Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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Balance the following
![### Stoichiometry Problem
**Problem Statement:**
2. __Zn + __HCl → __ZnCl₂ + __H₂
When 5.00g of zinc metal reacts with excess hydrochloric acid, how many grams of zinc chloride will be produced?
**Explanation:**
This question involves a chemical reaction between zinc metal (Zn) and hydrochloric acid (HCl). The reaction that takes place is written in an unbalanced equation format:
\[ \text{Zn} + \text{HCl} \rightarrow \text{ZnCl}_2 + \text{H}_2 \]
To solve this problem, one would need to balance the chemical equation first and then use stoichiometry to find out how many grams of zinc chloride (ZnCl₂) will be produced from 5.00 grams of zinc reacting with an excess of hydrochloric acid.
1. **Balance the Equation:**
\[ \text{Zn} + 2\text{HCl} \rightarrow \text{ZnCl}_2 + \text{H}_2 \]
2. **Calculate the molar masses:**
- Molar mass of Zn = 65.38 g/mol
- Molar mass of ZnCl₂ = 136.30 g/mol
3. **Convert the mass of Zn to moles:**
\[ \frac{5.00 \, \text{g Zn}}{65.38 \, \text{g/mol}} = 0.0765 \, \text{mol Zn} \]
4. **Use the stoichiometry of the balanced equation to find moles of ZnCl₂ produced:**
\[ \text{1 mol Zn} \rightarrow \text{1 mol ZnCl}_2 \]
So, 0.0765 mol Zn produces 0.0765 mol ZnCl₂.
5. **Convert moles of ZnCl₂ to grams:**
\[ 0.0765 \, \text{mol ZnCl}_2 \times 136.30 \, \text{g/mol} = 10.43 \, \text{g ZnCl}_2 \]
**Conclusion:**
\[ \boxed{10.43} \]
When 5.00 grams of zinc metal reacts with excess hydrochloric acid, 10.43 grams of zinc chloride will be produced.](https://content.bartleby.com/qna-images/question/42f6465b-f85d-48ef-ab35-b220e483503b/f3162a19-ca0b-487b-8744-6e1f774080f3/7rd1chf_processed.png)
Transcribed Image Text:### Stoichiometry Problem
**Problem Statement:**
2. __Zn + __HCl → __ZnCl₂ + __H₂
When 5.00g of zinc metal reacts with excess hydrochloric acid, how many grams of zinc chloride will be produced?
**Explanation:**
This question involves a chemical reaction between zinc metal (Zn) and hydrochloric acid (HCl). The reaction that takes place is written in an unbalanced equation format:
\[ \text{Zn} + \text{HCl} \rightarrow \text{ZnCl}_2 + \text{H}_2 \]
To solve this problem, one would need to balance the chemical equation first and then use stoichiometry to find out how many grams of zinc chloride (ZnCl₂) will be produced from 5.00 grams of zinc reacting with an excess of hydrochloric acid.
1. **Balance the Equation:**
\[ \text{Zn} + 2\text{HCl} \rightarrow \text{ZnCl}_2 + \text{H}_2 \]
2. **Calculate the molar masses:**
- Molar mass of Zn = 65.38 g/mol
- Molar mass of ZnCl₂ = 136.30 g/mol
3. **Convert the mass of Zn to moles:**
\[ \frac{5.00 \, \text{g Zn}}{65.38 \, \text{g/mol}} = 0.0765 \, \text{mol Zn} \]
4. **Use the stoichiometry of the balanced equation to find moles of ZnCl₂ produced:**
\[ \text{1 mol Zn} \rightarrow \text{1 mol ZnCl}_2 \]
So, 0.0765 mol Zn produces 0.0765 mol ZnCl₂.
5. **Convert moles of ZnCl₂ to grams:**
\[ 0.0765 \, \text{mol ZnCl}_2 \times 136.30 \, \text{g/mol} = 10.43 \, \text{g ZnCl}_2 \]
**Conclusion:**
\[ \boxed{10.43} \]
When 5.00 grams of zinc metal reacts with excess hydrochloric acid, 10.43 grams of zinc chloride will be produced.
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