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Chapter 8: Problem 34

Complete and balance the equation for the complete combustion of each of the following. $$ \begin{array}{ll}{\text { a. } C_{3} \mathrm{H}_{6}} & {\text { c. } C \mathrm{H}_{3} \mathrm{OH}} \\ {\text { b. } C_{5} \mathrm{H}_{12}} & {\text { d. } C_{12} \mathrm{H}_{22} \mathrm{O}_{11}}\end{array} $$

Short Answer

Expert verified
a) \( C_{3}H_{6} + \frac{9}{2}O_{2} \rightarrow 3CO_{2} + 3H_{2}O \) b) \(C_{5}H_{12} + \frac{17}{2}O_{2} \rightarrow 5CO_{2} + 6H_{2}O \) c) \( CH_{3}OH + \frac{3}{2}O_{2} \rightarrow CO_{2} + 2H_{2}O \) d) \( C_{12}H_{22}O_{11} + 12O_{2} \rightarrow 12CO_{2} + 11H_{2}O \)

Step by step solution

01

- Complete Combustion of Propane (C3H6)

Write down the general formula for complete combustion of propane: \( C_{3}H_{6} + O_{2} \rightarrow CO_{2} + H_{2}O \). The final step is to balance the equation by adjusting the coefficients (number of molecules) such that the number of atoms of each element is the same on both sides. The balanced equation is: \( C_{3}H_{6} + \frac{9}{2}O_{2} \rightarrow 3CO_{2} + 3H_{2}O \)
02

- Complete Combustion of Pentane (C5H12)

General formula for complete combustion of pentane: \( C_{5}H_{12} + O_{2} \rightarrow CO_{2} + H_{2}O \). The balanced equation is: \( C_{5}H_{12} + \frac{17}{2}O_{2} \rightarrow 5CO_{2} + 6H_{2}O \)
03

- Complete Combustion of Methanol(CH3OH)

General formula for complete combustion of methanol: \( CH_{3}OH + O_{2} \rightarrow CO_{2} + H_{2}O \). The balanced equation is: \( CH_{3}OH + \frac{3}{2}O_{2} \rightarrow CO_{2} + 2H_{2}O \)
04

- Complete Combustion of Sucrose (C12H22O11)

General formula for complete combustion of sucrose: \( C_{12}H_{22}O_{11} + O_{2} \rightarrow CO_{2} + H_{2}O \). The balanced equation is: \( C_{12}H_{22}O_{11} + 12O_{2} \rightarrow 12CO_{2} + 11H_{2}O \)

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Most popular questions from this chapter

Identify the type of reaction for each of the following. Then, predict products for the reaction, and balance the equation." reaction occurs, write "no reaction." $$\text{a}. \mathrm{HCl}(a q)+\mathrm{NaOH}(a q) \rightarrow\mathrm{NaCl}(a q)+\mathrm{H}_{2} \mathrm{O}(l)$$ $$\text{b}. \mathrm{Mg}(s)+2 \mathrm{HCl}(a q) \rightarrow \mathrm{MgCl}_{2}(a q)+\mathrm{H}_{2}(g)$$ $$\text{c}. \mathrm{CdCl}_{2}(a q)+\mathrm{Na}_{2} \mathrm{CO}_{3}(a q) \rightarrow 2 \mathrm{NaCl}(a q)+\mathrm{CdCO}_{3}(s)$$

Identify the type of reaction for each of the following. Then, predict products for the reaction and balance the equation. If no reaction occurs, write "no reaction." $$ \begin{array}{l}{\text { a. } \mathrm{C}_{2} \mathrm{H}_{6}+\mathrm{O}_{2} \rightarrow} \\ {\text { b. } \mathrm{H}_{2} \mathrm{SO}_{4}+\mathrm{Al} \rightarrow} \\ {\text { c. } \mathrm{N}_{2}+\mathrm{Mg} \rightarrow} \\\ {\text { d. } \mathrm{Na}_{2} \mathrm{CO}_{3} \rightarrow} \\ {\text { e. } \mathrm{Mg}\left(\mathrm{NO}_{3}\right)_{2}+\mathrm{Na}_{2} \mathrm{SO}_{4} \longrightarrow}\end{array} $$

Balance the following equations. $$\text{a}. \mathrm{CaH}_{2}(s)+\mathrm{H}_{2} \mathrm{O}(l) \longrightarrow\mathrm{Ca}(\mathrm{OH})_{2}(a q)+\mathrm{H}_{2}(g)$$ $$\text{b}. \mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{CCH}(g)+\mathrm{Br}_{2}(l) \longrightarrow\mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{CBr}_{2} \mathrm{CHBr}_{2}(l)$$ $$\text{c} \cdot \mathrm{Pb}^{2+}(a q)+\mathrm{OH}^{-}(a q) \rightarrow \mathrm{Pb}(\mathrm{OH})_{2}(s)$$ $$\text{d} . \mathrm{NO}_{2}(g)+\mathrm{H}_{2} \mathrm{O}(l) \rightarrow \mathrm{HNO}_{3}(a q)+\mathrm{NO}(g)$$

Graphing Calculator Least Common Multiples When writing chemical formulas or balancing a chemical equation, being able to identify the least com- mon multiple of a set of numbers can often help. Your graphing calculator has a least common multiple function that can compare two numbers. On a TI-83 Plus or similar graphing calculator, press MATH 8 . The screen should read "lcm(." Next, enter one number and then a comma followed by the other number and a closing parenthesis. Press ENTER, and the calculator will show the least common multiple of the pair you entered. Use this function as needed to find the answers to the following questions. $$\begin{array}{l}{\text { a. Tin(IV) sulfate contains } \mathrm{Sn}^{4+} \text { and } \mathrm{SO}_{4}^{2-}} \\ {\text { ions. Use the least common multiple of } 2} \\ {\text { and } 4 \text { to determine the empirical formula }} \\ {\text { for this compound. }}\end{array}$$ $$ \begin{array}{l}{\text { b. Aluminum ferrocyanide contains } \mathrm{Al}^{3+} \text { ions }} \\ {\text { and } \mathrm{Fe}(\mathrm{CN})_{6}^{4} \text { ions. Use the least common }} \\ {\text { multiple of } 3 \text { and } 4 \text { to determine the empiri- }} \\ {\text { cal formula for this compound. }}\end{array} $$ $$\text{c. Balance the following unbalanced equation}.$$$$ \text{___}\mathrm{P}_{4} \mathrm{O}_{10}(s)+\text{___}\mathrm{H}_{2} \mathrm{O}(g) \rightarrow\text{___}\mathrm{H}_{3} \mathrm{PO}_{4}(a q)$$ $$\text{d. Balance the following unbalanced equation}.$$ $$ \text{___}\mathrm{KMnO}_{4}(a q)+\text{___}\mathrm{MnCl}_{2}(a q)+2 \mathrm{H}_{2} \mathrm{O}(l) \longrightarrow\text{___}\mathrm{MnO}_{2}(s)+4 \mathrm{HCl}(a q)+2 \mathrm{KCl}(a q) $$

Write a balanced equation for each of the following: a. iron(III) oxide + magnesium \(\rightarrow\) magnesium oxide + iron b. nitrogen dioxide + water \(\longrightarrow\) nitric acid + nitrogen monoxide c. silicon tetrachloride + water \(\rightarrow\) silicon dioxide + hydrochloric acid
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