Log out Go to App
Go to App

Learning Materials

Features

Discover

Chapter 22: Problem 37

Write balanced equations for each of the following reactions.(a) When mercury (II) oxide is heated, it decomposes to form \(\mathrm{O}_{2}\) and mercury metal. (b) When copper(II) nitrate is heated strongly, it decomposes to form copper(II) oxide, nitrogen dioxide, and oxygen. (c) Lead(II) sulfide, PbS(s) reacts with ozone to form PbSO \(_{4}(s)\) and \(\mathrm{O}_{2}(g) .\) (d) When heated in air, \(Z n S(s)\) is converted to ZnO. (e) Potassium peroxide reacts with \(\mathrm{CO}_{2}(g)\) to give potassium carboate and \(\mathrm{O}_{2} .(\mathbf{f})\) Oxygen is converted to ozone in the upper atmosphere.

Short Answer

Expert verified
(a) \(2HgO \rightarrow O_2 + 2Hg\) (b) \(2Cu(NO_3)_2 \rightarrow 2CuO + 4NO_2 + O_2\) (c) \(PbS + 2O_3 \rightarrow PbSO_4 + O_2\) (d) \(ZnS + 3O_2 \rightarrow 2ZnO\) (e) \(2K_2O_2 + CO_2 \rightarrow K_2CO_3 + 2O_2\) (f) \(3O_2 \rightarrow 2O_3\)

Step by step solution

01

(a) Mercury(II) oxide decomposing to form O2 and mercury metal

Write the reaction: \[HgO \rightarrow O_2 + Hg\] Balance the equation: \[2HgO \rightarrow O_2 + 2Hg\]
02

(b) Copper(II) nitrate decomposing to form copper(II) oxide, nitrogen dioxide, and oxygen

Write the reaction: \[Cu(NO_3)_2 \rightarrow CuO + NO_2 + O_2\] Balance the equation: \[2Cu(NO_3)_2 \rightarrow 2CuO + 4NO_2 + O_2\]
03

(c) Lead(II) sulfide reacting with ozone to form PbSO4 and O2

Write the reaction: \[PbS + O_3 \rightarrow PbSO_4 + O_2\] Balance the equation: \[PbS + 2O_3 \rightarrow PbSO_4 + O_2\]
04

(d) Zinc sulfide being converted to zinc oxide when heated in air

Write the reaction: \[ZnS + O_2 \rightarrow ZnO\] Balance the equation: \[ZnS + 3O_2 \rightarrow 2ZnO\]
05

(e) Potassium peroxide reacting with CO2 to give potassium carbonate and O2

Write the reaction: \[K_2O_2 + CO_2 \rightarrow K_2CO_3 + O_2\] Balance the equation: \[2K_2O_2 + CO_2 \rightarrow K_2CO_3 + 2O_2\]
06

(f) Oxygen being converted to ozone in the upper atmosphere

Write the reaction: \[O_2 \rightarrow O_3\] Balance the equation: \[3O_2 \rightarrow 2O_3\]

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

Write complete balanced half-reactions for (a) oxidation of nitrous acid to nitrate ion in acidic solution, (b) oxidation of \(\mathrm{N}_{2}\) to \(\mathrm{N}_{2} \mathrm{O}\) in acidic solution.

Identify each of the following elements as a metal, non metal, or metalloid: (a) gallium, (b) molybdenum, (c) tellurium, ( \(\mathbf{d}\) ) arsenic, (e) xenon, (f) ruthenium.

A sulfuric acid plant produces a considerable amount of heat. This heat is used to generate electricity, which helps reduce operating costs. The synthesis of \(\mathrm{H}_{2} \mathrm{SO}_{4}\) consists of three main chemical processes: (a) oxidation of S to SO, (b) oxidation of \(\mathrm{SO}_{2}\) to \(\mathrm{SO}_{3},\) (c) the dissolving of \(\mathrm{SO}_{3}\) in \(\mathrm{H}_{2} \mathrm{SO}_{4}\) and the subsequent reaction with water to form \(\mathrm{H}_{2} \mathrm{SO}_{4}\) . If the third process produces \(130 \mathrm{kJ} / \mathrm{mol},\) how much heat is produced in preparing a mole of \(\mathrm{H}_{2} \mathrm{SO}_{4}\) from a mole of S? How much heat is produced in preparing 5000 pounds of \(\mathrm{H}_{2} \mathrm{SO}_{4} ?\)

Write a balanced chemical reaction for the condensation reaction between \(\mathrm{H}_{3} \mathrm{PO}_{4}\) molecules to form \(\mathrm{H}_{5} \mathrm{P}_{3} \mathrm{O}_{10} .\)

Account for the following observations: (a) \(\mathrm{H}_{3} \mathrm{PO}_{3}\) is a diprotic acid. (b) Nitric acid is a strong acid, whereas phosphoric acid is weak. (c) Phosphate rock is ineffective as a phosphate fertilizer. (d) Phosphorus does not exist at room temperature as diatomic molecules, but nitrogen does. (e) Solutions of \(\mathrm{Na}_{3} \mathrm{PO}_{4}\) are quite basic.
See all solutions

Recommended explanations on Chemistry Textbooks

Organic Chemistry

Read Explanation

Inorganic Chemistry

Read Explanation

Making Measurements

Read Explanation

Ionic and Molecular Compounds

Read Explanation

Nuclear Chemistry

Read Explanation

Physical Chemistry

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