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Chapter 3: Problem 70

Arrange the following substances in order of increasing mass percent of carbon. a. caffeine, \(\mathrm{C}_{\mathrm{s}} \mathrm{H}_{10} \mathrm{~N}_{4} \mathrm{O}_{2}\) 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 increasing order of mass percent of carbon are: Sucrose (42.11%), Caffeine (49.48%), and Ethanol (53.31%).

Step by step solution

01

Calculate the molar mass of C, H, N, and O

First, we need to find the molar mass of each element present in the given substances. Carbon (C): 12.01 g/mol Hydrogen (H): 1.008 g/mol Nitrogen (N): 14.007 g/mol Oxygen (O): 16.00 g/mol
02

Calculate the molar mass of each substance

Now, let's find the molar mass of each substance using the molar masses of their constituent elements. a. Caffeine, C8H10N4O2: Molar mass = (8 × 12.01) + (10 × 1.008) + (4 × 14.007) + (2 × 16.00) = 96.08 + 10.08 + 56.028 + 32 = 194.188 g/mol b. Sucrose, C12H22O11: Molar mass = (12 × 12.01) + (22 × 1.008) + (11 × 16.00) = 144.12 + 22.176 + 176 = 342.296 g/mol c. Ethanol, C2H5OH: Molar mass = (2 × 12.01) + (5 × 1.008) + 16.00 = 24.02 + 5.04 + 16 = 45.06 g/mol
03

Calculate the mass percent of carbon in each substance

Next, we will find the mass percent of carbon in each substance. a. Caffeine: Mass percent of carbon = (Total mass of carbon / Molar mass of caffeine) × 100 = (96.08 / 194.188) × 100 = 49.48% b. Sucrose: Mass percent of carbon = (Total mass of carbon / Molar mass of sucrose) × 100 = (144.12 / 342.296) × 100 = 42.11% c. Ethanol: Mass percent of carbon = (Total mass of carbon / Molar mass of ethanol) × 100 = (24.02 / 45.06) × 100 = 53.31%
04

Arrange the substances in increasing order of mass percent of carbon

Now we will arrange the substances in increasing order of their mass percent of carbon. Sucrose (42.11%) < Caffeine (49.48%) < Ethanol (53.31%) So, the order of substances in increasing mass percent of carbon is Sucrose, Caffeine, and Ethanol.

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Most popular questions from this chapter

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?

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