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Chapter 4: Problem 114

The manufacture of ethyl alcohol, \(\mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{OH}\) yields diethyl ether, \(\left(\mathrm{C}_{2} \mathrm{H}_{5}\right)_{2} \mathrm{O}\) as a by-product. The complete combustion of a \(1.005 \mathrm{g}\) sample of the product of this process yields \(1.963 \mathrm{g} \mathrm{CO}_{2} .\) What must be the mass percents of \(\left(\mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{OH}\right),\) and of \(\left(\mathrm{C}_{2} \mathrm{H}_{5}\right)_{2} \mathrm{O}\) in this sample?

Short Answer

Expert verified
The mass percents of \(CH_3CH_2OH\) and \((C_2H_5)_2O\) in the given sample should be equivalent to the carbon mass percentage in the sample, calculated by using the mass of carbon obtained from the combustion process.

Step by step solution

01

Calculate moles of carbon from obtained carbon dioxide

The mass of carbon dioxide obtained is \(1.963 g\). The molar mass of carbon dioxide is \(\(44.01 g/mol \)\). By dividing the mass of carbon dioxide by its molar mass, the number of moles of carbon can be calculated using the equation: \(\number of moles = mass/molar mass\)
02

Calculate mass of carbon in the original sample

The obtained moles in Step 1 are the moles of carbon in the sample. Since every mole of carbon has a mass of \(12 g\), the mass of carbon in the original sample can be determined by multiplying the moles of carbon obtained in Step 1 by \(12 g/mol\)
03

Calculate the mass percent of ethyl alcohol and diethyl ether

Essentially, both ethyl alcohol (\(CH_3CH_2OH\)) and diethyl ether (\((C_2H_5)_2O\)) have the same proportion of carbon. Hence, the carbon mass percentage in the original sample should be equal to the carbon mass percentage in each compound. The mass percentage can be calculated by dividing the mass of carbon in the original sample by the total mass of the sample, then multiplied by 100. Mass percentages of both compounds in the sample can thus be obtained.

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Most popular questions from this chapter

How much (a) glucose, \(\mathrm{C}_{6} \mathrm{H}_{12} \mathrm{O}_{6},\) in grams, must be dissolved in water to produce \(75.0 \mathrm{mL}\) of \(0.350 \mathrm{M} \mathrm{C}_{6} \mathrm{H}_{12} \mathrm{O}_{6} ?\) (b) methanol, \(\mathrm{CH}_{3} \mathrm{OH} \quad(d=0.792 \mathrm{g} / \mathrm{mL}),\) in milli- liters, must be dissolved in water to produce 2.25 L of \(0.485 \mathrm{M} \mathrm{CH}_{3} \mathrm{OH} ?\)

The incomplete combustion of gasoline produces \(\mathrm{CO}(\mathrm{g})\) as well as \(\mathrm{CO}_{2}(\mathrm{g}) .\) Write an equation for \((\mathrm{a})\) the complete combustion of the gasoline component octane, \(\mathrm{C}_{8} \mathrm{H}_{18}(\mathrm{l}),\) and \((\mathrm{b})\) incomplete combustion of octane with \(25 \%\) of the carbon appearing as \(\mathrm{CO}(\mathrm{g})\)

What are the molarities of the following solutes? (a) sucrose \(\left(\mathrm{C}_{12} \mathrm{H}_{22} \mathrm{O}_{11}\right)\) if \(150.0 \mathrm{g}\) is dissolved per \(250.0 \mathrm{mL}\) of water solution (b) urea, \(\mathrm{CO}\left(\mathrm{NH}_{2}\right)_{2},\) if \(98.3 \mathrm{mg}\) of the \(97.9 \%\) pure solid is dissolved in \(5.00 \mathrm{mL}\) of aqueous solution (c) methanol, \(\mathrm{CH}_{3} \mathrm{OH},(d=0.792 \mathrm{g} / \mathrm{mL})\) if \(125.0 \mathrm{mL}\) is dissolved in enough water to make 15.0 L of solution

A 0.696 mol sample of \(\mathrm{Cu}\) is added to \(136 \mathrm{mL}\) of \(6.0 \mathrm{M}\) HNO \(_{3}\). Assuming the following reaction is the only one that occurs, will the Cu react completely? $$\begin{aligned} 3 \mathrm{Cu}(\mathrm{s})+8 \mathrm{HNO}_{3}(\mathrm{aq}) & \longrightarrow 3 \mathrm{Cu}\left(\mathrm{NO}_{3}\right)_{2}(\mathrm{aq}) +4 \mathrm{H}_{2} \mathrm{O}(\mathrm{l})+2 \mathrm{NO}(\mathrm{g}) \end{aligned}$$

Cryolite, \(\mathrm{Na}_{3} \mathrm{AlF}_{6^{\prime}}\) is an important industrial reagent. It is made by the reaction below. $$\begin{array}{r} \mathrm{Al}_{2} \mathrm{O}_{3}(\mathrm{s})+6 \mathrm{NaOH}(\mathrm{aq})+12 \mathrm{HF}(\mathrm{g}) \longrightarrow 2 \mathrm{Na}_{3} \mathrm{AlF}_{6}(\mathrm{s})+9 \mathrm{H}_{2} \mathrm{O}(\mathrm{l}) \end{array}$$ In an experiment, \(7.81 \mathrm{g} \mathrm{Al}_{2} \mathrm{O}_{3}\) and excess \(\mathrm{HF}(\mathrm{g})\) were dissolved in 3.50 L of 0.141 M NaOH. If 28.2 g \(\mathrm{Na}_{3} \mathrm{AlF}_{6}\) was obtained, then what is the percent yield for this experiment?
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