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Chapter 3: Problem 40

Hexachlorophene, a compound made up of atoms of carbon, hydrogen, chlorine, and oxygen, is an ingredient in germicidal soaps. Combustion of a \(1.000-\mathrm{g}\) sample yields \(1.407 \mathrm{~g}\) of carbon dioxide, \(0.134 \mathrm{~g}\) of water, and \(0.523 \mathrm{~g}\) of chlorine gas. What are the mass percents of carbon, hydrogen, oxygen, and chlorine in hexachlorophene?

Short Answer

Expert verified
Answer: The mass percents of carbon, hydrogen, oxygen, and chlorine in hexachlorophene are approximately 38.396%, 1.4999%, 7.8041%, and 52.3%, respectively.

Step by step solution

01

Calculate the moles of CO₂, H₂O, and Cl₂ produced

To get started, we will use the masses of CO₂, H₂O, and Cl₂ produced to find the moles of each substance. We will use the molar mass of each compound to do this, which are: - CO₂: 12.01 g/mol (C) + 2 * 16.00 g/mol (O) = 44.01 g/mol - H₂O: 2 * 1.008 g/mol (H) + 16.00 g/mol (O) = 18.02 g/mol - Cl₂: 2 * 35.45 g/mol (Cl) = 70.90 g/mol Now, let's convert the masses to moles: - Moles of CO₂: (1.407 g) / (44.01 g/mol) = 0.03198 mol - Moles of H₂O: (0.134 g) / (18.02 g/mol) = 0.007442 mol - Moles of Cl₂: (0.523 g) / (70.90 g/mol) = 0.007372 mol
02

Convert moles to grams for each element

Next, we need to convert the moles of each substance to grams of individual elements: - Grams of C: (0.03198 mol) * (12.01 g/mol) = 0.38396 g - Grams of H: (0.007442 mol) * (2 * 1.008 g/mol) = 0.01499904 g - Grams of Cl: (0.007372 mol) * (2 * 35.45 g/mol) = 0.523 g Since we are given a 1.000 g sample and we've found the amount of three elements, we can find the amount of the remaining element, oxygen (O), by subtraction: - Grams of O: 1.000 g - (0.38396 g + 0.01499904 g + 0.523 g) = 0.07804096 g
03

Calculate the mass percents of each element

Finally, we can calculate the mass percent of each element in hexachlorophene by dividing the mass of each element by the total mass of the sample (1.000 g) and multiplying by 100. - Mass percent of C: (0.38396 g / 1.000 g) * 100 = 38.396% - Mass percent of H: (0.01499904 g / 1.000 g) * 100 = 1.4999% - Mass percent of Cl: (0.523 g / 1.000 g) * 100 = 52.3% - Mass percent of O: (0.07804096 g / 1.000 g) * 100 = 7.8041% Thus, the mass percents of carbon, hydrogen, oxygen, and chlorine in hexachlorophene are approximately 38.396%, 1.4999%, 7.8041%, and 52.3%, respectively.

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Most popular questions from this chapter

One way to remove nitrogen oxide (NO) from smoke stack emissions is to react it with ammonia. $$ 4 \mathrm{NH}_{3}(g)+6 \mathrm{NO}(g) \longrightarrow 5 \mathrm{~N}_{2}(g)+6 \mathrm{H}_{2} \mathrm{O}(l) $$ Calculate (a) the mass of water produced from \(0.839\) mol of ammonia. (b) the mass of NO required to react with \(3.402\) mol of ammonia. (c) the mass of ammonia required to produce \(12.0 \mathrm{~g}\) of nitrogen gas. (d) the mass of ammonia required to react with \(115 \mathrm{~g}\) of NO.

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