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Chapter 6: Problem 19

Elemental boron is produced in one industrial process by heating diboron trioxide with magnesium metal, also producing magnesium oxide as a by-product. Write the unbalanced chemical equation for this process.

Short Answer

Expert verified
\(B_2O_3 + Mg \rightarrow B + MgO\)

Step by step solution

01

1. Identify the reactants and products

The first step is to identify the chemical formulas for the reactants and products involved in the process. In this case, the reactants are diboron trioxide (B_2O_3) and magnesium metal (Mg), and the products are elemental boron (B) and magnesium oxide (MgO).
02

2. Write the unbalanced chemical equation

Now that we have identified the reactants and products, we can write the unbalanced chemical equation for this process. An unbalanced chemical equation shows the correct formulas for all species involved but does not necessarily obey the Law of Conservation of Mass (i.e., it may not have equal numbers of atoms for each element on both sides of the equation). Here is the unbalanced chemical equation for the given process: \(B_2O_3 + Mg \rightarrow B + MgO\) This equation represents the industrial process of producing elemental boron by heating diboron trioxide with magnesium metal while magnesium oxide is generated as a by-product.

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Most popular questions from this chapter

After balancing a chemical equation, we ordinarily make sure that the coefficients are the smallest ________ possible.

Balance each of the following chemical equations. a. \(\mathrm{SiCl}_{4}(l)+\mathrm{Mg}(s) \rightarrow \mathrm{Si}(s)+\mathrm{MgCl}_{2}(s)\) b. \(\mathrm{NO}(g)+\mathrm{Cl}_{2}(g) \rightarrow \mathrm{NOCl}(g)\) c. \(\operatorname{MnO}_{2}(s)+\mathrm{Al}(s) \rightarrow \operatorname{Mn}(s)+\mathrm{Al}_{2} \mathrm{O}_{3}(s)\) d. \(\operatorname{Cr}(s)+S_{8}(s) \rightarrow C r_{2} S_{3}(s)\) e. \(\mathrm{NH}_{3}(g)+\mathrm{F}_{2}(g) \rightarrow \mathrm{NH}_{4} \mathrm{F}(s)+\mathrm{NF}_{3}(g)\) f. \(\mathrm{Ag}_{2} \mathrm{S}(s)+\mathrm{H}_{2}(g) \rightarrow \mathrm{Ag}(s)+\mathrm{H}_{2} \mathrm{S}(g)\) g. \(\mathrm{O}_{2}(g) \rightarrow \mathrm{O}_{3}(g)\) h. \(\mathrm{Na}_{2} \mathrm{SO}_{3}(a q)+\mathrm{S}_{8}(s) \rightarrow \mathrm{Na}_{2} \mathrm{S}_{2} \mathrm{O}_{3}(a q)\)

Balance each of the following chemical equations. a. \(\mathrm{FeCl}_{3}(a q)+\mathrm{KOH}(a q) \rightarrow \mathrm{Fe}(\mathrm{OH})_{3}(s)+\mathrm{KCl}(a q)\). b. \(\mathrm{Pb}\left(\mathrm{C}_{2} \mathrm{H}_{3} \mathrm{O}_{2}\right)_{2}(a q)+\mathrm{KI}(a q) \rightarrow\) \(\mathrm{PbI}_{2}(s)+\mathrm{KC}_{2} \mathrm{H}_{3} \mathrm{O}_{2}(a q)\) c. \(\mathrm{P}_{4} \mathrm{O}_{10}(s)+\mathrm{H}_{2} \mathrm{O}(l) \rightarrow \mathrm{H}_{3} \mathrm{PO}_{4}(a q)\) d. \(\mathrm{Li}_{2} \mathrm{O}(s)+\mathrm{H}_{2} \mathrm{O}(l) \rightarrow \mathrm{LiOH}(a q)\) e. \(\operatorname{MnO}_{2}(s)+\mathrm{C}(s) \rightarrow \operatorname{Mn}(s)+\mathrm{CO}_{2}(g)\) f. \(\operatorname{Sb}(s)+\mathrm{Cl}_{2}(g) \rightarrow \mathrm{SbCl}_{3}(s)\) g. \(\mathrm{CH}_{4}(g)+\mathrm{H}_{2} \mathrm{O}(g) \rightarrow \mathrm{CO}(g)+\mathrm{H}_{2}(g)\) h. \(\operatorname{FeS}(s)+\operatorname{HCl}(a q) \rightarrow \operatorname{Fe} \mathrm{Cl}_{2}(a q)+\mathrm{H}_{2} \mathrm{S}(g)\)

How do we know when a chemical reaction is taking place? Can you think of an example of how each of the five senses (sight, hearing, taste, touch, smell) might be used in detecting when a chemical reaction has taken place?

When lead(II) sulfide is heated to high temperatures in a stream of pure oxygen gas, solid lead(II) oxide forms with the release of gaseous sulfur dioxide. Write the unbalanced chemical equation for this reaction.
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