the balanced redox reactions a. I 2 (s)+ Fe(s) → FeI 2 (s) b. Cl 2 (s)+ H 2 O 2 (aq) → Cl − (aq) + O 2 (g) (acidic) c. Hg 2 + (aq)+ H 2 (g) → Hg(l) + H 2 O(l) (basic) d. CH 3 OH(l)+ O 2 (g) → CO 2 (g) + H 2 O(l) (acidic)

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Answer 1

Question

Chapter 19, Problem 138E

Interpretation Introduction

To determine: the balanced redox reactions

a. $I_{2} (s)+ Fe(s) \to {FeI}_{2} (s)$

b. ${Cl}_{2} {(s)+ H}_{2} O_{2} (aq) \to {Cl}^{-} {(aq) + O}_{2} (g)  (acidic)$

c. ${Hg}^{2 +} {(aq)+ H}_{2} (g) \to {Hg(l) + H}_{2} O(l)  (basic)$

d. ${CH}_{3} {OH(l)+ O}_{2} (g) \to {CO}_{2} {(g) + H}_{2} O(l)  (acidic)$

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Answer 2

Question

Chapter 19, Problem 138E

Interpretation Introduction

To determine: the balanced redox reactions

a. $I_{2} (s)+ Fe(s) \to {FeI}_{2} (s)$

b. ${Cl}_{2} {(s)+ H}_{2} O_{2} (aq) \to {Cl}^{-} {(aq) + O}_{2} (g)  (acidic)$

c. ${Hg}^{2 +} {(aq)+ H}_{2} (g) \to {Hg(l) + H}_{2} O(l)  (basic)$

d. ${CH}_{3} {OH(l)+ O}_{2} (g) \to {CO}_{2} {(g) + H}_{2} O(l)  (acidic)$

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Answer 3

Question

Chapter 19, Problem 138E

Interpretation Introduction

To determine: the balanced redox reactions

a. $I_{2} (s)+ Fe(s) \to {FeI}_{2} (s)$

b. ${Cl}_{2} {(s)+ H}_{2} O_{2} (aq) \to {Cl}^{-} {(aq) + O}_{2} (g)  (acidic)$

c. ${Hg}^{2 +} {(aq)+ H}_{2} (g) \to {Hg(l) + H}_{2} O(l)  (basic)$

d. ${CH}_{3} {OH(l)+ O}_{2} (g) \to {CO}_{2} {(g) + H}_{2} O(l)  (acidic)$

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Answer 4

Question

Chapter 19, Problem 138E

Interpretation Introduction

To determine: the balanced redox reactions

a. $I_{2} (s)+ Fe(s) \to {FeI}_{2} (s)$

b. ${Cl}_{2} {(s)+ H}_{2} O_{2} (aq) \to {Cl}^{-} {(aq) + O}_{2} (g)  (acidic)$

c. ${Hg}^{2 +} {(aq)+ H}_{2} (g) \to {Hg(l) + H}_{2} O(l)  (basic)$

d. ${CH}_{3} {OH(l)+ O}_{2} (g) \to {CO}_{2} {(g) + H}_{2} O(l)  (acidic)$

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Answer 5

Chapter 19, Problem 138E

Interpretation Introduction

To determine: the balanced redox reactions

a. $I_{2} (s)+ Fe(s) \to {FeI}_{2} (s)$

b. ${Cl}_{2} {(s)+ H}_{2} O_{2} (aq) \to {Cl}^{-} {(aq) + O}_{2} (g)  (acidic)$

c. ${Hg}^{2 +} {(aq)+ H}_{2} (g) \to {Hg(l) + H}_{2} O(l)  (basic)$

d. ${CH}_{3} {OH(l)+ O}_{2} (g) \to {CO}_{2} {(g) + H}_{2} O(l)  (acidic)$

Answer 6

Chapter 19, Problem 138E

Interpretation Introduction

To determine: the balanced redox reactions

a. $I_{2} (s)+ Fe(s) \to {FeI}_{2} (s)$

b. ${Cl}_{2} {(s)+ H}_{2} O_{2} (aq) \to {Cl}^{-} {(aq) + O}_{2} (g)  (acidic)$

c. ${Hg}^{2 +} {(aq)+ H}_{2} (g) \to {Hg(l) + H}_{2} O(l)  (basic)$

d. ${CH}_{3} {OH(l)+ O}_{2} (g) \to {CO}_{2} {(g) + H}_{2} O(l)  (acidic)$

Answer 7

Chapter 19, Problem 138E

Interpretation Introduction

To determine: the balanced redox reactions

a. $I_{2} (s)+ Fe(s) \to {FeI}_{2} (s)$

b. ${Cl}_{2} {(s)+ H}_{2} O_{2} (aq) \to {Cl}^{-} {(aq) + O}_{2} (g)  (acidic)$

c. ${Hg}^{2 +} {(aq)+ H}_{2} (g) \to {Hg(l) + H}_{2} O(l)  (basic)$

d. ${CH}_{3} {OH(l)+ O}_{2} (g) \to {CO}_{2} {(g) + H}_{2} O(l)  (acidic)$

Answer 8

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Answer 9

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Answer 10

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Answer 11

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the balanced redox reactions a. I 2 (s)+ Fe(s) → FeI 2 (s) b. Cl 2 (s)+ H 2 O 2 (aq) → Cl − (aq) + O 2 (g) (acidic) c. Hg 2 + (aq)+ H 2 (g) → Hg(l) + H 2 O(l) (basic) d. CH 3 OH(l)+ O 2 (g) → CO 2 (g) + H 2 O(l) (acidic)

Solution Summary: The author explains the balanced redox reactions by adding both 1 and 2 to get the overall reaction.

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Chapter 19 Solutions

the balanced redox reactions a. I 2 (s)+ Fe(s) → FeI 2 (s) b. Cl 2 (s)+ H 2 O 2 (aq) → Cl − (aq) + O 2 (g) (acidic) c. Hg 2 + (aq)+ H 2 (g) → Hg(l) + H 2 O(l) (basic) d. CH 3 OH(l)+ O 2 (g) → CO 2 (g) + H 2 O(l) (acidic)

Solution Summary: The author explains the balanced redox reactions by adding both 1 and 2 to get the overall reaction.

To determine: the balanced redox reactions a. I2(s)+ Fe(s) → FeI2(s) b. Cl2(s)+ H2O2(aq) → Cl−(aq) + O2(g) (acidic) c.Hg2+(aq)+ H2(g) → Hg(l) + H2O(l) (basic) d. CH3OH(l)+ O2(g) → CO2(g) + H2O(l) (acidic)

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Chapter 19 Solutions