Copper metal can be prepared by roasting copper ore, which can contain cuprite (Cu₂S) and copper(II) sulfide. Cu₂ S(s) + O₂(g) → 2 Cu(s) + SO₂ (g) CuS(s) + O₂(g) → Cu(s) + SO₂ (g) Suppose an ore sample contains 10.0% impurity in addition to a mixture of CuS and Cu₂ S. Heating 100.0 g of the mixture produces 75.8 g of copper metal with a purity of 91.1%. What is the weight percent of CuS in the ore? The weight percent of Cu₂ S? Weight percent of Cus = Weight percent of Cu₂ S = % %
Copper metal can be prepared by roasting copper ore, which can contain cuprite (Cu₂S) and copper(II) sulfide. Cu₂ S(s) + O₂(g) → 2 Cu(s) + SO₂ (g) CuS(s) + O₂(g) → Cu(s) + SO₂ (g) Suppose an ore sample contains 10.0% impurity in addition to a mixture of CuS and Cu₂ S. Heating 100.0 g of the mixture produces 75.8 g of copper metal with a purity of 91.1%. What is the weight percent of CuS in the ore? The weight percent of Cu₂ S? Weight percent of Cus = Weight percent of Cu₂ S = % %
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
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![### Preparation of Copper Metal from Copper Ore
Copper metal can be prepared by roasting copper ore. The ore can contain cuprite (\( \text{Cu}_2\text{S} \)) and copper(II) sulfide (\( \text{CuS} \)).
#### Relevant Chemical Reactions
1. For cuprite:
\[ \text{Cu}_2\text{S}(s) + \text{O}_2(g) \rightarrow 2 \text{Cu}(s) + \text{SO}_2(g) \]
2. For copper(II) sulfide:
\[ \text{CuS}(s) + \text{O}_2(g) \rightarrow \text{Cu}(s) + \text{SO}_2(g) \]
#### Problem Statement
Suppose an ore sample contains 10.0% impurity in addition to a mixture of \( \text{CuS} \) and \( \text{Cu}_2\text{S} \). Heating 100.0 g of the mixture produces 75.8 g of copper metal with a purity of 91.1%. What are the weight percent of \( \text{CuS} \) and \( \text{Cu}_2\text{S} \) in the ore?
#### Calculation Requirements
- **Weight percent of \( \text{CuS} \)** in the ore:
\[ \boxed{\text{Weight percent of CuS} \: \%} \]
- **Weight percent of \( \text{Cu}_2\text{S} \)** in the ore:
\[ \boxed{\text{Weight percent of Cu}_2\text{S} \: \%} \]
### Steps to Solve the Problem:
1. Calculate the actual weight of copper produced from the reaction.
2. Determine the total weight of copper that can be produced from the given weights of \( \text{CuS} \) and \( \text{Cu}_2\text{S} \).
3. Use stoichiometry to relate the masses of \( \text{CuS} \) and \( \text{Cu}_2\text{S} \) to the masses of copper produced.
4. Develop equations using the known purity and total mass.
5. Solve for the weights of \( \text{CuS} \) and \( \text{Cu}_2](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F7a354f1c-cdfd-41e5-a863-9a86a504af1c%2F3544396c-ce1a-4c60-982c-99c951545cc2%2F1nxhaol_processed.png&w=3840&q=75)
Transcribed Image Text:### Preparation of Copper Metal from Copper Ore
Copper metal can be prepared by roasting copper ore. The ore can contain cuprite (\( \text{Cu}_2\text{S} \)) and copper(II) sulfide (\( \text{CuS} \)).
#### Relevant Chemical Reactions
1. For cuprite:
\[ \text{Cu}_2\text{S}(s) + \text{O}_2(g) \rightarrow 2 \text{Cu}(s) + \text{SO}_2(g) \]
2. For copper(II) sulfide:
\[ \text{CuS}(s) + \text{O}_2(g) \rightarrow \text{Cu}(s) + \text{SO}_2(g) \]
#### Problem Statement
Suppose an ore sample contains 10.0% impurity in addition to a mixture of \( \text{CuS} \) and \( \text{Cu}_2\text{S} \). Heating 100.0 g of the mixture produces 75.8 g of copper metal with a purity of 91.1%. What are the weight percent of \( \text{CuS} \) and \( \text{Cu}_2\text{S} \) in the ore?
#### Calculation Requirements
- **Weight percent of \( \text{CuS} \)** in the ore:
\[ \boxed{\text{Weight percent of CuS} \: \%} \]
- **Weight percent of \( \text{Cu}_2\text{S} \)** in the ore:
\[ \boxed{\text{Weight percent of Cu}_2\text{S} \: \%} \]
### Steps to Solve the Problem:
1. Calculate the actual weight of copper produced from the reaction.
2. Determine the total weight of copper that can be produced from the given weights of \( \text{CuS} \) and \( \text{Cu}_2\text{S} \).
3. Use stoichiometry to relate the masses of \( \text{CuS} \) and \( \text{Cu}_2\text{S} \) to the masses of copper produced.
4. Develop equations using the known purity and total mass.
5. Solve for the weights of \( \text{CuS} \) and \( \text{Cu}_2
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