H₂SO₃ $\rarr$ 2Mn²⁺ + 5SO₄^2- + 4H⁺ + 3H₂O

A)MnO₄^-
B)H₂SO₃
C)Mn²⁺
D)SO₄^2-
E)H⁺

Question 44

The oxidation number of N in N₂H₄ is

A)+4
B)-4
C)+2
D)-2
E)0

Question 45

Identify the elements that are oxidized and reduced in the following reaction. KClO₃(aq)+ 6HBr(aq) $\rarr$ KCl(aq)+ 3Br₂(l)+ 3H₂O(l)

A)Br is oxidized and Cl is reduced
B)Cl is oxidized and H is reduced
C)H is oxidized and O is reduced
D)O is oxidized and Cl is reduced
E)Cl is oxidized and Br is reduced

Question 46

Which one of the following is a redox reaction?

A)2Al(s)+ 3H₂SO₄(aq) $\rarr$ Al₂(SO₄)₃(aq)+ 3H₂(g)
B)2KBr(aq)+ Pb(NO₃)₂(aq) $\rarr$ 2KNO₃(aq)+ PbBr₂(s)
C)CaBr₂(aq)+ H₂SO₄(aq) $\rarr$ CaSO₄(s)+ 2HBr(g)
D)H⁺(aq)+ OH^- (aq) $\rarr$ H₂O(l)
E)CO₃^2- (aq)+ HSO₄^-(aq) $\rarr$ HCO₃^- (aq)+ SO₄^2- (aq)

Question 47

What element is oxidized in the following chemical reaction? NiO₂ + Cd + 2H₂O $\rarr$ Ni(OH)₂ + Cd(OH)₂

A)Ni
B)Cd
C)O
D)H
E)This is not a redox reaction.

Question 48

In the following redox reaction 4NH₃ + 3Ca(ClO)₂ $\rarr$ 2N₂ + 6H₂O + 3CaCl₂
which element is oxidized and which is reduced?

A)H is oxidized and N is reduced
B)N is oxidized and Cl is reduced
C)N is oxidized and O is reduced
D)Cl is oxidized and O is reduced
E)Cl is oxidized and N is reduced

Question 49

In the following chemical reaction the oxidizing agent is 5S + 6KNO₃ + 2CaCO₃ $\rarr$ 3K₂SO₄ + 2CaSO₄ + CO₂ + 3N₂

A)S
B)N₂
C)KNO₃
D)CaSO₄
E)CaCO₃

Question 50

What element is oxidized in the following chemical reaction? 3Cu + 8HNO₃ $\rarr$ 3Cu(NO₃)₂ + 2NO + 4H₂O

A)Cu
B)H
C)N
D)O
E)H₂O

Question 51

Which choice gives the correct oxidation numbers for all three elements in Rb₂SO₃ in the order that the elements are shown in the formula?

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

Question 52

Predict the products of the following single replacement reaction. Fe(s)+ CuSO₄(aq) $\rarr$

A)Cu(s)+ FeSO₄(aq)
B)Fe(s)+ Cu(s)+ SO₄(aq)
C)CuS(s)+ Fe₂SO₄(aq)
D)FeCuSO₄(aq)
E)FeO(s)+ CuSO₃(aq)

Question 53

Identify the reducing agent in the following chemical reaction. Cd + NiO₂ + 2H₂O $\rarr$ Cd(OH)₂ + Ni(OH)₂

A)Cd
B)NiO₂
C)H₂O
D)Cd(OH)₂
E)Ni(OH)₂

Question 54

Identify the reducing agent in the following chemical reaction. 5Fe²⁺(aq)+ MnO₄^-(aq) + 8H⁺(aq) $\rarr$ 5Fe³⁺(aq)+ Mn²⁺(aq)+ 4H₂O(l)

A)Fe²⁺
B)MnO₄^-
C)H⁺
D)Mn²⁺
E)Fe³⁺

Question 55

Select the compound in which sulfur has its highest possible oxidation number.

A)H₂S
B)SO₂
C)SCl₂
D)H₂SO₃
E)Na₂SO₄

Question 56

Which of the following equations does not represent an oxidation-reduction reaction?

A)3Al + 6HCl $\rarr$ 3H₂ + AlCl₃
B)2H₂O $\rarr$ 2H₂ + O₂
C)2NaCl + Pb(NO₃)₂ $\rarr$ PbCl₂ + 3NaNO₃
D)2NaI + Br₂ $\rarr$ 2NaBr + I₂
E)Cu(NO₃)₂ + Zn $\rarr$ Zn(NO₃)₂ + Cu

Question 57

What element is reduced in the following chemical reaction? Cu + 2H₂SO₄ $\rarr$ CuSO₄ + SO₂ + 2H₂O

A)Cu
B)H
C)S
D)O
E)H₂O

Question 58

The highest possible oxidation number of carbon is

A)+8
B)+6
C)+4
D)+2
E)-4

Question 59

What element is oxidized in the following chemical reaction? H₂SO₄ + Cd(OH)₂ $\rarr$ 2H₂O + CdSO₄

A)H
B)S
C)O
D)Cd
E)this is not a redox reaction

Question 60

Which of the following is an example of a disproportionation reaction?

