Thank you for visiting According to the following reaction how many grams of sulfur are formed when 37 4 g of water are formed 2 text H 2 text. 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 :
Sure! Let's work through this problem step by step to find out how many grams of sulfur are formed when 37.4 grams of water are produced in the reaction.
1. Identify the Reaction:
The chemical reaction given is:
[tex]\[ 2 \text{H}_2\text{S} + \text{SO}_2 \rightarrow 3 \text{S} + 2 \text{H}_2\text{O} \][/tex]
2. Determine Molar Masses:
- Molar mass of water (Hâ‚‚O) is approximately 18.015 g/mol.
- Molar mass of sulfur (S) is approximately 32.07 g/mol.
3. Calculate Moles of Water:
First, we calculate the number of moles of water formed from 37.4 grams:
[tex]\[
\text{Moles of } \text{H}_2\text{O} = \frac{37.4 \text{ g}}{18.015 \text{ g/mol}} \approx 2.076 \text{ moles}
\][/tex]
4. Relate Moles of Water to Moles of Sulfur:
From the balanced equation, we see that 2 moles of water are produced from 3 moles of sulfur. Thus, for every 2 moles of water formed, there are 3 moles of sulfur formed:
[tex]\[
\text{Moles of S} = \left(\frac{3}{2}\right) \times \text{Moles of } \text{H}_2\text{O} \approx \left(\frac{3}{2}\right) \times 2.076 \approx 3.114 \text{ moles}
\][/tex]
5. Calculate the Mass of Sulfur:
Now, convert the moles of sulfur to grams:
[tex]\[
\text{Mass of S} = 3.114 \text{ moles} \times 32.07 \text{ g/mol} \approx 99.87 \text{ grams}
\][/tex]
Therefore, when 37.4 grams of water are formed, approximately 99.8 grams of sulfur are produced. So, the correct answer is 99.8 g S.
1. Identify the Reaction:
The chemical reaction given is:
[tex]\[ 2 \text{H}_2\text{S} + \text{SO}_2 \rightarrow 3 \text{S} + 2 \text{H}_2\text{O} \][/tex]
2. Determine Molar Masses:
- Molar mass of water (Hâ‚‚O) is approximately 18.015 g/mol.
- Molar mass of sulfur (S) is approximately 32.07 g/mol.
3. Calculate Moles of Water:
First, we calculate the number of moles of water formed from 37.4 grams:
[tex]\[
\text{Moles of } \text{H}_2\text{O} = \frac{37.4 \text{ g}}{18.015 \text{ g/mol}} \approx 2.076 \text{ moles}
\][/tex]
4. Relate Moles of Water to Moles of Sulfur:
From the balanced equation, we see that 2 moles of water are produced from 3 moles of sulfur. Thus, for every 2 moles of water formed, there are 3 moles of sulfur formed:
[tex]\[
\text{Moles of S} = \left(\frac{3}{2}\right) \times \text{Moles of } \text{H}_2\text{O} \approx \left(\frac{3}{2}\right) \times 2.076 \approx 3.114 \text{ moles}
\][/tex]
5. Calculate the Mass of Sulfur:
Now, convert the moles of sulfur to grams:
[tex]\[
\text{Mass of S} = 3.114 \text{ moles} \times 32.07 \text{ g/mol} \approx 99.87 \text{ grams}
\][/tex]
Therefore, when 37.4 grams of water are formed, approximately 99.8 grams of sulfur are produced. So, the correct answer is 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 formed 2 text H 2 text. 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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