How many moles of aluminum are required to completely react with 107 mL of 6.00 M H.SO. according to the balanced chemical reaction: 2 Al(s) + 3 H:SO.(aq) → Al:(SO.)»(aq) + 3 H:(g)
How many moles of aluminum are required to completely react with 107 mL of 6.00 M H.SO. according to the balanced chemical reaction: 2 Al(s) + 3 H:SO.(aq) → Al:(SO.)»(aq) + 3 H:(g)
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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![**Transcription for Educational Website:**
---
**Problem Statement:**
How many moles of aluminum are required to completely react with \(107 \, \text{mL}\) of \(6.00 \, \text{M} \, \text{H}_2\text{SO}_4\), according to the balanced chemical reaction:
\[
2 \, \text{Al(s)} + 3 \, \text{H}_2\text{SO}_4(aq) \rightarrow \text{Al}_2(\text{SO}_4)_3(aq) + 3 \, \text{H}_2(g)
\]
**Calculation Overview:**
1. **Starting Amount:**
- Initially, the **starting amount** section is labeled but not filled in.
2. **Conversion Factors:**
- The interactive diagram allows for the adjustment of factors in conversion calculations.
3. **Conversion Factors and Units:**
- Numerical inputs available include: \(0.428\), \(0.0374\), \(1\), \(3\), \(107\), \(1000\), \(0.001\), \(0.963\).
- Units corresponding to these numbers include:
- \(\text{mL} \, \text{H}_2\text{SO}_4\)
- \(\text{M} \, \text{H}_2\text{SO}_4\)
- \(\text{g} \, \text{H}_2\text{SO}_4\)
- \(\text{g} \, \text{Al}\)
- \(\text{mol} \, \text{H}_2\text{SO}_4\)
- \(\text{mol} \, \text{Al}\)
- \(\text{mol} \, \text{Al}_2(\text{SO}_4)_3\)
- \(\text{g} \, \text{H}_2\)
4. **Buttons and Functions:**
- **Add Factor:** Input space for additional conversion factors.
- **Answer and Reset:** Buttons to compute and clear the results.
5. **Constant Values:**
- Molar masses and Avogadro's number are provided for conversions:
- \(98.08\) (likely g/mol](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F048127f3-de9a-44a1-9086-2f981c8bd58d%2Ff82ec51c-e84a-4dae-abb7-e252a81acdce%2Fugwxtz_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Transcription for Educational Website:**
---
**Problem Statement:**
How many moles of aluminum are required to completely react with \(107 \, \text{mL}\) of \(6.00 \, \text{M} \, \text{H}_2\text{SO}_4\), according to the balanced chemical reaction:
\[
2 \, \text{Al(s)} + 3 \, \text{H}_2\text{SO}_4(aq) \rightarrow \text{Al}_2(\text{SO}_4)_3(aq) + 3 \, \text{H}_2(g)
\]
**Calculation Overview:**
1. **Starting Amount:**
- Initially, the **starting amount** section is labeled but not filled in.
2. **Conversion Factors:**
- The interactive diagram allows for the adjustment of factors in conversion calculations.
3. **Conversion Factors and Units:**
- Numerical inputs available include: \(0.428\), \(0.0374\), \(1\), \(3\), \(107\), \(1000\), \(0.001\), \(0.963\).
- Units corresponding to these numbers include:
- \(\text{mL} \, \text{H}_2\text{SO}_4\)
- \(\text{M} \, \text{H}_2\text{SO}_4\)
- \(\text{g} \, \text{H}_2\text{SO}_4\)
- \(\text{g} \, \text{Al}\)
- \(\text{mol} \, \text{H}_2\text{SO}_4\)
- \(\text{mol} \, \text{Al}\)
- \(\text{mol} \, \text{Al}_2(\text{SO}_4)_3\)
- \(\text{g} \, \text{H}_2\)
4. **Buttons and Functions:**
- **Add Factor:** Input space for additional conversion factors.
- **Answer and Reset:** Buttons to compute and clear the results.
5. **Constant Values:**
- Molar masses and Avogadro's number are provided for conversions:
- \(98.08\) (likely g/mol
![The image displays a question from a chemistry exercise, labeled as “Question 22 of 27.” The task involves calculating how many moles of aluminum are needed to completely react with 107 milliliters of 6.00 M H₂SO₄, according to the balanced chemical equation:
\[ 2 \, \text{Al (s)} + 3 \, \text{H₂SO₄ (aq)} \rightarrow \text{Al₂(SO₄)₃ (aq)} + 3 \, \text{H₂ (g)} \]
The problem-solving interface is structured into different sections for calculation:
1. **Starting Amount:** Fields are provided for input, labeled as "STARTING AMOUNT."
2. **Calculation Area:** This section is used for multiplying and adding factors.
3. **Add Factor Section:** Contains numerical buttons and various units/labels such as:
- Numbers: 0.428, 0.0374, 1, 3, 107, etc.
- Constants: 6.022 × 10²³
- Units and Labels: mL H₂SO₄, M H₂SO₄, g H₂SO₄, g Al, mol H₂, mol Al, mol Al₂(SO₄)₃, etc.
4. **Answer Section:** Allows users to input answers or calculations and reset if needed.
This tool appears to facilitate the step-by-step calculation of reactant and product quantities in a chemical reaction.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F048127f3-de9a-44a1-9086-2f981c8bd58d%2Ff82ec51c-e84a-4dae-abb7-e252a81acdce%2F3l7pxqv_processed.jpeg&w=3840&q=75)
Transcribed Image Text:The image displays a question from a chemistry exercise, labeled as “Question 22 of 27.” The task involves calculating how many moles of aluminum are needed to completely react with 107 milliliters of 6.00 M H₂SO₄, according to the balanced chemical equation:
\[ 2 \, \text{Al (s)} + 3 \, \text{H₂SO₄ (aq)} \rightarrow \text{Al₂(SO₄)₃ (aq)} + 3 \, \text{H₂ (g)} \]
The problem-solving interface is structured into different sections for calculation:
1. **Starting Amount:** Fields are provided for input, labeled as "STARTING AMOUNT."
2. **Calculation Area:** This section is used for multiplying and adding factors.
3. **Add Factor Section:** Contains numerical buttons and various units/labels such as:
- Numbers: 0.428, 0.0374, 1, 3, 107, etc.
- Constants: 6.022 × 10²³
- Units and Labels: mL H₂SO₄, M H₂SO₄, g H₂SO₄, g Al, mol H₂, mol Al, mol Al₂(SO₄)₃, etc.
4. **Answer Section:** Allows users to input answers or calculations and reset if needed.
This tool appears to facilitate the step-by-step calculation of reactant and product quantities in a chemical reaction.
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