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Answer :
To solve this problem, we need to determine how many grams of sulfur are formed when 37.4 grams of water are produced according to the given chemical reaction:
[tex]\[ 2 \text{H}_2\text{S} (g) + \text{SO}_2 (g) \rightarrow 3 \text{S} (s) + 2 \text{H}_2\text{O} (l) \][/tex]
Here's a step-by-step guide to solving the problem:
1. Calculate Moles of Water Formed:
- First, we need to find out how many moles of water (H[tex]\(_2\)[/tex]O) are represented by 37.4 grams.
- The molar mass of water is approximately 18.02 g/mol.
- To find the moles of water, divide the mass of water by its molar mass:
[tex]\[
\text{moles of H}_2\text{O} = \frac{37.4 \text{ g}}{18.02 \text{ g/mol}} = 2.075
\][/tex]
2. Use Stoichiometry to Find Moles of Sulfur Formed:
- According to the balanced equation, 2 moles of water are produced for every 3 moles of sulfur.
- We can use this ratio to find how many moles of sulfur are formed:
[tex]\[
\text{moles of S} = \frac{3}{2} \times \text{moles of H}_2\text{O} = \frac{3}{2} \times 2.075 = 3.113
\][/tex]
3. Convert Moles of Sulfur to Grams:
- The molar mass of sulfur (S) is approximately 32.07 g/mol.
- To find the mass of sulfur formed, multiply the moles of sulfur by its molar mass:
[tex]\[
\text{grams of S} = 3.113 \times 32.07 \text{ g/mol} = 99.8 \text{ g}
\][/tex]
Therefore, when 37.4 grams of water are formed, 99.8 grams of sulfur are produced. The correct answer is 99.8 g S.
[tex]\[ 2 \text{H}_2\text{S} (g) + \text{SO}_2 (g) \rightarrow 3 \text{S} (s) + 2 \text{H}_2\text{O} (l) \][/tex]
Here's a step-by-step guide to solving the problem:
1. Calculate Moles of Water Formed:
- First, we need to find out how many moles of water (H[tex]\(_2\)[/tex]O) are represented by 37.4 grams.
- The molar mass of water is approximately 18.02 g/mol.
- To find the moles of water, divide the mass of water by its molar mass:
[tex]\[
\text{moles of H}_2\text{O} = \frac{37.4 \text{ g}}{18.02 \text{ g/mol}} = 2.075
\][/tex]
2. Use Stoichiometry to Find Moles of Sulfur Formed:
- According to the balanced equation, 2 moles of water are produced for every 3 moles of sulfur.
- We can use this ratio to find how many moles of sulfur are formed:
[tex]\[
\text{moles of S} = \frac{3}{2} \times \text{moles of H}_2\text{O} = \frac{3}{2} \times 2.075 = 3.113
\][/tex]
3. Convert Moles of Sulfur to Grams:
- The molar mass of sulfur (S) is approximately 32.07 g/mol.
- To find the mass of sulfur formed, multiply the moles of sulfur by its molar mass:
[tex]\[
\text{grams of S} = 3.113 \times 32.07 \text{ g/mol} = 99.8 \text{ g}
\][/tex]
Therefore, when 37.4 grams of water are formed, 99.8 grams of sulfur are produced. The correct answer is 99.8 g S.
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