How many grams of sulfur are present in 1.24 moles of sulfur dioxide? The molar mass of sulfur dioxide is 64.066 g/mol, the molar mass of sulfur is 32.07g/mol
The Correct Answer and Explanation is :
To determine how many grams of sulfur are present in 1.24 moles of sulfur dioxide (SO₂), we can use stoichiometry, which involves converting moles to grams using the molar mass of sulfur.
Step-by-Step Solution:
- Write down the molar masses:
- Molar mass of sulfur dioxide (SO₂) = 64.066 g/mol
- Molar mass of sulfur (S) = 32.07 g/mol
- Understand the composition of sulfur dioxide (SO₂):
- The molecular formula for sulfur dioxide (SO₂) indicates that each molecule of SO₂ contains 1 atom of sulfur (S) and 2 atoms of oxygen (O).
- Therefore, each mole of sulfur dioxide contains 1 mole of sulfur atoms.
- Use the given moles of sulfur dioxide:
- We are given that there are 1.24 moles of sulfur dioxide. Since each mole of SO₂ contains 1 mole of sulfur, the number of moles of sulfur in 1.24 moles of SO₂ is also 1.24 moles.
- Convert moles of sulfur to grams:
- To convert moles of sulfur to grams, we multiply the number of moles of sulfur by the molar mass of sulfur (32.07 g/mol). [
\text{Mass of sulfur} = \text{moles of sulfur} \times \text{molar mass of sulfur}
]
[
\text{Mass of sulfur} = 1.24 \, \text{moles} \times 32.07 \, \text{g/mol}
]
[
\text{Mass of sulfur} = 39.7 \, \text{grams}
]
Final Answer:
The mass of sulfur in 1.24 moles of sulfur dioxide is 39.7 grams.
Explanation:
Sulfur dioxide (SO₂) consists of sulfur and oxygen. When calculating the mass of sulfur in a given amount of SO₂, we use the fact that each molecule of SO₂ contains one sulfur atom. Therefore, the number of moles of sulfur in any given sample of SO₂ will be equal to the number of moles of SO₂. By multiplying the number of moles of sulfur (1.24 moles) by the molar mass of sulfur (32.07 g/mol), we obtain the mass of sulfur in grams. This calculation assumes that all sulfur in SO₂ is accounted for and that no other compounds are present.