A)2C₂H₆(g)+ 7O₂(g) $\rarr$ 4CO₂(g)+ 6H₂O(l)
B)2KBr(aq)+ Cl₂(g) $\rarr$ 2KCl(aq)+ Br₂(l)
C)2H₂O₂(aq) $\rarr$ 2H₂O(l)+ O₂(g)
D)CaBr₂(aq)+ H₂SO₄(aq) $\rarr$ CaSO₄(s)+ 2HBr(g)
E)2Al(s)+ 3H₂SO₄(aq) $\rarr$ Al₂(SO₄)₃(aq)+ 3H₂(g)

Question 61

What mass of Na₂SO₄ is needed to prepare 350.mL of a solution having a sodium ion concentration of 0.125 M?

A)3.11 g
B)24.9 g
C)12.4 g
D)6.21 g
E)8.88 g

Question 62

Which of the following represents a metal displacement reaction?

A)2NaN₃(s) $\rarr$ 2Na(s)+ 3N₂(g)
B)Fe₂O₃(s)+ 2Al(s) $\rarr$ 2Fe(s)+ Al₂O₃(s)
C)3NO₂(g)+ H₂O(l) $\rarr$ 2HNO₃(aq)+ NO(g)
D)2P(s)+ 3Cl₂(g) $\rarr$ 2PCl₃(g)
E)2ZnS(s)+ 3O₂(g) $\rarr$ 2ZnO(s)+ 2SO₂(g)

Question 63

Zinc dissolves in hydrochloric acid to yield hydrogen gas: Zn(s)+ 2HCl(aq) $\rarr$ ZnCl₂(aq)+ H₂(g)
What mass of hydrogen gas is produced when a 7.35 g chunk of zinc dissolves in 500. mL of 1.200M HCl?

A)0.605 g
B)0.113 g
C)0.302 g
D)0.453 g
E)0.227 g

Question 64

Which of the following represents a combustion reaction?

A)2C₂H₆(g)+ 7O₂(g) $\rarr$ 4CO₂(g)+ 6H₂O(l)
B)LiOH(aq)+ HNO₃(aq) $\rarr$ LiNO₃(aq)+ H₂O(l)
C)N₂(g)+ 3H₂(g) $\rarr$ 2NH₃(g)
D)2Na(s)+ 2H₂O(l) $\rarr$ 2NaOH(aq)+ H₂(g)
E)2Al(s)+ 3H₂SO₄(aq) $\rarr$ Al₂(SO₄)₃(aq)+ 3H₂(g)

Question 65

A 3.682 g sample of KClO₃ is dissolved in enough water to give 375.mL of solution.What is the chlorate ion concentration in this solution?

A)3.00 * 10^-2 M
B)4.41 * 10^-2 M
C)0.118 M
D)1.65 * 10^-2 M
E)8.01 * 10^-2 M

Question 66

When 38.0 mL of 0.1250 M H₂SO₄ is added to 100.mL of a solution of PbI₂, a precipitate of PbSO₄ forms. The PbSO₄ is then filtered from the solution, dried, and weighed. If the recovered PbSO₄ is found to have a mass of 0.0471 g, what was the concentration of iodide ions in the original solution?

A)3.10 * 10^-4 M
B)1.55 * 10^-4 M
C)6.20 * 10^-3 M
D)3.11 * 10^-3 M
E)1.55 * 10^-3 M

Question 67

What mass of K₂CO₃ is needed to prepare 200.mL of a solution having a potassium ion concentration of 0.150 M?

A)4.15 g
B)10.4 g
C)13.8 g
D)2.07 g
E)1.49 g

Question 68

What mass of Li₃PO₄ is needed to prepare 500.mL of a solution having a lithium ion concentration of 0.175 M?

A)6.75 g
B)10.1 g
C)19.3 g
D)30.4 g
E)3.38 g

Question 69

A 50.0 mL sample of 0.436 M NH₄NO₃ is diluted with water to a total volume of 250.0 mL. What is the ammonium nitrate concentration in the resulting solution?

A)21.8 M
B)0.459 M
C)2.18 * 10^-2 M
D)8.72* 10^-2 M
E)0.109 M

Question 70

Which of the following represents a precipitation reaction?

A)2H₂(g)+ O₂(g) $\rarr$ 2H₂O(l)
B)CaBr₂(aq)+ H₂SO₄(aq) $\rarr$ CaSO₄(s)+ 2HBr(g)
C)2KNO₃(s) $\rarr$ 2KNO₂(s)+ O₂(g)
D)2KBr(aq)+ Cl₂(g) $\rarr$ 2KCl(aq)+ Br₂(l)
E)2Al(s)+ 3H₂SO₄(aq) $\rarr$ Al₂(SO₄)₃(aq)+ 3H₂(g)

Question 71

A 0.9182 g sample of CaBr₂ is dissolved in enough water to give 500.mL of solution.What is the calcium ion concentration in this solution?

