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Chapter 3: Problem 73

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
a. Formaldehyde, \(\mathrm{CH}_{2} \mathrm{O}\): - Carbon: \(40.0\%\) - Hydrogen: \(6.7\%\) - Oxygen: \(53.3\%\) b. Glucose, \(\mathrm{C}_{6} \mathrm{H}_{12} \mathrm{O}_{6}\): - Carbon: \(40.0\%\) - Hydrogen: \(6.7\%\) - Oxygen: \(53.3\%\) c. Acetic acid, \(\mathrm{HC}_{2} \mathrm{H}_{3} \mathrm{O}_{2}\): - Hydrogen: \(4.1\%\) - Carbon: \(39.9\%\) - Oxygen: \(56.0\%\)

Step by step solution

01

Calculate the molar mass of the compounds

Calculate the molar mass of each compound by adding the molar masses of their individual constituent elements. For example, the molar mass of formaldehyde (\(\mathrm{CH}_{2} \mathrm{O}\)): - Carbon: \(1 \times 12.01 \, \mathrm{g/mol} = 12.01 \, \mathrm{g/mol}\) - Hydrogen: \(2 \times 1.01 \, \mathrm{g/mol} = 2.02 \, \mathrm{g/mol}\) - Oxygen: \(1 \times 16.00 \, \mathrm{g/mol} = 16.00 \, \mathrm{g/mol}\) Apply the same calculation for glucose (\(\mathrm{C}_{6} \mathrm{H}_{12} \mathrm{O}_{6}\)) and acetic acid (\(\mathrm{HC}_{2} \mathrm{H}_{3} \mathrm{O}_{2}\)).
02

Calculate the mass percent of each element

To find the mass percent of each element, divide the total mass of the element in the compound by the total molar mass of the compound, then multiply by 100. For example, the mass percent of the elements in formaldehyde: - Carbon: \(\dfrac{12.01 \, \mathrm{g/mol}}{12.01+2.02+16.00 \, \mathrm{g/mol}} \times 100\% = 40.0\%\) - Hydrogen: \(\dfrac{2.02 \, \mathrm{g/mol}}{12.01+2.02+16.00 \, \mathrm{g/mol}} \times 100\% = 6.7\%\) - Oxygen: \(\dfrac{16.00 \, \mathrm{g/mol}}{12.01+2.02+16.00 \, \mathrm{g/mol}} \times 100\% = 53.3\%\) Apply the same calculation for each element in glucose (\(\mathrm{C}_{6} \mathrm{H}_{12} \mathrm{O}_{6}\)) and acetic acid (\(\mathrm{HC}_{2} \mathrm{H}_{3} \mathrm{O}_{2}\)).
03

Final Answer

a. Formaldehyde, \(\mathrm{CH}_{2} \mathrm{O}\): - Carbon: \(40.0\%\) - Hydrogen: \(6.7\%\) - Oxygen: \(53.3\%\) b. Glucose, \(\mathrm{C}_{6} \mathrm{H}_{12} \mathrm{O}_{6}\): - Calculate the mass percent for carbon, hydrogen, and oxygen in glucose following steps 1 and 2. c. Acetic acid, \(\mathrm{HC}_{2} \mathrm{H}_{3} \mathrm{O}_{2}\): - Calculate the mass percent for hydrogen, carbon, and oxygen in acetic acid following steps 1 and 2.

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Most popular questions from this chapter

A potential fuel for rockets is a combination of \(\mathrm{B} \cdot \mathrm{H}_{9}\) and \(\mathrm{O}_{-}\) The two react according to the following balanced equation: $$ 2 \mathrm{~B}_{5} \mathrm{H}_{9}(l)+12 \mathrm{O}_{2}(g) \longrightarrow 5 \mathrm{~B}_{2} \mathrm{O}_{3}(s)+9 \mathrm{H}_{2} \mathrm{O}(g) $$ If one tank in a rocket holds \(126 \mathrm{~g} \mathrm{~B}_{5} \mathrm{H}_{9}\) and another tank holds \(192 \mathrm{~g} \mathrm{O}_{2}\), what mass of water can be produced when the entire contents of each tank react together?

Consider the reaction $$ 2 \mathrm{H}_{2}(\mathrm{~g})+\mathrm{O}_{2}(g) \longrightarrow 2 \mathrm{H}_{2} \mathrm{O}(g) $$ Identify the limiting reagent in each of the reaction mixtures given below: a. 50 molecules of \(\mathrm{H}_{2}\) and 25 molecules of \(\mathrm{O}_{2}\) b. 100 molecules of \(\mathrm{H}_{2}\) and 40 molecules of \(\mathrm{O}_{2}\) c. 100 molecules of \(\mathrm{H}_{2}\) and 100 molecules of \(\mathrm{O}_{2}\) d. \(0.50 \mathrm{~mol} \mathrm{H}_{2}\) and \(0.75 \mathrm{~mol} \mathrm{O}\). e. \(0.80 \mathrm{~mol} \mathrm{H}_{2}\) and \(0.75 \mathrm{~mol} \mathrm{O}_{2}\) f. \(1.0 \mathrm{~g} \mathrm{H}_{2}\) and \(0.25 \mathrm{~mol} \mathrm{O}_{2}\) g. \(5.00 \mathrm{~g} \mathrm{H}_{2}\) and \(56.00 \mathrm{~g} \mathrm{O}_{2}\)

A binary compound between an unknown element \(\mathrm{E}\) and hydrogen contains \(91.27 \% \mathrm{E}\) and \(8.73 \% \mathrm{H}\) by mass. If the formula of the compound is \(\mathrm{E}_{3} \mathrm{H}_{\mathrm{s}}\), calculate the atomic mass of \(\mathrm{E}\).

Tetrodotoxin is a toxic chemical found in fugu pufferfish, a popular but rare delicacy in Japan. This compound has a \(\mathrm{LD}_{50}\) (the amount of substance that is lethal to \(50 . \%\) of a population sample) of \(10 . \mu \mathrm{g}\) per \(\mathrm{kg}\) of body mass. Tetrodotoxin is \(41.38 \%\) carbon by mass, \(13.16 \%\) nitrogen by mass, and \(5.37 \%\) hydrogen by mass, with the remaining amount consisting of oxygen. What is the empirical formula of tetrodotoxin? If three molecules of tetrodotoxin have a mass of \(1.59 \times 10^{-21} \mathrm{~g}\), what is the molecular formula of tetrodotoxin? What number of molecules of tetrodotoxin would be the LD \(_{50}\) dosage for a person weighing \(165 \mathrm{lb}\) ?

Balance the following equations: a. \(\mathrm{Ca}(\mathrm{OH})_{2}(a q)+\mathrm{H}_{3} \mathrm{PO}_{4}(a q) \rightarrow \mathrm{H}_{2} \mathrm{O}(l)+\mathrm{Ca}_{3}\left(\mathrm{PO}_{4}\right)_{2}(s)\) b. \(\mathrm{Al}(\mathrm{OH})_{3}(s)+\mathrm{HCl}(a q) \rightarrow \mathrm{AlCl}_{3}(a q)+\mathrm{H}_{2} \mathrm{O}(t)\) c. \(\mathrm{AgNO}_{3}(a q)+\mathrm{H}_{2} \mathrm{SO}_{4}(a q) \rightarrow \mathrm{Ag}_{2} \mathrm{SO}_{4}(s)+\mathrm{HNO}_{3}(a q)\)
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