   Chapter 21, Problem 131SCQ

Chapter
Section
Textbook Problem

Xenon trioxide, XeO3, reacts with aqueous base to form the xenate anion, HXeO4−. This ion reacts further with OH− to form the perxenate anion, XeO64−, in the following reaction: 2 HXeO 4 − (aq) + 2 OH − (aq)  →  XeO 6 4 − (aq) + Xe(g) + O 2 (g) + 2 H 2 O( l ) Identify the elements that are oxidized and reduced in this reaction. You will note that the equation is balanced with respect to the number of atoms on either side. Verify that the redox part of this equation is also balanced, that is, that the extents of oxidation and reduction are also equal.

Interpretation Introduction

Interpretation: To identify the elements that are oxidized and reduced in the given reaction

Concept introduction:

Redox reaction are the type of reaction in which one substance is being oxidized and another one is being reduced. The species which acts as an oxidising agent in the reaction itself gets reduced and vice-versa.

An example of redox-type reaction is the reaction of Xenon trioxide and a base to form xenate anion and further perxenate ion.

Explanation

The given reaction is,

2HXeO4(aq)+2OH(aq)XeO64(aq)+Xe(g)+O2(g)+2H2O(l)

The oxidation number of xenon in HXeO4 is +6. The oxidation number of xenon in XeO64 is +8 and in Xe is zero

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