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Chapter 3: Problem 73

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 compositions by mass for the compounds are: a. Acrylic Acid: \(50.00\% \ \mathrm{C}, 5.58\% \ \mathrm{H}, 44.42\% \ \mathrm{O}\) b. Methyl Acrylate: \(55.82\% \ \mathrm{C}, 7.03\% \ \mathrm{H}, 37.15\% \ \mathrm{O}\) c. Acrylonitrile: \(67.76\% \ \mathrm{C}, 5.70\% \ \mathrm{H}, 26.54\% \ \mathrm{N}\)

Step by step solution

01

Find the molar mass of \(\mathrm{C}_{3} \mathrm{H}_{4} \mathrm{O}_{2}\)

From the periodic table, the atomic masses of Carbon, Hydrogen, and Oxygen are \(12.01\,\text{g/mol}\), \(1.01\,\text{g/mol}\), and \(16.00\,\text{g/mol}\), respectively. The molar mass of \(\mathrm{C}_{3} \mathrm{H}_{4} \mathrm{O}_{2}\) is: \[3(12.01)+4(1.01)+2(16.00)=72.06\,\text{g/mol}\]
02

Find the percent composition by mass of each element

To find the percent composition by mass of each element, divide the mass contribution of each element by the total molar mass and multiply by 100. Carbon: \(\frac{3(12.01)}{72.06} \times 100 = 50.00\%\) Hydrogen: \(\frac{4(1.01)}{72.06} \times 100 = 5.58\%\) Oxygen: \(\frac{2(16.00)}{72.06} \times 100 = 44.42\%\) Acrylic Acid Percent Composition: \(50.00\% \ \mathrm{C}, 5.58\% \ \mathrm{H}, 44.42\% \ \mathrm{O}\) b. Methyl Acrylate:
03

Find the molar mass of \(\mathrm{C}_{4} \mathrm{H}_{6} \mathrm{O}_{2}\)

The molar mass of \(\mathrm{C}_{4} \mathrm{H}_{6} \mathrm{O}_{2}\) is: \[4(12.01)+6(1.01)+2(16.00)=86.08\,\text{g/mol}\]
04

Find the percent composition by mass of each element

To find the percent composition by mass of each element, divide the mass contribution of each element by the total molar mass and multiply by 100. Carbon: \(\frac{4(12.01)}{86.08} \times 100 = 55.82\%\) Hydrogen: \(\frac{6(1.01)}{86.08} \times 100 = 7.03\%\) Oxygen: \(\frac{2(16.00)}{86.08} \times 100 = 37.15\%\) Methyl Acrylate Percent Composition: \(55.82\% \ \mathrm{C}, 7.03\% \ \mathrm{H}, 37.15\% \ \mathrm{O}\) c. Acrylonitrile:
05

Find the molar mass of \(\mathrm{C}_{3} \mathrm{H}_{3} \mathrm{N}\)

From the periodic table, the atomic mass of Nitrogen is \(14.01\,\text{g/mol}\). The molar mass of \(\mathrm{C}_{3} \mathrm{H}_{3} \mathrm{N}\) is: \[3(12.01)+3(1.01)+1(14.01)=53.08\,\text{g/mol}\]
06

Find the percent composition by mass of each element

To find the percent composition by mass of each element, divide the mass contribution of each element by the total molar mass and multiply by 100. Carbon: \(\frac{3(12.01)}{53.08} \times 100 = 67.76\%\) Hydrogen: \(\frac{3(1.01)}{53.08} \times 100 = 5.70\%\) Nitrogen: \(\frac{1(14.01)}{53.08} \times 100 = 26.54\%\) Acrylonitrile Percent Composition: \(67.76\% \ \mathrm{C}, 5.70\% \ \mathrm{H}, 26.54\% \ \mathrm{N}\)

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Most popular questions from this chapter

Arrange the following substances in order of increasing mass percent of carbon. a. caffeine, \(\mathrm{C}_{8} \mathrm{H}_{10} \mathrm{~N}_{4} \mathrm{O}_{2}\) b. sucrose, \(\bar{C}_{12} \mathrm{H}_{22} \mathrm{O}_{11}\) c. ethanol, \(\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{OH}\)

Ammonia reacts with \(\mathrm{O}_{2}\) to form either \(\mathrm{NO}(g)\) or \(\mathrm{NO}_{2}(g) \mathrm{ac}-\) cording to these unbalanced equations: $$ \begin{array}{l} \mathrm{NH}_{3}(g)+\mathrm{O}_{2}(g) \longrightarrow \mathrm{NO}(g)+\mathrm{H}_{2} \mathrm{O}(g) \\ \mathrm{NH}_{3}(g)+\mathrm{O}_{2}(g) \longrightarrow \mathrm{NO}_{2}(g)+\mathrm{H}_{2} \mathrm{O}(g) \end{array} $$ In a certain experiment \(2.00\) moles of \(\mathrm{NH}_{3}(g)\) and \(10.00 \mathrm{moles}\) of \(\mathrm{O}_{2}(g)\) are contained in a closed flask. After the reaction is complete, \(6.75\) moles of \(\mathrm{O}_{2}(g)\) remains. Calculate the number of moles of \(\mathrm{NO}(g)\) in the product mixture: (Hint: You cannot do this problem by adding the balanced equations because you cannot assume that the two reactions will occur with equal probability.)

A \(0.4230-\mathrm{g}\) sample of impure sodium nitrate was heated, converting all the sodium nitrate to \(0.2864 \mathrm{~g}\) of sodium nitrite and oxygen gas. Determine the percent of sodium nitrate in the oriainal sample.

Over the years, the thermite reaction has been used for welding railroad rails, in incendiary bombs, and to ignite solid-fuel rocket motors. The reaction is $$ \mathrm{Fe}_{2} \mathrm{O}_{3}(s)+2 \mathrm{Al}(s) \longrightarrow 2 \mathrm{Fe}(l)+\mathrm{Al}_{2} \mathrm{O}_{3}(s) $$ What masses of iron(III) oxide and aluminum must be used to produce \(15.0 \mathrm{~g}\) iron? What is the maximum mass of aluminum oxide that could be produced?

Vitamin A has a molar mass of \(286.4 \mathrm{~g} / \mathrm{mol}\) and a general molecular formula of \(\mathrm{C}_{x} \mathrm{H}_{2} \mathrm{E}\), where \(\mathrm{E}\) is an unknown element. If vitamin \(\mathrm{A}\) is \(83.86 \% \mathrm{C}\) and \(10.56 \% \mathrm{H}\) by mass, what is the molecular formula of vitamin \(\mathrm{A}\) ?
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