/*! This file is auto-generated */ .wp-block-button__link{color:#fff;background-color:#32373c;border-radius:9999px;box-shadow:none;text-decoration:none;padding:calc(.667em + 2px) calc(1.333em + 2px);font-size:1.125em}.wp-block-file__button{background:#32373c;color:#fff;text-decoration:none} Problem 26 Write balanced equations for eac... [FREE SOLUTION] | 91影视

91影视

Log out

Learning Materials

Features

Discover

Chapter 22: Problem 26

Write balanced equations for each of the following reactions (some of these are analogous to reactions shown in the chapter). (a) Aluminum metal reacts with acids to form hydrogen gas. (b) Steam reacts with magnesium metal to give magnesium oxide and hydrogen. (c) Manganese(IV) oxide is reduced to manganese(II) oxide by hydrogen gas. (d) Calcium hydride reacts with water to generate hydrogen gas.

Short Answer

Expert verified
The balanced equations for the given reactions are as follows: a) \(2Al(s) + 6HCl(aq) \rightarrow 2AlCl鈧�(aq) + 3H鈧�(g)\) b) \(Mg(s) + H鈧侽(g) \rightarrow MgO(s) + H鈧�(g)\) c) \(MnO鈧�(s) + 2H鈧�(g) \rightarrow MnO(s) + 2H鈧侽(g)\) d) \(CaH鈧�(s) + 2H鈧侽(l) \rightarrow Ca(OH)鈧�(aq) + 2H鈧�(g)\)

Step by step solution

01

Write the unbalanced equation

Al(s) + HCl(aq) -> AlCl鈧�(aq) + H鈧�(g)
02

Balance the equation

To balance the equation, we need 6 HCl molecules to produce 3 H鈧� molecules so that there are 6 H atoms on both sides of the equation. So, the balanced equation will be: 2Al(s) + 6HCl(aq) -> 2AlCl鈧�(aq) + 3H鈧�(g) #b)# Steam reacts with magnesium to give magnesium oxide and hydrogen
03

Write the unbalanced equation

Mg(s) + H鈧侽(g) -> MgO(s) + H鈧�(g)
04

Balance the equation

To balance the equation, we simply need 1 Mg atom, 1 H鈧侽 molecule, 1 MgO molecule and 1 H鈧� molecule, as there are already equal numbers of Mg, O and H atoms on both sides. The balanced equation is: Mg(s) + H鈧侽(g) -> MgO(s) + H鈧�(g) #c)# Manganese(IV) oxide is reduced to manganese(II) oxide by hydrogen gas
05

Write the unbalanced equation

MnO鈧�(s) + H鈧�(g) -> MnO(s) + H鈧侽(g)
06

Balance the equation

To balance this equation, 2 H atoms are needed on both sides of the equation. The balanced equation is: MnO鈧�(s) + 2H鈧�(g) -> MnO(s) + 2H鈧侽(g) #d)# Calcium hydride reacts with water to generate hydrogen gas
07

Write the unbalanced equation

CaH鈧�(s) + H鈧侽(l) -> Ca(OH)鈧�(aq) + H鈧�(g)
08

Balance the equation

In this case, we need the same number of H, Ca and O atoms on both sides of the equation: 2 H鈧侽 molecules provide 4 H atoms to balance the 4 H atoms from CaH鈧� and H鈧�. The balanced equation is: CaH鈧�(s) + 2H鈧侽(l) -> Ca(OH)鈧�(aq) + 2H鈧�(g)

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.

Over 30 million students worldwide already upgrade their learning with 91影视!

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 the chemical formula for each of the following compounds, and indicate the oxidation state of nitrogen in each: (a) sodium nitrite, (b) ammonia, (c) nitrous oxide, (d) sodium cyanide, (e) nitric acid, (f) nitrogen dioxide.

Account for the following observations: (a) Phosphorus forms a pentachloride, but nitrogen does not. (b) \(\mathrm{H}_{3} \mathrm{PO}_{2}\) is a monoprotic acid. (c) Phosphonium salts, such as \(\mathrm{PH}_{4} \mathrm{Cl}\), can be formed under anhydrous conditions, but they can't be made in aqueous solution. (d) White phosphorus is extremely reactive.

Explain each of the following observations: (a) At room temperature \(\mathrm{I}_{2}\) is a solid, \(\mathrm{Br}_{2}\) is a liquid, and \(\mathrm{Cl}_{2}\) and \(\mathrm{F}_{2}\) are both gases. (b) \(\mathrm{F}_{2}\) cannot be prepared by electrolytic oxidation of aqueous \(\mathrm{F}^{-}\) solutions. (c) The boiling point of HF is much higher than those of the other hydrogen halides. (d) The halogens decrease in oxidizing power in the order \(\mathrm{F}_{2}>\mathrm{Cl}_{2}>\mathrm{Br}_{2}>\mathrm{I}_{2}\)

Write the chemical formula for each of the following compounds, and indicate the oxidation state of the group \(6 \mathrm{~A}\) element in each: (a) sulfur tetrachloride, (b) selenium trioxide, (c) sodium thiosulfate, (d) hydrogen sulfide, \((\mathrm{e})\) sulfuric acid.

Write a molecular formula for each compound, and indicate the oxidation state of the group \(5 \mathrm{~A}\) element in each formula: (a) phosphorous acid, (b) pyrophosphoric acid, (c) antimony trichloride, (d) magnesium arsenide, (e) diphosphorus pentoxide.
See all solutions

Recommended explanations on Chemistry Textbooks

Chemical Reactions

Read Explanation

Making Measurements

Read Explanation

The Earths Atmosphere

Read Explanation

Chemical Analysis

Read Explanation

Ionic and Molecular Compounds

Read Explanation

Inorganic 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.