Log out Go to App
Go to App

Learning Materials

Features

Discover

Chapter 22: Problem 10

Write a chemical equation for the hydrolysis in alkaline solution of \(\mathrm{XeF}_{6}\) that yields \(\mathrm{XeO}_{6}^{4-}, \mathrm{Xe}, \mathrm{O}_{2}, \mathrm{F}^{-}\) and \(\mathrm{H}_{2} \mathrm{O}\) as products.

Short Answer

Expert verified
The balanced chemical equation for the hydrolysis of \(\mathrm{XeF}_{6}\) that yields \(\mathrm{XeO}_{6}^{4-}, \mathrm{Xe}, \mathrm{O}_{2}, \mathrm{F}^{-}\), and \(\mathrm{H}_{2} \mathrm{O}\) as products is: \(\mathrm{XeF}_{6} + 6\mathrm{OH}^{-} → \mathrm{Xe} + \mathrm{XeO}_{6}^{4-} + \mathrm{O}_{2} + 4\mathrm{F}^{-} + 3\mathrm{H}_{2} \mathrm{O}\).

Step by step solution

01

Write the initial reaction

The first step in writing a chemical equation is outlining the reactants and the products. The reactant provided is \(\mathrm{XeF}_{6}\) and the reaction is in an alkaline solution, meaning there is also \(\mathrm{OH}^{-}\) present. This results in the following products: \(\mathrm{Xe}, \mathrm{XeO}_{6}^{4-}, \mathrm{O}_{2}, \mathrm{F}^{-}, \mathrm{H}_{2} \mathrm{O}\). Thus, the initial reaction can be written as: \(\mathrm{XeF}_{6} + n\mathrm{OH}^{-} → \mathrm{Xe} + \mathrm{XeO}_{6}^{4-} + \mathrm{O}_{2} + \mathrm{F}^{-} + \mathrm{H}_{2} \mathrm{O}\)
02

Balance the equation

The second step is to balance the equation by ensuring there is the same number of each atom on both sides of the equation. This can be achieved by adding coefficients (the numbers in front of the reactants or products) accordingly. After inspection, the balanced equation is: \(\mathrm{XeF}_{6} + 6\mathrm{OH}^{-} → \mathrm{Xe} + \(\mathrm{XeO}_{6}^{4-} + \mathrm{O}_{2} + 4\mathrm{F}^{-} + 3\mathrm{H}_{2} \mathrm{O}\)
03

Confirm the equation is balanced

By checking each type of atom separately one can confirm that the equation is balanced, which means having the same number of atoms of each element on both sides of the equation. The final chemical equation is: \(\mathrm{XeF}_{6} + 6\mathrm{OH}^{-} → \mathrm{Xe} + \mathrm{XeO}_{6}^{4-} + \mathrm{O}_{2} + 4\mathrm{F}^{-} + 3\mathrm{H}_{2} \mathrm{O}\)

Unlock Step-by-Step Solutions & Ace Your Exams!

  • Full Textbook Solutions

    Get detailed explanations and key concepts

  • Unlimited Al creation

    Al flashcards, explanations, exams and more...

  • Ads-free access

    To over 500 millions flashcards

  • Money-back guarantee

    We refund you if you fail your exam.

Start your free trial

Over 30 million students worldwide already upgrade their learning with Vaia!

One App. One Place for Learning.

All the tools & learning materials you need for study success - in one app.

Get started for free

Most popular questions from this chapter

In your own words, define the following terms: (a) polyhalide ion; (b) polyphosphate; (c) interhalogen; (d) disproportionation.

Polonium is the only element known to crystallize in the simple cubic form. In this structure, the interatomic distance between a Po atom and each of its six nearest neighbors is \(335 \mathrm{pm}\). Use this description of the crystal structure to estimate the density of polonium.

Although relatively rare, all of the following compounds exist. Based on what you know about related compounds (for example, from the periodic table), propose a plausible name or formula for each compound: (a) silver(I) astatide; (b) \(\mathrm{Na}_{4} \mathrm{XeO}_{6} ;\) (c) magnesium polonide; (d) \(\mathrm{H}_{2} \mathrm{TeO}_{3} ;\) (e) potassium thioselenate; (f) \(\mathrm{KAtO}_{4}\).

When heated, each of the following substances decomposes to the products indicated. Write balanced equations for these reactions. (a) \(\mathrm{NH}_{4} \mathrm{NO}_{3}(\mathrm{s})\) to \(\mathrm{N}_{2}(\mathrm{g}), \mathrm{O}_{2}(\mathrm{g}),\) and \(\mathrm{H}_{2} \mathrm{O}(\mathrm{g})\) (b) \(\mathrm{NaNO}_{3}(\mathrm{s})\) to sodium nitrite and oxygen gas (c) \(\mathrm{Pb}\left(\mathrm{NO}_{3}\right)_{2}(\mathrm{s})\) to lead(II) oxide, nitrogen dioxide, and oxygen.

Joseph Priestley, a British chemist, was credited with the discovering oxygen in \(1774 .\) In his experiments, he generated oxygen gas by heating \(\mathrm{HgO}(\mathrm{s}) .\) The other product of the decomposition reaction is \(\mathrm{Hg}(1) .\) What volume of wet \(\mathrm{O}_{2}(\mathrm{g})\) is obtained from the decomposition of \(1.0 \mathrm{g} \mathrm{HgO}(\mathrm{s}),\) if the gas is collected over water at \(25^{\circ} \mathrm{C}\) and a barometric pressure of \(756 \mathrm{mmHg} ?\) The vapor pressure of water is \(23.76 \mathrm{mmHg}\) at \(25^{\circ} \mathrm{C}\).
See all solutions

Recommended explanations on Chemistry Textbooks

Organic Chemistry

Read Explanation

Nuclear Chemistry

Read Explanation

Kinetics

Read Explanation

Chemical Analysis

Read Explanation

Inorganic Chemistry

Read Explanation

Chemistry Branches

Read Explanation
View all explanations

What do you think about this solution?

We value your feedback to improve our textbook solutions.

Study anywhere. Anytime. Across all devices.

Sign-up for free