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Chapter 3: Problem 67

Calculate the percent composition by mass of the following compounds that are important starting materials for synthetic polymers: a. \(\mathrm{C}_{3} \mathrm{H}_{4} \mathrm{O}_{2}\) (acrylic acid, from which acrylic plastics are made) b. \(\mathrm{C}_{4} \mathrm{H}_{6} \mathrm{O}_{2}\) (methyl acrylate, from which Plexiglas is made) c. \(\mathrm{C}_{3} \mathrm{H}_{3} \mathrm{~N}\) (acrylonitrile, from which Orlon is made)

Short Answer

Expert verified
The percent composition by mass of the given compounds are as follows: a. Acrylic acid (\(C_{3}H_{4}O_{2}\)): 50% carbon, 5.6% hydrogen, and 44.4% oxygen. b. Methyl acrylate (\(C_{4}H_{6}O_{2}\)): 55.8% carbon, 7.0% hydrogen, and 37.2% oxygen. c. Acrylonitrile (\(C_{3}H_{3}N\)): 67.9% carbon, 5.7% hydrogen, and 26.4% nitrogen.

Step by step solution

01

Determine the molar mass of the compound.

The molar mass is the sum of the atomic masses of the elements in the compound, weighted by the number of atoms of each element. The molar mass of carbon, hydrogen, and oxygen are approximately 12 g/mol, 1 g/mol, and 16 g/mol, respectively.\[Molar\:mass\:of\:C_{3}H_{4}O_{2}=(3\times12+4\times1+2\times16)g/mol=72\:g/mol\]
02

Calculate the mass of each element in the compound.

Now, we will multiply the atomic mass of each element by the number of moles of the element present in one mole of the compound. \[Mass\:of\:Carbon=3\times12=36\:g/mol\] \[Mass\:of\:Hydrogen=4\times1=4\:g/mol\] \[Mass\:of\:Oxygen=2\times16=32\:g/mol\]
03

Calculate the mass percent of each element.

We can now calculate the mass percent of each element by dividing the mass of the element by the molar mass of the compound and multiplying the result by 100. \[MassPercent_{Carbon}=\frac{36}{72}\times100=50\%\] \[MassPercent_{Hydrogen}=\frac{4}{72}\times100=5.6\%\] \[MassPercent_{Oxygen}=\frac{32}{72}\times100=44.4\%\] So, the percent composition by mass of acrylic acid is approximately 50% carbon, 5.6% hydrogen, and 44.4% oxygen. #Exercise b: C4H6O2 (methyl acrylate)#
04

Determine the molar mass of the compound.

\[Molar\:mass\:of\:C_{4}H_{6}O_{2}=(4\times12+6\times1+2\times16)g/mol=86\:g/mol\]
05

Calculate the mass of each element in the compound.

\[ Mass\:of\:Carbon=4\times12=48\:g/mol\] \[Mass\:of\:Hydrogen=6\times1=6\:g/mol\] \[Mass\:of\:Oxygen=2\times16=32\:g/mol\]
06

Calculate the mass percent of each element.

\[ MassPercent_{Carbon}=\frac{48}{86}\times100=55.8\%\] \[MassPercent_{Hydrogen}=\frac{6}{86}\times100=7.0\%\] \[MassPercent_{Oxygen}=\frac{32}{86}\times100=37.2\%\] So, the percent composition by mass of methyl acrylate is approximately 55.8% carbon, 7.0% hydrogen, and 37.2% oxygen. #Exercise c: C3H3N (acrylonitrile)#
07

Determine the molar mass of the compound.

The atomic mass of nitrogen is approximately 14 g/mol. \[Molar\:mass\:of\:C_{3}H_{3}N=(3\times12+3\times1+1\times14)g/mol=53\:g/mol\]
08

Calculate the mass of each element in the compound.

\[ Mass\:of\:Carbon=3\times12=36\:g/mol\] \[Mass\:of\:Hydrogen=3\times1=3\:g/mol\] \[Mass\:of\:Nitrogen=1\times14=14\:g/mol\]
09

Calculate the mass percent of each element.

\[ MassPercent_{Carbon}=\frac{36}{53}\times100=67.9\%\] \[MassPercent_{Hydrogen}=\frac{3}{53}\times100=5.7\%\] \[MassPercent_{Nitrogen}=\frac{14}{53}\times100=26.4\%\] So, the percent composition by mass of acrylonitrile is approximately 67.9% carbon, 5.7% hydrogen, and 26.4% nitrogen.

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Most popular questions from this chapter

Determine the molecular formula of a compound that contains \(26.7 \% \mathrm{P}, 12.1 \% \mathrm{~N}\), and \(61.2 \% \mathrm{Cl}\), and has a molar mass of \(580 \mathrm{~g} / \mathrm{mol}\).

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You take \(1.00 \mathrm{~g}\) of an aspirin tablet (a compound consisting solely of carbon, hydrogen, and oxygen), burn it in air, and collect \(2.20\) \(\mathrm{g} \mathrm{CO}_{2}\) and \(0.400 \mathrm{~g} \mathrm{H}_{2} \mathrm{O}\). You know that the molar mass of aspirin is between 170 and \(190 \mathrm{~g} / \mathrm{mol}\). Reacting 1 mole of salicylic acid with 1 mole of acetic anhydride \(\left(\mathrm{C}_{4} \mathrm{H}_{6} \mathrm{O}_{3}\right)\) gives you 1 mole of aspirin and 1 mole of acetic acid \(\left(\mathrm{C}_{2} \mathrm{H}_{4} \mathrm{O}_{2}\right)\). Use this information to determine the molecular formula of salicylic acid.

Bornite \(\left(\mathrm{Cu}_{3} \mathrm{FeS}_{3}\right)\) is a copper ore used in the production of copper. When heated, the following reaction occurs: $$ 2 \mathrm{Cu}_{3} \mathrm{FeS}_{3}(s)+7 \mathrm{O}_{2}(g) \longrightarrow 6 \mathrm{Cu}(s)+2 \mathrm{FeO}(s)+6 \mathrm{SO}_{2}(g) $$ If \(2.50\) metric tons of bornite is reacted with excess \(\mathrm{O}_{2}\) and the process has an \(86.3 \%\) yield of copper, what mass of copper is produced?
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