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Chapter 3: Problem 120

Anabolic steroids are performance enhancement drugs whose use has been banned from most major sporting activities. One anabolic steroid is fluoxymesterone \(\left(\mathrm{C}_{20} \mathrm{H}_{29} \mathrm{FO}_{3}\right) .\) Calculate the percent composition by mass of fluoxymesterone.

Short Answer

Expert verified
The percent composition by mass of fluoxymesterone (C20H29FO3) is approximately 71.38% carbon, 8.70% hydrogen, 5.65% fluorine, and 14.27% oxygen.

Step by step solution

01

Find the molar mass of fluoxymesterone

To determine the molar mass of fluoxymesterone (C20H29FO3), we need to find the total mass of all the atoms in one mole of the compound. We can do this by multiplying the number of each atom by its molar mass: - For carbon (C), the molar mass is 12.01 g/mol. - For hydrogen (H), the molar mass is 1.01 g/mol. - For fluorine (F), the molar mass is 19 g/mol. - For oxygen (O), the molar mass is 16 g/mol. Molar mass of fluoxymesterone: = (20 * 12.01) + (29 * 1.01) + (1 * 19) + (3 * 16) = 240.2 + 29.29 + 19 + 48 = 336.49 g/mol
02

Find the individual masses of elements in fluoxymesterone

To find the mass of each element in fluoxymesterone, we multiply the number of atoms of the element with their respective molar mass. Mass of carbon (C) = 20 * 12.01 g/mol = 240.2 g/mol Mass of hydrogen (H) = 29 * 1.01 g/mol = 29.29 g/mol Mass of fluorine (F) = 1 * 19 g/mol = 19 g/mol Mass of oxygen (O) = 3 * 16 g/mol = 48 g/mol
03

Calculate the percent composition by mass of each element

To find the percent composition by mass of each element in fluoxymesterone, we divide the mass of each element by the molar mass of the compound and multiply by 100. Percent composition of carbon (C) = (240.2 g/mol) / (336.49 g/mol) * 100 = 71.38% Percent composition of hydrogen (H) = (29.29 g/mol) / (336.49 g/mol) * 100 = 8.70% Percent composition of fluorine (F) = (19 g/mol) / (336.49 g/mol) * 100 = 5.65% Percent composition of oxygen (O) = (48 g/mol) / (336.49 g/mol) * 100 = 14.27% Thus, the percent composition by mass of fluoxymesterone (C20H29FO3) is approximately 71.38% carbon, 8.70% hydrogen, 5.65% fluorine, and 14.27% oxygen.

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Most popular questions from this chapter

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?

Coke is an impure form of carbon that is often used in the industrial production of metals from their oxides. If a sample of coke is \(95 \%\) carbon by mass, determine the mass of coke needed to react completely with \(1.0\) ton of copper(II) oxide. $$ 2 \mathrm{CuO}(s)+\mathrm{C}(s) \longrightarrow 2 \mathrm{Cu}(s)+\mathrm{CO}_{2}(g) $$

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

Bornite \(\left(\mathrm{Cu}_{3} \mathrm{FeS}_{3}\right)\) is a copper ore used in the production of copper. When heated, the following reaction occurs: $$ 2 \mathrm{Cu}_{3} \mathrm{FeS}_{3}(s)+7 \mathrm{O}_{2}(g) \longrightarrow 6 \mathrm{Cu}(s)+2 \mathrm{FeO}(s)+6 \mathrm{SO}_{2}(g) $$ If \(2.50\) metric tons of bornite is reacted with excess \(\mathrm{O}_{2}\) and the process has an \(86.3 \%\) yield of copper, what mass of copper is produced?

A \(2.077-g\) sample of an element, which has an atomic mass between 40 and 55 , reacts with oxygen to form \(3.708 \mathrm{~g}\) of an oxide. Determine the formula of the oxide (and identify the element).
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