Thank you for visiting According to the following reaction how many grams of sulfur are formed when 37 4 g of water are produced 2 H 2 S g. This page is designed to guide you through key points and clear explanations related to the topic at hand. We aim to make your learning experience smooth, insightful, and informative. Dive in and discover the answers you're looking for!
Answer :
To find out how many grams of sulfur are formed when 37.4 grams of water are produced, we can use the stoichiometry of the 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]
Step 1: Calculate the moles of water
First, we need to determine the number of moles of water (Hâ‚‚O) formed. The molar mass of water is approximately 18.015 grams per mole.
[tex]\[
\text{Moles of H}_2\text{O} = \frac{\text{Mass of H}_2\text{O}}{\text{Molar mass of H}_2\text{O}} = \frac{37.4 \, \text{g}}{18.015 \, \text{g/mol}} \approx 2.076 \, \text{moles}
\][/tex]
Step 2: Use stoichiometry to find the moles of sulfur
From the balanced equation, we see that 2 moles of Hâ‚‚O are produced for every 3 moles of sulfur (S) formed. Therefore, the moles of sulfur that are formed are calculated as follows:
[tex]\[
\text{Moles of S} = \left(\frac{3 \, \text{moles of S}}{2 \, \text{moles of H}_2\text{O}}\right) \times 2.076 \, \text{moles of H}_2\text{O} \approx 3.114 \, \text{moles}
\][/tex]
Step 3: Calculate the mass of sulfur
Finally, we convert the moles of sulfur to grams using the molar mass of sulfur, which is approximately 32.06 grams per mole:
[tex]\[
\text{Mass of S} = \text{Moles of S} \times \text{Molar mass of S} = 3.114 \, \text{moles} \times 32.06 \, \text{g/mol} \approx 99.8 \, \text{g}
\][/tex]
So, the mass of sulfur formed is approximately 99.8 grams. Therefore, the correct answer is:
D) 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]
Step 1: Calculate the moles of water
First, we need to determine the number of moles of water (Hâ‚‚O) formed. The molar mass of water is approximately 18.015 grams per mole.
[tex]\[
\text{Moles of H}_2\text{O} = \frac{\text{Mass of H}_2\text{O}}{\text{Molar mass of H}_2\text{O}} = \frac{37.4 \, \text{g}}{18.015 \, \text{g/mol}} \approx 2.076 \, \text{moles}
\][/tex]
Step 2: Use stoichiometry to find the moles of sulfur
From the balanced equation, we see that 2 moles of Hâ‚‚O are produced for every 3 moles of sulfur (S) formed. Therefore, the moles of sulfur that are formed are calculated as follows:
[tex]\[
\text{Moles of S} = \left(\frac{3 \, \text{moles of S}}{2 \, \text{moles of H}_2\text{O}}\right) \times 2.076 \, \text{moles of H}_2\text{O} \approx 3.114 \, \text{moles}
\][/tex]
Step 3: Calculate the mass of sulfur
Finally, we convert the moles of sulfur to grams using the molar mass of sulfur, which is approximately 32.06 grams per mole:
[tex]\[
\text{Mass of S} = \text{Moles of S} \times \text{Molar mass of S} = 3.114 \, \text{moles} \times 32.06 \, \text{g/mol} \approx 99.8 \, \text{g}
\][/tex]
So, the mass of sulfur formed is approximately 99.8 grams. Therefore, the correct answer is:
D) 99.8 g S
Thank you for reading the article According to the following reaction how many grams of sulfur are formed when 37 4 g of water are produced 2 H 2 S g. We hope the information provided is useful and helps you understand this topic better. Feel free to explore more helpful content on our website!
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