The product for the given reaction has to be shown and the major product has to be indicated. Concept introduction: Autoxidation involves reaction of a C − H bond, (usually allylic one) with oxygen under radical initiation condition. The product is a hydroperoxide. Mechanism involves a radical chain process in which resonance-delocalized allylic radical intermediates reacts with molecular oxygen to give peroxy radical that continues the radical chain. Major product is more substituted double bond.

Question

A solution contains 0.097 M Ce3+, 1.55x10-3 M Ce4+, 1.55x10-3 M Mn2+, 0.097 M MnO4-, and 1.00 M HClO4 (F= 9.649 x 104 C/mol). a) Write a balanced net reaction that can occur between species in this solution. b) Calculate deltaG0 and K for the reaction. c) Calculate E and deltaG for the conditions given. Ce4+ + e- = Ce3+ E0= 1.70 V MnO4- + 8H+ + 5e- = Mn2+ + 4H2O E0= 1.507 V

Answer 1

Question

Chapter 8, Problem 8.31P

(a)

Interpretation Introduction

Interpretation:

The product for the given reaction has to be shown and the major product has to be indicated.

Concept introduction:

Autoxidation involves reaction of a C−H bond, (usually allylic one) with oxygen under radical initiation condition. The product is a hydroperoxide.

Mechanism involves a radical chain process in which resonance-delocalized allylic radical intermediates reacts with molecular oxygen to give peroxy radical that continues the radical chain.

Major product is more substituted double bond.

(b)

Interpretation Introduction

Interpretation:

The product for the given reaction has to be shown and the major product has to be indicated.

Concept introduction:

Autoxidation involves reaction of a C−H bond, (usually allylic one) with oxygen under radical initiation condition. The product is a hydroperoxide.

Mechanism involves a radical chain process in which resonance-delocalized allylic radical intermediates reacts with molecular oxygen to give peroxy radical that continues the radical chain.

Major product is more substituted double bond.

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A solution contains 0.097 M Ce3+, 1.55x10-3 M Ce4+, 1.55x10-3 M Mn2+, 0.097 M MnO4-, and 1.00 M HClO4 (F= 9.649 x 104 C/mol). a) Write a balanced net reaction that can occur between species in this solution. b) Calculate deltaG0 and K for the reaction. c) Calculate E and deltaG for the conditions given. Ce4+ + e- = Ce3+ E0= 1.70 V MnO4- + 8H+ + 5e- = Mn2+ + 4H2O E0= 1.507 V

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