Chapter 21, Problem 117IL

### Chemistry & Chemical Reactivity

10th Edition
John C. Kotz + 3 others
ISBN: 9781337399074

Chapter
Section

### Chemistry & Chemical Reactivity

10th Edition
John C. Kotz + 3 others
ISBN: 9781337399074
Textbook Problem

# A common analytical method for hydrazine involves its oxidation with iodate ion, IO3−, in acid solution. In the process, hydrazine acts as a four-electron reducing agent. N 2 (g) + 5 H 3 O + (aq) +   4   e − → N 2 H 5 + (aq) + 5 H 2 O ( l )   E ° = − 0.23  V Write the balanced equation for the reaction of hydrazine in acid solution (N2H5+) with IO3−(aq) to give N2 and I2. Calculate E° for this reaction.

Interpretation Introduction

Interpretation:

To write the balanced reaction of hydrazine in acid solution with iodate ion and also calculate the E for the reaction.

Concept introduction:

The formula for hydrazine is N2H4. In acidic solution it exists as N2H5+. It can be oxidized to N2 by the iodate ion. The formula for iodate ion is IO3. Hydrazine acts as a four electron reducing agent.

A balanced chemical equation occurs when the number of atoms in reactant side is equal to the number of atoms in the product side.

The standard cell potential expression is written as follows,

Ecell=Ecathode+Eanode

Explanation

The Eâˆ˜ for the reaction is calculated below.

Given:

The given reaction is,

Â Â Â Â N2H5+(aq)+IO3âˆ’(aq)â†’N2(g)+I2(g)

Hydrazine is oxidised to nitrogen. The hydrogen is balancedÂ  by the additon of H+ to the equation.

Â Â Â Â N2H5+(aq)â†’N2(g)+5H+

The charge has to be balanced by the addition of electrons.

Â Â Â Â N2H5+(aq)â†’N2(g)+5H++4eâˆ’

Iodate ion is reduced to iodine. The hydrogen is balancedÂ  by the additon of H+ Aand oxygen is balanced by the addition of H2O.

Â Â Â Â 2IO3âˆ’(aq)+12H+â†’I2(aq)+6H2O(l)

The charge has to be balanced by the addition of electrons.

â€‚Â 2IO3âˆ’(aq)+12H++10eâˆ’â†’I2(aq)+6H2O(l)

Thus,

The oxidation reaction is,

â€‚Â N2H5+(aq)â†’N2(g

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