A)9.19 * 10^-3 M
B)2.30 * 10^-3 M
C)2.72 * 10^-3 M
D)4.59 * 10^-3 M
E)1.25 * 10^-3 M

Question 72

When 50.0 mL of a 0.3000 M AgNO₃ solution is added to 50.0 mL of a solution of MgCl₂, an AgCl precipitate forms immediately. The precipitate is then filtered from the solution, dried, and weighed. If the recovered AgCl is found to have a mass of 0.1183 g, what as the concentration of magnesium ions in the original MgCl₂ solution?

A)0.300 M
B)8.25 * 10^-3 M
C)1.65 * 10^-2 M
D)2.06 * 10^-5 M
E)4.13 * 10^-3 M

Question 73

When 20.0 mL of a 0.250 M (NH₄)₂S solution is added to 150.0 mL of a solution of Cu(NO₃)₂, a CuS precipitate forms. The precipitate is then filtered from the solution, dried, and weighed. If the recovered CuS is found to have a mass of 0.3491 g, what was the concentration of copper ions in the original Cu(NO₃)₂ solution?

A)3.65 * 10^-3 M
B)1.22 * 10^-2 M
C)3.33 * 10^-2 M
D)4.87 * 10^-2 M
E)2.43* 10^-2 M

Question 74

Which of the following represents a hydrogen displacement reaction?

A)2C₂H₆(g)+ 7O₂(g) $\rarr$ 4CO₂(g)+ 6H₂O(l)
B)2KBr(aq)+ Cl₂(g) $\rarr$ 2KCl(aq)+ Br₂(l)
C)N₂(g)+ 3H₂(g) $\rarr$ 2NH₃(g)
D)CaBr₂(aq)+ H₂SO₄(aq) $\rarr$ CaSO₄(s)+ 2HBr(g)
E)2Al(s)+ 3H₂SO₄(aq) $\rarr$ Al₂(SO₄)₃(aq)+ 3H₂(g)

Question 75

A 4.691 g sample of MgCl₂ is dissolved in enough water to give 750.mL of solution.What is the magnesium ion concentration in this solution?

A)3.70 * 10^-2 M
B)1.05 * 10^-2 M
C)6.57 * 10^-2 M
D)4.93 * 10^-2 M
E)0.131 M

Question 76

A 20.00 mL sample of 0.1015 M nitric acid is introduced into a flask, and water is added until the volume of the solution reaches 250.mL. What is the concentration of nitric acid in the final solution?

A)1.27 M
B)8.12 * 10^-3 M
C)0.406 M
D)3.25 * 10^-2 M
E)5.08 * 10^-4 M

Question 77

The concentration of oxalate ion (C₂O₄^2-)in a sample can be determined by titration with a solution of permanganate ion (MnO₄^-)of known concentration. The net ionic equation for this reaction is 2MnO₄^- + 5C₂O₄^2- + 16H⁺ $\rarr$ 2Mn²⁺ + 8H₂O + 10CO₂
A 30.00 mL sample of an oxalate solution is found to react completely with 21.93 mL of a 0.1725 M solution of MnO₄^-. What is the oxalate ion concentration in the sample?

A)0.02914 M
B)0.4312 M
C)0.1821 M
D)0.3152 M
E)0.05044 M

Question 78

One method of determining the concentration of hydrogen peroxide (H₂O₂)in a solution is through titration with iodide ion. The net ionic equation for this reaction is H₂O₂ + 2I^- +2H⁺ $\rarr$ I₂ + 2H₂O
A 50.00 mL sample of a hydrogen peroxide solution is found to react completely with 37.12 mL of a 0.1500 M KI solution. What is the concentration of hydrogen peroxide in the sample?

A)5.568 * 10^-2 M
B)0.2227 M
C)0.1010 M
D)0.4041 M
E)0.1114 M

Question 79

Which of the following represents an acid-base neutralization reaction?

A)2Al(s)+ 3H₂SO₄(aq) $\rarr$ Al₂(SO₄)₃(aq)+ 3H₂(g)
B)SO₂(g)+ H₂O(l) $\rarr$ H₂SO₃(g)
C)LiOH(aq)+ HNO₃(aq) $\rarr$ LiNO₃(aq)+ H₂O(l)
D)2KBr(aq)+ Cl₂(g) $\rarr$ 2KCl(aq)+ Br₂(l)
E)CaBr₂(aq)+ H₂SO₄(aq) $\rarr$ CaSO₄(s)+ 2HBr(g)

Question 80

Which of the following represents a halogen displacement reaction?

A)2KBr(aq)+ Cl₂(g) $\rarr$ 2KCl(aq)+ Br₂(l)
B)2Na(s)+ 2H₂O(l) $\rarr$ 2NaOH(aq)+ H₂(g)
C)CaBr₂(aq)+ H₂SO₄(aq) $\rarr$ CaSO₄(s)+ 2HBr(g)
D)2KNO₃(s) $\rarr$ 2KNO₂(s)+ O₂(g)
E)2LiOH(aq)+ H₂SO₄(aq) $\rarr$ Li₂SO₄(aq)+ 2H₂O(l)