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Answer :
To determine the percent composition of sulfur in sulfuric acid, [tex]\(H_2SO_4\)[/tex], we follow these steps:
1. First, note the atomic masses of the elements:
- Hydrogen: [tex]\(1.008\, \text{g/mol}\)[/tex]
- Sulfur: [tex]\(32.06\, \text{g/mol}\)[/tex]
- Oxygen: [tex]\(16.00\, \text{g/mol}\)[/tex]
2. Next, calculate the total mass contributed by each element in one mole of [tex]\(H_2SO_4\)[/tex]:
- Hydrogen: There are 2 hydrogen atoms, so:
[tex]$$\text{Mass of H} = 2 \times 1.008 = 2.016\, \text{g/mol}$$[/tex]
- Sulfur: There is 1 sulfur atom:
[tex]$$\text{Mass of S} = 1 \times 32.06 = 32.06\, \text{g/mol}$$[/tex]
- Oxygen: There are 4 oxygen atoms:
[tex]$$\text{Mass of O} = 4 \times 16.00 = 64.00\, \text{g/mol}$$[/tex]
3. Now, find the total molar mass of [tex]\(H_2SO_4\)[/tex]:
[tex]$$\text{Total molar mass} = 2.016 + 32.06 + 64.00 = 98.076\, \text{g/mol}$$[/tex]
4. Finally, calculate the percent composition of sulfur:
[tex]$$\text{Percent of S} = \left(\frac{32.06}{98.076}\right) \times 100 \approx 32.688935\%$$[/tex]
Rounding this to one decimal place, we get approximately [tex]\(32.7\%\)[/tex].
Thus, the best answer is:
[tex]$$\textbf{C. } 32.7\%$$[/tex]
1. First, note the atomic masses of the elements:
- Hydrogen: [tex]\(1.008\, \text{g/mol}\)[/tex]
- Sulfur: [tex]\(32.06\, \text{g/mol}\)[/tex]
- Oxygen: [tex]\(16.00\, \text{g/mol}\)[/tex]
2. Next, calculate the total mass contributed by each element in one mole of [tex]\(H_2SO_4\)[/tex]:
- Hydrogen: There are 2 hydrogen atoms, so:
[tex]$$\text{Mass of H} = 2 \times 1.008 = 2.016\, \text{g/mol}$$[/tex]
- Sulfur: There is 1 sulfur atom:
[tex]$$\text{Mass of S} = 1 \times 32.06 = 32.06\, \text{g/mol}$$[/tex]
- Oxygen: There are 4 oxygen atoms:
[tex]$$\text{Mass of O} = 4 \times 16.00 = 64.00\, \text{g/mol}$$[/tex]
3. Now, find the total molar mass of [tex]\(H_2SO_4\)[/tex]:
[tex]$$\text{Total molar mass} = 2.016 + 32.06 + 64.00 = 98.076\, \text{g/mol}$$[/tex]
4. Finally, calculate the percent composition of sulfur:
[tex]$$\text{Percent of S} = \left(\frac{32.06}{98.076}\right) \times 100 \approx 32.688935\%$$[/tex]
Rounding this to one decimal place, we get approximately [tex]\(32.7\%\)[/tex].
Thus, the best answer is:
[tex]$$\textbf{C. } 32.7\%$$[/tex]
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