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Chapter 3: Problem 94

Balance each of the following chemical equations. a. \(\mathrm{KO}_{2}(s)+\mathrm{H}_{2} \mathrm{O}(l) \rightarrow \mathrm{KOH}(a q)+\mathrm{O}_{2}(g)+\mathrm{H}_{2} \mathrm{O}_{2}(a q)\) b. \(\mathrm{Fe}_{2} \mathrm{O}_{3}(s)+\mathrm{HNO}_{3}(a q) \rightarrow \mathrm{Fe}\left(\mathrm{NO}_{3}\right)_{3}(a q)+\mathrm{H}_{2} \mathrm{O}(l)\) c. \(\mathrm{NH}_{3}(g)+\mathrm{O}_{2}(g) \rightarrow \mathrm{NO}(g)+\mathrm{H}_{2} \mathrm{O}(g)\) d. \(\mathrm{PCl}_{5}(l)+\mathrm{H}_{2} \mathrm{O}(l) \rightarrow \mathrm{H}_{3} \mathrm{PO}_{4}(a q)+\mathrm{HCl}(g)\) e. \(\mathrm{CaO}(s)+\mathrm{C}(s) \rightarrow \mathrm{CaC}_{2}(s)+\mathrm{CO}_{2}(g)\) f. \(\operatorname{MoS}_{2}(s)+\mathrm{O}_{2}(g) \rightarrow \mathrm{MoO}_{3}(s)+\mathrm{SO}_{2}(g)\) g. \(\mathrm{FeCO}_{3}(s)+\mathrm{H}_{2} \mathrm{CO}_{3}(a q) \rightarrow \mathrm{Fe}\left(\mathrm{HCO}_{3}\right)_{2}(a q)\)

Short Answer

Expert verified
a. \(\mathrm{KO}_{2} + 2\mathrm{H}_{2}\mathrm{O} \rightarrow 2\mathrm{KOH} + \mathrm{O}_{2} + \mathrm{H}_{2}\mathrm{O}_{2}\) b. \(\mathrm{Fe}_{2}\mathrm{O}_{3} + 6\mathrm{HNO}_{3} \rightarrow 2\mathrm{Fe}\left(\mathrm{NO}_{3}\right)_{3} + 3\mathrm{H}_{2}\mathrm{O}\) c. \(4\mathrm{NH}_{3} + 5\mathrm{O}_{2} \rightarrow 4\mathrm{NO} + 6\mathrm{H}_{2}\mathrm{O}\) d. \(\mathrm{PCl}_{5} + 4\mathrm{H}_{2}\mathrm{O} \rightarrow \mathrm{H}_{3}\mathrm{PO}_{4} + 5\mathrm{HCl}\) e. \(\mathrm{CaO} + \mathrm{C} \rightarrow \mathrm{CaC}_{2} + \mathrm{CO}_{2}\) f. \(\mathrm{MoS}_{2} + 7\mathrm{O}_{2} \rightarrow 2\mathrm{MoO}_{3} + 2\mathrm{SO}_{2}\) g. \(\mathrm{FeCO}_{3} + \mathrm{H}_{2}\mathrm{CO}_{3} \rightarrow \mathrm{Fe}\left(\mathrm{HCO}_{3}\right)_{2}\)

Step by step solution

01

Add coefficients to balance potassium on both sides

Start by adding a 2 in front of \(\mathrm{KOH}\): \(\mathrm{KO}_{2}+\mathrm{H}_{2}\mathrm{O} \rightarrow 2\mathrm{KOH}+\mathrm{O}_{2}+\mathrm{H}_{2}\mathrm{O}_{2}\)
02

Adjust coefficients to balance oxygen and hydrogen

Now, adjust the rest of the coefficients as such: \(\mathrm{KO}_{2}+2\mathrm{H}_{2}\mathrm{O} \rightarrow 2\mathrm{KOH}+\mathrm{O}_{2}+\mathrm{H}_{2}\mathrm{O}_{2}\) Now all atoms are balanced. b. Balancing iron(III) oxide (\(\mathrm{Fe}_{2}\mathrm{O}_{3}\)) reaction with nitric acid (\(\mathrm{HNO}_{3}\)):
03

Start by adding coefficients to balance iron and nitrate ions on both sides

Add a 2 in front of \(\mathrm{Fe}\left(\mathrm{NO}_{3}\right)_{3}\) and a 6 in front of \(\mathrm{HNO}_{3}\): \(\mathrm{Fe}_{2}\mathrm{O}_{3}+6\mathrm{HNO}_{3} \rightarrow 2\mathrm{Fe}\left(\mathrm{NO}_{3}\right)_{3}+3\mathrm{H}_{2}\mathrm{O}\) Now, all atoms are balanced. c. Balancing ammonia (\(\mathrm{NH}_{3}\)) reaction with oxygen gas (\(\mathrm{O}_{2}\)):
04

Start by adding coefficients to balance nitrogen and hydrogen on both sides

Add a 4 in front of \(\mathrm{NH}_{3}\) and a 4 in front of \(\mathrm{NO}\): \(4\mathrm{NH}_{3}+\mathrm{O}_{2} \rightarrow 4\mathrm{NO}+6\mathrm{H}_{2}\mathrm{O}\)
05

Adjust coefficients to balance oxygen

Finally, add a 5 in front of \(\mathrm{O}_{2}\): \(4\mathrm{NH}_{3}+5\mathrm{O}_{2} \rightarrow 4\mathrm{NO}+6\mathrm{H}_{2}\mathrm{O}\) Now all atoms are balanced. d. Balancing phosphorus pentachloride (\(\mathrm{PCl}_{5}\)) reaction with water (\(\mathrm{H}_{2}\mathrm{O}\)):
06

