2.96 grams of CaCl2 (111.1 g/mol) is reacted via the following reaction. How much AuCI (232.4 g/mol) is produced? CaCl2(aq) + 2AUNO3(aq) --> 2AUCI(s) + Ca(NO3)2(aq)
2.96 grams of CaCl2 (111.1 g/mol) is reacted via the following reaction. How much AuCI (232.4 g/mol) is produced? CaCl2(aq) + 2AUNO3(aq) --> 2AUCI(s) + Ca(NO3)2(aq)
Chemistry
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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
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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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![**Chemistry Reaction Calculation**
In this exercise, we are given that 2.96 grams of calcium chloride (CaCl₂), with a molar mass of 111.1 g/mol, is reacted through the following chemical equation:
\[ \text{CaCl}_2(\text{aq}) + 2\text{AuNO}_3(\text{aq}) \rightarrow 2\text{AuCl}(\text{s}) + \text{Ca(NO}_3)_2(\text{aq}) \]
The task is to determine how much gold chloride (\[\text{AuCl}\]), with a molar mass of 232.4 g/mol, is produced from this reaction.
**Understanding the Reaction:**
1. **Reactants**:
- Calcium chloride (\[\text{CaCl}_2\]) is reacted in aqueous form.
- Gold nitrate (\[2\text{AuNO}_3\]) is also present in aqueous form.
2. **Products**:
- Solid gold chloride (\[2\text{AuCl}\]) is formed.
- Calcium nitrate (\[\text{Ca(NO}_3)_2\]) remains in aqueous form.
**Calculation Approach:**
1. **Determine Moles of CaCl₂**:
- Convert the given mass of CaCl₂ into moles using its molar mass.
2. **Use Stoichiometry**:
- From the balanced equation, relate the moles of CaCl₂ to moles of AuCl.
- Use the molar ratio to calculate the moles of AuCl produced.
3. **Calculate Mass of AuCl**:
- Convert the moles of AuCl into grams using its molar mass.
This process allows us to find the amount of AuCl produced from the initial quantity of CaCl₂ provided.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F14ad990f-dd7d-47e0-a13f-1f780fa26f58%2F07981618-7861-47ce-8715-af3617e99f3c%2Ftl01okd_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Chemistry Reaction Calculation**
In this exercise, we are given that 2.96 grams of calcium chloride (CaCl₂), with a molar mass of 111.1 g/mol, is reacted through the following chemical equation:
\[ \text{CaCl}_2(\text{aq}) + 2\text{AuNO}_3(\text{aq}) \rightarrow 2\text{AuCl}(\text{s}) + \text{Ca(NO}_3)_2(\text{aq}) \]
The task is to determine how much gold chloride (\[\text{AuCl}\]), with a molar mass of 232.4 g/mol, is produced from this reaction.
**Understanding the Reaction:**
1. **Reactants**:
- Calcium chloride (\[\text{CaCl}_2\]) is reacted in aqueous form.
- Gold nitrate (\[2\text{AuNO}_3\]) is also present in aqueous form.
2. **Products**:
- Solid gold chloride (\[2\text{AuCl}\]) is formed.
- Calcium nitrate (\[\text{Ca(NO}_3)_2\]) remains in aqueous form.
**Calculation Approach:**
1. **Determine Moles of CaCl₂**:
- Convert the given mass of CaCl₂ into moles using its molar mass.
2. **Use Stoichiometry**:
- From the balanced equation, relate the moles of CaCl₂ to moles of AuCl.
- Use the molar ratio to calculate the moles of AuCl produced.
3. **Calculate Mass of AuCl**:
- Convert the moles of AuCl into grams using its molar mass.
This process allows us to find the amount of AuCl produced from the initial quantity of CaCl₂ provided.
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