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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Question
How many moles are present in 19.4 g of N2 and 19.4 g of F2?
![### a) Chemical Reaction Analysis
For the following unbalanced chemical equation, suppose that exactly 5.45 g of each reactant is taken.
\[ \text{S(s) + H}_2\text{SO}_4\text{(aq)} \rightarrow \text{SO}_2\text{(g) + H}_2\text{O(l)} \]
- **Limiting reactant:** [Input Box]
- **Mass of SO₂ =** [Input Box] g
- **Mass of H₂O =** [Input Box] g
### b) Chemical Reaction Analysis
For the following unbalanced chemical equation, suppose that exactly 5.40 g of each reactant is taken.
\[ \text{MnO}_2\text{(s) + H}_2\text{SO}_4\text{(aq)} \rightarrow \text{Mn(SO}_4\text{)}_2\text{(s) + H}_2\text{O(l)} \]
- **Limiting reactant:** [Input Box]
- **Mass of Mn(SO₄)₂ =** [Input Box] g
- **Mass of H₂O =** [Input Box] g
### Iron(III) Oxide Formation
If steel wool (iron) is heated until it glows and is placed in a bottle containing pure oxygen, the iron reacts spectacularly to produce iron(III) oxide.
\[ \text{Fe(s) + O}_2\text{(g)} \rightarrow \text{Fe}_2\text{O}_3\text{(s)} \]
If 1.12 g of iron is heated and placed in a bottle containing 0.0165 mol of oxygen gas, what mass of iron(III) oxide is produced?
- **Mass =** [Input Box] g](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F41533dd6-be05-40da-a627-190380aa1e53%2F9eeb7dae-0387-48f2-aced-ee52419114b4%2Fudzltg_processed.png&w=3840&q=75)
Transcribed Image Text:### a) Chemical Reaction Analysis
For the following unbalanced chemical equation, suppose that exactly 5.45 g of each reactant is taken.
\[ \text{S(s) + H}_2\text{SO}_4\text{(aq)} \rightarrow \text{SO}_2\text{(g) + H}_2\text{O(l)} \]
- **Limiting reactant:** [Input Box]
- **Mass of SO₂ =** [Input Box] g
- **Mass of H₂O =** [Input Box] g
### b) Chemical Reaction Analysis
For the following unbalanced chemical equation, suppose that exactly 5.40 g of each reactant is taken.
\[ \text{MnO}_2\text{(s) + H}_2\text{SO}_4\text{(aq)} \rightarrow \text{Mn(SO}_4\text{)}_2\text{(s) + H}_2\text{O(l)} \]
- **Limiting reactant:** [Input Box]
- **Mass of Mn(SO₄)₂ =** [Input Box] g
- **Mass of H₂O =** [Input Box] g
### Iron(III) Oxide Formation
If steel wool (iron) is heated until it glows and is placed in a bottle containing pure oxygen, the iron reacts spectacularly to produce iron(III) oxide.
\[ \text{Fe(s) + O}_2\text{(g)} \rightarrow \text{Fe}_2\text{O}_3\text{(s)} \]
If 1.12 g of iron is heated and placed in a bottle containing 0.0165 mol of oxygen gas, what mass of iron(III) oxide is produced?
- **Mass =** [Input Box] g
![**Chemistry Stoichiometry Practice: Limiting Reactant and Mole Calculations**
1. **Mole Calculation**
- **Problem:** How many moles are present in 19.4 g of \( \text{N}_2 \) and 19.4 g of \( \text{F}_2 \)?
- **Input Fields:**
- Moles of \( \text{N}_2 \): [Text Box] mol \( \text{N}_2 \)
- Moles of \( \text{F}_2 \): [Text Box] mol \( \text{F}_2 \)
- **Button:** Submit
2. **Product Formation from Reactants**
- **Problem:** What amount of \( \text{NF}_3 \) can be formed from the amount of each reactant?
- If all of the \( \text{N}_2 \) was used up in the reaction, how many moles of \( \text{NF}_3 \) would be produced?
- **Input Field:** [Text Box] mol \( \text{NF}_3 \)
- **Button:** Submit
3. **Product Formation from Reactants (Continued)**
- **Problem:** What amount of \( \text{NF}_3 \) can be formed from the amount of each reactant?
- If all of the \( \text{F}_2 \) was used up in the reaction, how many moles of \( \text{NF}_3 \) would be produced?
- **Input Field:** [Text Box] mol \( \text{NF}_3 \)
- **Button:** Submit
4. **Identifying the Limiting Reactant**
- **Scenario:** If all of the \( \text{N}_2 \) is used up in the reaction, 1.38 mol \( \text{NF}_3 \) would be produced. If all of the \( \text{F}_2 \) is used up in the reaction, 0.340 mol \( \text{NF}_3 \) would be produced.
- **Question:** Which reactant is the limiting reactant?
- **Options:**
- \( \text{N}_2 \)
- \( \text{F}_2 \)
- **Button:** Submit
5. **Mass of Product from Limiting React](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F41533dd6-be05-40da-a627-190380aa1e53%2F9eeb7dae-0387-48f2-aced-ee52419114b4%2Fts4laob_processed.png&w=3840&q=75)
Transcribed Image Text:**Chemistry Stoichiometry Practice: Limiting Reactant and Mole Calculations**
1. **Mole Calculation**
- **Problem:** How many moles are present in 19.4 g of \( \text{N}_2 \) and 19.4 g of \( \text{F}_2 \)?
- **Input Fields:**
- Moles of \( \text{N}_2 \): [Text Box] mol \( \text{N}_2 \)
- Moles of \( \text{F}_2 \): [Text Box] mol \( \text{F}_2 \)
- **Button:** Submit
2. **Product Formation from Reactants**
- **Problem:** What amount of \( \text{NF}_3 \) can be formed from the amount of each reactant?
- If all of the \( \text{N}_2 \) was used up in the reaction, how many moles of \( \text{NF}_3 \) would be produced?
- **Input Field:** [Text Box] mol \( \text{NF}_3 \)
- **Button:** Submit
3. **Product Formation from Reactants (Continued)**
- **Problem:** What amount of \( \text{NF}_3 \) can be formed from the amount of each reactant?
- If all of the \( \text{F}_2 \) was used up in the reaction, how many moles of \( \text{NF}_3 \) would be produced?
- **Input Field:** [Text Box] mol \( \text{NF}_3 \)
- **Button:** Submit
4. **Identifying the Limiting Reactant**
- **Scenario:** If all of the \( \text{N}_2 \) is used up in the reaction, 1.38 mol \( \text{NF}_3 \) would be produced. If all of the \( \text{F}_2 \) is used up in the reaction, 0.340 mol \( \text{NF}_3 \) would be produced.
- **Question:** Which reactant is the limiting reactant?
- **Options:**
- \( \text{N}_2 \)
- \( \text{F}_2 \)
- **Button:** Submit
5. **Mass of Product from Limiting React
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