Start by adding coefficients to balance phosphorus and hydrogen on both sides

Add a 5 in front of \(\mathrm{HCl}\) and adjust the rest of the coefficients as such: \(\mathrm{PCl}_{5}+4\mathrm{H}_{2}\mathrm{O} \rightarrow \mathrm{H}_{3}\mathrm{PO}_{4}+5\mathrm{HCl}\) Now all atoms are balanced. e. Balancing calcium oxide (\(\mathrm{CaO}\)) reaction with carbon (\(\mathrm{C}\)):
07

No coefficients need to be added

\(\mathrm{CaO}+\mathrm{C} \rightarrow \mathrm{CaC}_{2}+\mathrm{CO}_{2}\) All atoms are already balanced. f. Balancing molybdenum disulfide (\(\mathrm{MoS}_{2}\)) reaction with oxygen gas (\(\mathrm{O}_{2}\)):
08

Start by adding coefficients to balance molybdenum and sulfur on both sides

Add a 2 in front of \(\mathrm{MoO}_{3}\) and a 2 in front of \(\mathrm{SO}_{2}\): \(\mathrm{MoS}_{2}+\mathrm{O}_{2} \rightarrow 2\mathrm{MoO}_{3}+2\mathrm{SO}_{2}\)
09

Adjust coefficients to balance oxygen

Now, add a 7 in front of \(\mathrm{O}_{2}\): \(\mathrm{MoS}_{2}+7\mathrm{O}_{2} \rightarrow 2\mathrm{MoO}_{3}+2\mathrm{SO}_{2}\) Now all atoms are balanced. g. Balancing iron(II) carbonate (\(\mathrm{FeCO}_{3}\)) reaction with carbonic acid (\(\mathrm{H}_{2}\mathrm{CO}_{3}\)):
10

No coefficients need to be added

\(\mathrm{FeCO}_{3}+\mathrm{H}_{2}\mathrm{CO}_{3} \rightarrow \mathrm{Fe}\left(\mathrm{HCO}_{3}\right)_{2}\) All atoms are already balanced.

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Most popular questions from this chapter

Consider the following balanced chemical equation: $$ A+5 B \longrightarrow 3 C+4 D $$ a. Equal masses of \(\mathrm{A}\) and \(\mathrm{B}\) are reacted. Complete each of the following with either "A is the limiting reactant because \(" ;{ }^{\prime *} \mathrm{~B}\) is the limiting reactant because \("\) or "we cannot determine the limiting reactant because i. If the molar mass of \(\mathrm{A}\) is greater than the molar mass of B, then ii. If the molar mass of \(\mathrm{B}\) is greater than the molar mass of A, then b. The products of the reaction are carbon dioxide (C) and water (D). Compound \(\mathrm{A}\) has the same molar mass as carbon dioxide. Compound \(\mathrm{B}\) is a diatomic molecule. Identify \(\mathrm{com}-\) pound \(\mathrm{B}\) and support your answer. c. Compound \(\mathrm{A}\) is a hydrocarbon that is \(81.71 \%\) carbon by mass. Detemine its empirical and molecular formulas.

What amount (moles) is represented by each of these samples? a. \(150.0 \mathrm{~g} \mathrm{Fe}_{2} \mathrm{O}_{3}\) b. \(10.0 \mathrm{mg} \mathrm{NO}_{2}\) c. \(1.5 \times 10^{16}\) molecules of \(\mathrm{BF}_{3}\)

The compound \(\mathrm{As}_{2} \mathrm{I}_{4}\) is synthesized by reaction of arsenic metal with arsenic triiodide. If a solid cubic block of arsenic \((d=5.72\) \(\mathrm{g} / \mathrm{cm}^{3}\) ) that is \(3.00 \mathrm{~cm}\) on edge is allowed to react with \(1.01 \times 10^{24}\) molecules of arsenic triiodide, what mass of \(\mathrm{As}_{2} \mathrm{I}_{4}\) can be prepared? If the percent yield of \(\mathrm{As}_{2} \mathrm{I}_{4}\) was \(75.6 \%\), what mass of \(\mathrm{As}_{2} \mathrm{I}_{4}\) was actually isolated?

Boron consists of two isotopes, \({ }^{10} \mathrm{~B}\) and \({ }^{11} \mathrm{~B}\). Chlorine also has two isotopes, \({ }^{35} \mathrm{Cl}\) and \({ }^{37} \mathrm{Cl}\). Consider the mass spectrum of \(\mathrm{BCl}_{3}\). How many peaks would be present, and what approximate mass would each peak correspond to in the \(\mathrm{BCl}_{3}\) mass spectrum?

In using a mass spectrometer, a chemist sees a peak at a mass of \(30.0106\). Of the choices \({ }^{12} \mathrm{C}_{2}{ }^{1} \mathrm{H}_{6},{ }^{12} \mathrm{C}^{1} \mathrm{H}_{2}{ }^{16} \mathrm{O}\), and \({ }^{14} \mathrm{~N}^{16} \mathrm{O}\), which is responsible for this peak? Pertinent masses are \({ }^{1} \mathrm{H}, 1.007825\); \({ }^{16} \mathrm{O}, 15.994915 ;\) and \({ }^{14} \mathrm{~N}, 14.003074 .\)
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