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Chapter 3: Problem 79

Express the composition of each of the following compounds as the mass percents of its elements. a. formaldehyde, \(\mathrm{CH}_{2} \mathrm{O}\) b. glucose, \(\mathrm{C}_{6} \mathrm{H}_{12} \mathrm{O}_{6}\) c. acetic acid, \(\mathrm{HC}_{2} \mathrm{H}_{3} \mathrm{O}_{2}\)

Short Answer

Expert verified
The mass percentages of each element in the compounds are: a. Formaldehyde, \(\mathrm{CH}_{2} \mathrm{O}\): C: 39.97%, H: 6.73%, O: 53.30% b. Glucose, \(\mathrm{C}_{6} \mathrm{H}_{12} \mathrm{O}_{6}\): C: 39.99%, H: 6.71%, O: 53.30% c. Acetic acid, \(\mathrm{HC}_{2} \mathrm{H}_{3} \mathrm{O}_{2}\): C: 40.00%, H: 6.68%, O: 53.32%

Step by step solution

01

Find the molar mass of each component

For C: 12.01 g/mol, for H: 1.01 g/mol, for O: 16.00 g/mol.
02

Calculate the molar mass of the whole compound

Molar mass of formaldehyde is: 12.01 g/mol + 2 x 1.01 g/mol + 16.00 g/mol = 30.03 g/mol.
03

Calculate the mass percentages of each element in the compound

C: \(\frac{12.01}{30.03}\) x 100% = 39.97% H: \(\frac{2 \times 1.01}{30.03}\) x 100% = 6.73% O: \(\frac{16.00}{30.03}\) x 100% = 53.30% b. Glucose, \(\mathrm{C}_{6} \mathrm{H}_{12} \mathrm{O}_{6}\)
04

Find the molar mass of each component

For C: 12.01 g/mol, for H: 1.01 g/mol, for O: 16.00 g/mol.
05

Calculate the molar mass of the whole compound

Molar mass of glucose is: 6 x 12.01 g/mol + 12 x 1.01 g/mol + 6 x 16.00 g/mol = 180.18 g/mol.
06

Calculate the mass percentages of each element in the compound

C: \(\frac{6 \times 12.01}{180.18}\) x 100% = 39.99% H: \(\frac{12 \times 1.01}{180.18}\) x 100% = 6.71% O: \(\frac{6 \times 16.00}{180.18}\) x 100% = 53.30% c. Acetic acid, \(\mathrm{HC}_{2} \mathrm{H}_{3} \mathrm{O}_{2}\)
07

Find the molar mass of each component

For C: 12.01 g/mol, for H: 1.01 g/mol, for O: 16.00 g/mol.
08

Calculate the molar mass of the whole compound

Molar mass of acetic acid is: 1.01 g/mol + 2 x 12.01 g/mol + 3 x 1.01 g/mol + 2 x 16.00 g/mol = 60.05 g/mol.
09

Calculate the mass percentages of each element in the compound

C: \(\frac{2 \times 12.01}{60.05}\) x 100% = 40.00% H: \(\frac{1.01 + 3 \times 1.01}{60.05}\) x 100% = 6.68% O: \(\frac{2 \times 16.00}{60.05}\) x 100% = 53.32%

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Most popular questions from this chapter

Methane \(\left(\mathrm{CH}_{4}\right)\) is the main component of marsh gas. Heating methane in the presence of sulfur produces carbon disulfide and hydrogen sulfide as the only products. a. Write the balanced chemical equation for the reaction of methane and sulfur. b. Calculate the theoretical yield of carbon disulfide when 120\. g of methane is reacted with an equal mass of sulfur.

Which of the following statements about chemical equations is(are) true? a. When balancing a chemical equation, you can never change the coefficient in front of any chemical formula. b. The coefficients in a balanced chemical equation refer to the number of grams of reactants and products. c. In a chemical equation, the reactants are on the right and the products are on the left. d. When balancing a chemical equation, you can never change the subscripts of any chemical formula. e. In chemical reactions, matter is neither created nor destroyed so a chemical equation must have the same number of atoms on both sides of the equation.

Bacterial digestion is an economical method of sewage treatment. The reaction \(5 \mathrm{CO}_{2}(g)+55 \mathrm{NH}_{4}^{+}(a q)+76 \mathrm{O}_{2}(g) \stackrel{\text { hacteria }}{\longrightarrow}\) \(\mathrm{C}_{3} \mathrm{H}_{7} \mathrm{O}_{2} \mathrm{~N}(s)+54 \mathrm{NO}_{2}^{-}(a q)+52 \mathrm{H}_{2} \mathrm{O}(t)+109 \mathrm{H}^{+}(a q)\) bacterial tissue is an intermediate step in the conversion of the nitrogen in organic compounds into nitrate ions. What mass of bacterial tissue is produced in a treatment plant for every \(1.0 \times 10^{4} \mathrm{~kg}\) of wastewater containing \(3.0 \% \mathrm{NH}_{4}{ }^{+}\) ions by mass? Assume that \(95 \%\) of the ammonium ions are consumed by the bacteria.

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The empirical formula of styrene is \(\mathrm{CH} ;\) the molar mass of styrene is \(104.14 \mathrm{~g} / \mathrm{mol}\). What number of \(\mathrm{H}\) atoms are present in a \(2.00-g\) sample of styrene?
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