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Chapter 4: Problem 7

Write balanced equations to represent the complete combustion of each of the following in excess oxygen: (a) butane, \(\mathrm{C}_{4} \mathrm{H}_{10} ;\) (b) isopropyl alcohol, \(\mathrm{CH}_{3} \mathrm{CH}(\mathrm{OH}) \mathrm{CH}_{3} ;\) (c) lactic acid, \(\mathrm{CH}_{3} \mathrm{CH}(\mathrm{OH}) \mathrm{COOH}\)

Short Answer

Expert verified
The balanced equations for the complete combustion are: (a) \(\mathrm{C}_{4} \mathrm{H}_{10} + 13/2 O_{2} \rightarrow 4 CO_{2} + 5 H_{2}O\) (b) \(\mathrm{CH}_{3} \mathrm{CH}(\mathrm{OH}) \mathrm{CH}_{3} + 4O_{2} \rightarrow 3CO_{2} + 4H_{2}O\) (c) \(\mathrm{CH}_{3} \mathrm{CH}(\mathrm{OH}) \mathrm{COOH} + 3O_{2} \rightarrow 3CO_{2} + 4H_{2}O\)

Step by step solution

01

Combustion of Butane

Butane, \(\mathrm{C}_{4} \mathrm{H}_{10}\), reacts with oxygen (O2) to produce carbon dioxide (CO2) and water (H2O). The unbalanced equation is \( \mathrm{C}_{4} \mathrm{H}_{10} + O_{2} \rightarrow CO_{2} + H_{2}O\). To balance the equation, start by balancing the carbons, followed by the hydrogen and lastly the oxygen, providing the balanced equation \( \mathrm{C}_{4} \mathrm{H}_{10} + 13/2 O_{2} \rightarrow 4 CO_{2} + 5 H_{2}O\)
02

Combustion of Isopropyl Alcohol

Isopropyl alcohol, \(\mathrm{CH}_{3} \mathrm{CH}(\mathrm{OH}) \mathrm{CH}_{3}\), reacts with oxygen (O2) to also produce carbon dioxide (CO2) and water (H2O). The unbalanced equation is \( \mathrm{CH}_{3} \mathrm{CH}(\mathrm{OH}) \mathrm{CH}_{3} + O_{2} \rightarrow CO_{2} + H_{2}O\). Again, balance the carbons first, then hydrogens, and finally the oxygens, to get the balanced equation \( \mathrm{CH}_{3} \mathrm{CH}(\mathrm{OH}) \mathrm{CH}_{3} + 4O_{2} \rightarrow 3CO_{2} + 4H_{2}O\)
03

Combustion of Lactic Acid

Lactic acid, \(\mathrm{CH}_{3} \mathrm{CH}(\mathrm{OH}) \mathrm{COOH}\), undergoes combustion with oxygen (O2) to yield carbon dioxide (CO2) and water (H2O). The unbalanced equation is \( \mathrm{CH}_{3} \mathrm{CH}(\mathrm{OH}) \mathrm{COOH} + O_{2} \rightarrow CO_{2} + H_{2}O\). Begin by balancing the carbons, then hydrogens, and finally the oxygens, resulting in the balanced equation \( \mathrm{CH}_{3} \mathrm{CH}(\mathrm{OH}) \mathrm{COOH} + 3O_{2} \rightarrow 3CO_{2} + 4H_{2}O\)

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Most popular questions from this chapter

The rocket boosters of the space shuttle Discovery, launched on July \(26,2005,\) used a fuel mixture containing primarily solid ammonium perchlorate, \(\mathrm{NH}_{4} \mathrm{ClO}_{4}(\mathrm{s}),\) and aluminum metal. The unbalanced chemical equation for the reaction is given below. \(\mathrm{Al}(\mathrm{s})+\mathrm{NH}_{4} \mathrm{ClO}_{4}(\mathrm{s}) \longrightarrow\) $$ \mathrm{Al}_{2} \mathrm{O}_{3}(\mathrm{s})+\mathrm{AlCl}_{3}(\mathrm{s})+\mathrm{H}_{2} \mathrm{O}(\mathrm{l})+\mathrm{N}_{2}(\mathrm{g}) $$ What is the minimum mass of \(\mathrm{NH}_{4} \mathrm{ClO}_{4}\) consumed, per kilogram of \(\mathrm{Al}\), by the reaction of \(\mathrm{NH}_{4} \mathrm{ClO}_{4}\) and Al?[Hint: Balance the elements in the order \(\mathrm{Cl}, \mathrm{H},\) \(\mathrm{O}, \mathrm{Al}, \mathrm{N} .\)]

A \(25.0 \mathrm{mL}\) sample of \(\mathrm{HCl}(\mathrm{aq})\) is diluted to a volume of 500.0 mL. If the concentration of the diluted solution is found to be \(0.085 \mathrm{M} \mathrm{HCl}\), what was the concentration of the original solution?

Appendix E describes a useful study aid known as concept mapping. Using the method presented in Appendix \(\mathrm{E},\) construct a concept map relating the topics found in Sections \(4-3,4-4,\) and \(4-5\).

A drop \((0.05 \mathrm{mL})\) of \(12.0 \mathrm{M} \mathrm{HCl}\) is spread over a sheet of thin aluminum foil. Assume that all the acid reacts with, and thus dissolves through, the foil. What will be the area, in \(\mathrm{cm}^{2}\), of the cylindrical hole produced? (Density of \(\mathrm{Al}=2.70 \mathrm{g} / \mathrm{cm}^{3} ;\) foil thickness \(=0.10 \mathrm{mm} .)\) \(2 \mathrm{Al}(\mathrm{s})+6 \mathrm{HCl}(\mathrm{aq}) \longrightarrow 2 \mathrm{AlCl}_{3}(\mathrm{aq})+3 \mathrm{H}_{2}(\mathrm{g})\)

Which has the higher concentration of sucrose: a \(46 \%\) sucrose solution by mass \((d=1.21 \mathrm{g} / \mathrm{mL}),\) or \(1.50 \mathrm{M}\) \(\mathrm{C}_{12} \mathrm{H}_{22} \mathrm{O}_{11}\) ? Explain your reasoning.
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