Log out Go to App
Go to App

Learning Materials

Features

Discover

Chapter 20: Problem 29

Boron hydrides were once evaluated for possible use as rocket fuels. Complete and balance the following equation for the combustion of diborane. $$\mathrm{B}_{2} \mathrm{H}_{6}+\mathrm{O}_{2} \longrightarrow \mathrm{B}(\mathrm{OH})_{3}$$

Short Answer

Expert verified
The balanced equation for the combustion of diborane (\(\mathrm{B}_{2}\mathrm{H}_{6}\)) with oxygen (\(\mathrm{O}_{2}\)) to produce boron hydroxide (\(\mathrm{B}(\mathrm{OH})_{3}\)) is: \[ \mathrm{B}_{2}\mathrm{H}_{6} + 3\mathrm{O}_{2} \longrightarrow 2\mathrm{B}(\mathrm{OH})_{3} \]

Step by step solution

01

Identify All Chemical Species

In this combustion reaction, we have: - Diborane (B2H6) as the reactant - Oxygen (O2) as the reactant - Boron hydroxide (BOH3) as the product
02

Write the Unbalanced Equation

Now, let's write the unbalanced chemical equation: $$ \mathrm{B}_{2}\mathrm{H}_{6} + \mathrm{O}_{2} \longrightarrow \mathrm{B}(\mathrm{OH})_{3} $$
03

Balance the Equation for Boron Atoms

Since there are 2 boron atoms in B2H6, we need 2 boron hydroxide (BOH3) units on the product side to balance the boron atoms: $$ \mathrm{B}_{2}\mathrm{H}_{6} + \mathrm{O}_{2} \longrightarrow \underline{2}\mathrm{B}(\mathrm{OH})_{3} $$
04

Balance the Equation for Hydrogen Atoms

We have 6 hydrogen atoms in B2H6, and there are 3 hydrogen atoms in each BOH3 molecule. Since we have 2 BOH3 molecules on the product side, the hydrogen atoms are already balanced: $$ \mathrm{B}_{2}\mathrm{H}_{6} + \mathrm{O}_{2} \longrightarrow 2\mathrm{B}(\mathrm{OH})_{3} $$
05

Balance the Equation for Oxygen Atoms

Finally, we need to balance the oxygen atoms. We have 3 oxygen atoms in each of the 2 BOH3 molecules on the product side, making a total of 6 oxygen atoms. So, we need 3 O2 molecules on the reactant side to balance the oxygen atoms: $$ \mathrm{B}_{2}\mathrm{H}_{6} + \underline{3}\mathrm{O}_{2} \longrightarrow 2\mathrm{B}(\mathrm{OH})_{3} $$
06

Check the Balanced Equation

Now our balanced equation is: $$ \mathrm{B}_{2}\mathrm{H}_{6} + 3\mathrm{O}_{2} \longrightarrow 2\mathrm{B}(\mathrm{OH})_{3} $$ Let's check the number of atoms for each element: - Boron: 2 atoms on both sides (B2H6 and 2*BOH3) - Hydrogen: 6 atoms on both sides (B2H6 and 2*(3*H)) - Oxygen: 6 atoms on both sides (3*O2 and 2*(3*O)) The chemical equation is now balanced.

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

Many structures of phosphorus-containing compounds are drawn with some \(\mathrm{P}=\mathrm{O}\) bonds. These bonds are not the typical \(\pi\) bonds we've considered, which involve the overlap of two \(p\) orbitals. Instead, they result from the overlap of a \(d\) orbital on the phosphorus atom with a \(p\) orbital on oxygen. This type of \(\pi\) bonding is sometimes used as an explanation for why \(\mathrm{H}_{3} \mathrm{PO}_{3}\) has the first structure below rather than the second: Draw a picture showing how a \(d\) orbital and a \(p\) orbital overlap to form a \(\pi\) bond.

Silicon is produced for the chemical and electronics industries by the following reactions. Give the balanced equation for each reaction. a. \(\mathrm{SiO}_{2}(s)+\mathrm{C}(s) \longrightarrow \mathrm{Si}(s)+\mathrm{CO}(g)\) b. Silicon tetrachloride is reacted with very pure magnesium, producing silicon and magnesium chloride. c. \(\mathrm{Na}_{2} \mathrm{SiF}_{6}(s)+\mathrm{Na}(s) \longrightarrow \mathrm{Si}(s)+\mathrm{NaF}(s)\)

Although the earth was formed from the same interstellar material as the sun, there is little elemental hydrogen \(\left(\mathrm{H}_{2}\right)\) in the earth's atmosphere. Explain.

Using data from Appendix 4, calculate \(\Delta H^{\circ}, \Delta G^{\circ}\), and \(K_{\mathrm{p}}\) (at \(298 \mathrm{~K}\) ) for the production of ozone from oxygen: $$3 \mathrm{O}_{2}(g) \rightleftharpoons 2 \mathrm{O}_{3}(g)$$ At \(30 \mathrm{~km}\) above the surface of the earth, the temperature is about \(230 . \mathrm{K}\), and the partial pressure of oxygen is about \(1.0 \times 10^{-3}\) atm. Estimate the partial pressure of ozone in equilibrium with oxygen at \(30 \mathrm{~km}\) above the earth's surface. Is it reasonable to assume that the equilibrium between oxygen and ozone is maintained under these conditions? Explain.

One harmful effect of acid rain is the deterioration of structures and statues made of marble or limestone, both of which are essentially calcium carbonate. The reaction of calcium carbonate with sulfuric acid yields carbon dioxide, water, and calcium sulfate. Because calcium sulfate is marginally soluble in water, part of the object is washed away by the rain. Write a balanced chemical equation for the reaction of sulfuric acid with calcium carbonate.
See all solutions

Recommended explanations on Chemistry Textbooks

Nuclear Chemistry

Read Explanation

Chemical Reactions

Read Explanation

Physical Chemistry

Read Explanation

Chemistry Branches

Read Explanation

Inorganic Chemistry

Read Explanation

The Earths Atmosphere

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