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Chapter 5: Problem 76

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, \(\mathrm{C}_{12} \mathrm{H}_{22} \mathrm{O}_{11}\) c. ethanol, \(\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{OH}\)

Short Answer

Expert verified
The substances arranged in order of increasing mass percent of carbon are: 1. Sucrose (\(\mathrm{C}_{12} \mathrm{H}_{22} \mathrm{O}_{11}\)): 42.11% carbon 2. Caffeine (\(\mathrm{C}_{8} \mathrm{H}_{10} \mathrm{N}_{4} \mathrm{O}_{2}\)): 49.48% carbon 3. Ethanol (\(\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{OH}\)): 52.17% carbon

Step by step solution

01

Calculate the molar mass of each substance

For this, we'll need the molar mass of each element (C, H, N, and O), which are approximately 12 g/mol, 1 g/mol, 14 g/mol, and 16 g/mol, respectively. a. Caffeine, \(\mathrm{C}_{8} \mathrm{H}_{10} \mathrm{N}_{4} \mathrm{O}_{2}\) Molar mass = (8 × 12) + (10 × 1) + (4 × 14) + (2 × 16) = 194 g/mol b. Sucrose, \(\mathrm{C}_{12} \mathrm{H}_{22} \mathrm{O}_{11}\) Molar mass = (12 × 12) + (22 × 1) + (11 × 16) = 342 g/mol c. Ethanol, \(\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{OH}\) Molar mass = (2 × 12) + (6 × 1) + (1 × 16) = 46 g/mol
02

Calculate the mass of carbon in each substance

Next, we will find the mass of carbon in each substance. a. Caffeine: 8 atoms of carbon, each with a mass of 12 g/mol, so the mass of carbon = 8 × 12 = 96 g/mol b. Sucrose: 12 atoms of carbon, each with a mass of 12 g/mol, so the mass of carbon = 12 × 12 = 144 g/mol c. Ethanol: 2 atoms of carbon, each with a mass of 12 g/mol, so the mass of carbon = 2 × 12 = 24 g/mol
03

Calculate the mass percent of carbon in each substance

Now, we can find the mass percent of carbon in each substance: a. Caffeine: (mass of carbon / molar mass) × 100 = (96 / 194) × 100 = 49.48% b. Sucrose: (mass of carbon / molar mass) × 100 = (144 / 342) × 100 = 42.11% c. Ethanol: (mass of carbon / molar mass) × 100 = (24 / 46) × 100 = 52.17%
04

Arrange the substances in increasing order of mass percent of carbon

Now that we have the mass percent of carbon for each substance, we can arrange them in increasing order: 1. Sucrose: 42.11% carbon 2. Caffeine: 49.48% carbon 3. Ethanol: 52.17% carbon

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Most popular questions from this chapter

An ionic compound \(\mathrm{MX}_{3}\) is prepared according to the following unbalanced chemical equation. $$\mathbf{M}+\mathbf{X}_{2} \longrightarrow \mathbf{M X}_{3}$$ A \(0.105-\mathrm{g}\) sample of \(\mathrm{X}_{2}\) contains \(8.92 \times 10^{20}\) molecules. The compound \(\mathrm{MX}_{3}\) consists of \(54.47 \%\) X by mass. What are the identities of \(\mathrm{M}\) and \(\mathrm{X}\), and what is the correct name for \(\mathrm{MX}_{3} ?\) Starting with 1.00 g each of \(M\) and \(X_{2}\), what mass of \(M X_{3}\) can be prepared?

Balance the following equations: a. \(\operatorname{Cr}(s)+\mathrm{S}_{8}(s) \rightarrow \mathrm{Cr}_{2} \mathrm{S}_{3}(s)\) b. \(\mathrm{NaHCO}_{3}(s) \stackrel{\text { Heat }}{\longrightarrow} \mathrm{Na}_{2} \mathrm{CO}_{3}(s)+\mathrm{CO}_{2}(g)+\mathrm{H}_{2} \mathrm{O}(g)\) c. \(\mathrm{KClO}_{3}(s) \stackrel{\text { Heat }}{\longrightarrow} \mathrm{KCl}(s)+\mathrm{O}_{2}(g)\) d. \(\mathrm{Eu}(s)+\mathrm{HF}(g) \rightarrow \mathrm{EuF}_{3}(s)+\mathrm{H}_{2}(g)\)

Acrylonitrile \(\left(\mathrm{C}_{3} \mathrm{H}_{3} \mathrm{N}\right)\) is the starting material for many synthetic carpets and fabrics. It is produced by the following reaction. $$2 \mathrm{C}_{3} \mathrm{H}_{6}(g)+2 \mathrm{NH}_{3}(g)+3 \mathrm{O}_{2}(g) \longrightarrow 2 \mathrm{C}_{3} \mathrm{H}_{3} \mathrm{N}(g)+6 \mathrm{H}_{2} \mathrm{O}(g)$$ If \(15.0 \mathrm{g}\) \(\mathrm{C}_{3} \mathrm{H}_{6}, 10.0 \mathrm{g} \mathrm{O}_{2},\) and \(5.00 \mathrm{g}\) \(\mathrm{NH}_{3}\) are reacted, what mass of acrylonitrile can be produced, assuming \(100 \%\) yield?

An element X forms both a dichloride (XCI_) and a tetrachloride \(\left(\mathrm{XCl}_{4}\right) .\) Treatment of \(10.00 \mathrm{g} \mathrm{XCl}_{2}\) with excess chlorine forms \(12.55 \mathrm{g} \mathrm{XCl}_{4} .\) Calculate the atomic mass of \(\mathrm{X},\) and identify \(\mathrm{X}\).

A gas contains a mixture of \(\mathrm{NH}_{3}(g)\) and \(\mathrm{N}_{2} \mathrm{H}_{4}(g),\) both of which react with \(\mathrm{O}_{2}(g)\) to form \(\mathrm{NO}_{2}(g)\) and \(\mathrm{H}_{2} \mathrm{O}(g) .\) The gaseous mixture (with an initial mass of \(61.00 \mathrm{g}\) ) is reacted with 10.00 moles \(\mathrm{O}_{2}\), and after the reaction is complete, 4.062 moles of \(\mathrm{O}_{2}\) remains. Calculate the mass percent of \(\mathrm{N}_{2} \mathrm{H}_{4}(g)\) in the original gaseous mixture.
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