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Chapter 4: Problem 8

Write balanced equations to represent the complete combustion of each of the following in excess oxygen: (a) propylene, \(\mathrm{C}_{3} \mathrm{H}_{6} ;\) (b) thiobenzoic acid, \(\mathrm{C}_{6} \mathrm{H}_{5} \mathrm{COSH}\) (c) glycerol, \(\mathrm{CH}_{2}(\mathrm{OH}) \mathrm{CH}(\mathrm{OH}) \mathrm{CH}_{2} \mathrm{OH}\)

Short Answer

Expert verified
The balanced equations for the combustion of propylene, thiobenzoic acid, and glycerol are: \(\mathrm{C}_{3} \mathrm{H}_{6} + 5\mathrm{O}_{2} \rightarrow 3\mathrm{CO}_{2} + 3\mathrm{H}_{2}\mathrm{O}\), \(\mathrm{C}_{6} \mathrm{H}_{5} \mathrm{COSH} + 8\mathrm{O}_{2} \rightarrow 7\mathrm{CO}_{2} + 3\mathrm{H}_{2}\mathrm{O} + \mathrm{SO}_{2}\), and \(\mathrm{CH}_{2}(\mathrm{OH}) \mathrm{CH}(\mathrm{OH}) \mathrm{CH}_{2} \mathrm{OH} + 5\mathrm{O}_{2} \rightarrow 3\mathrm{CO}_{2} + 4\mathrm{H}_{2}\mathrm{O}\) respectively.

Step by step solution

01

Combustion of Propylene

Propylene \(\mathrm{C}_{3} \mathrm{H}_{6}\) reacts with oxygen \(\mathrm{O}_{2}\) to produce carbon dioxide \(\mathrm{CO}_{2}\) and water \(\mathrm{H}_{2}\mathrm{O}\). The unbalanced equation is: \(\mathrm{C}_{3} \mathrm{H}_{6} + \mathrm{O}_{2} \rightarrow \mathrm{CO}_{2} + \mathrm{H}_{2}\mathrm{O}\). Balancing, we obtain: \(\mathrm{C}_{3} \mathrm{H}_{6} + 5\mathrm{O}_{2} \rightarrow 3\mathrm{CO}_{2} + 3\mathrm{H}_{2}\mathrm{O}\)
02

Combustion of Thiobenzoic Acid

Thiobenzoic Acid \(\mathrm{C}_{6} \mathrm{H}_{5} \mathrm{COSH}\) will also react with \(\mathrm{O}_{2}\) to produce carbon dioxide \(\mathrm{CO}_{2}\), water \(\mathrm{H}_{2}\mathrm{O}\) and sulfur \(\mathrm{SO}_{2}\). The unbalanced equation is: \(\mathrm{C}_{6} \mathrm{H}_{5} \mathrm{COSH} + \mathrm{O}_{2} \rightarrow \mathrm{CO}_{2} + \mathrm{H}_{2}\mathrm{O} + \mathrm{SO}_{2}\). After balancing, the equation becomes: \(\mathrm{C}_{6} \mathrm{H}_{5} \mathrm{COSH} + 8\mathrm{O}_{2} \rightarrow 7\mathrm{CO}_{2} + 3\mathrm{H}_{2}\mathrm{O} + \mathrm{SO}_{2}\)
03

Combustion of Glycerol

Glycerol \(\mathrm{CH}_{2}(\mathrm{OH}) \mathrm{CH}(\mathrm{OH}) \mathrm{CH}_{2} \mathrm{OH}\) reacts with \(\mathrm{O}_{2}\) to produce \(\mathrm{CO}_{2}\) and \(\mathrm{H}_{2}\mathrm{O}\). The unbalanced equation is: \(\mathrm{CH}_{2}(\mathrm{OH}) \mathrm{CH}(\mathrm{OH}) \mathrm{CH}_{2} \mathrm{OH} + \mathrm{O}_{2} \rightarrow \mathrm{CO}_{2} + \mathrm{H}_{2}\mathrm{O}\). After balancing, this becomes: \(\mathrm{CH}_{2}(\mathrm{OH}) \mathrm{CH}(\mathrm{OH}) \mathrm{CH}_{2} \mathrm{OH} + 5\mathrm{O}_{2} \rightarrow 3\mathrm{CO}_{2} + 4\mathrm{H}_{2}\mathrm{O}\)

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Most popular questions from this chapter

Write a chemical equation to represent the complete combustion of malonic acid, a compound with \(34.62 \% \mathrm{C}, 3.88 \% \mathrm{H},\) and \(61.50 \% \mathrm{O},\) by mass.

An organic liquid is either methyl alcohol \(\left(\mathrm{CH}_{3} \mathrm{OH}\right)\) ethyl alcohol \(\left(\mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{OH}\right),\) or a mixture of the two. A 0.220-g sample of the liquid is burned in an excess of \(\mathrm{O}_{2}(\mathrm{g})\) and yields \(0.352 \mathrm{g} \mathrm{CO}_{2}(\mathrm{g}) .\) Is the liquid a pure alcohol or a mixture of the two?

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Which of the following is a \(0.500 \mathrm{M} \mathrm{KCl}\) solution? (a) \(0.500 \mathrm{g} \mathrm{KCl} / \mathrm{mL}\) solution; (b) \(36.0 \mathrm{g} \mathrm{KCl} / \mathrm{L}\) solu- tion; (c) 7.46 mg KCl/mL solution; (d) 373 g KCl in 10.00 L solution

To prepare a solution that is \(0.50 \mathrm{M} \mathrm{KCl}\) starting with \(100.0 \mathrm{mL}\) of \(0.40 \mathrm{M} \mathrm{KCl},\) you should \((\mathrm{a})\) add \(20.0 \mathrm{mL}\) of water; (b) add 0.075 g KCl; (c) add 0.10 mol KCl; (d) evaporate \(20.0 \mathrm{mL}\) of water.
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