02 not diiw boouborq el (90siq Ismisob ono of g ni) blog to 22601 srl as isrW.8 10. How much current (in A to one decimal place) is needed to produce 100.0 g of gold in 3.00 hr? (aq) + 3e Au(s) Au³+ A: 13.6
02 not diiw boouborq el (90siq Ismisob ono of g ni) blog to 22601 srl as isrW.8 10. How much current (in A to one decimal place) is needed to produce 100.0 g of gold in 3.00 hr? (aq) + 3e Au(s) Au³+ A: 13.6
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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![### Title: Calculating Current Required for Electroplating Gold
**Question:**
How much current (in amperes, A, rounded to one decimal place) is needed to produce 100.0 g of gold in 3.00 hours?
**Chemical Reaction:**
\[ \text{Au}^{3+} (\text{aq}) + 3\text{e}^- \rightarrow \text{Au} (\text{s}) \]
**Answer:**
\[ A = 13.6 \]
**Explanation:**
The problem involves calculating the necessary current for electroplating gold through the reduction of gold ions (\(\text{Au}^{3+}\)) to solid gold (\(\text{Au}\)). The balanced chemical reaction shows that three electrons (\(3\text{e}^-\)) are required for each gold ion reduced. Using principles of electrochemistry and stoichiometry, calculations can be performed to determine the current, using the given mass of gold and time.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F8e77b376-6a5c-4963-870c-f49a6e984799%2Fc8ce7822-f10c-4b20-a490-15de2d78e27e%2F2xgf5f_processed.jpeg&w=3840&q=75)
Transcribed Image Text:### Title: Calculating Current Required for Electroplating Gold
**Question:**
How much current (in amperes, A, rounded to one decimal place) is needed to produce 100.0 g of gold in 3.00 hours?
**Chemical Reaction:**
\[ \text{Au}^{3+} (\text{aq}) + 3\text{e}^- \rightarrow \text{Au} (\text{s}) \]
**Answer:**
\[ A = 13.6 \]
**Explanation:**
The problem involves calculating the necessary current for electroplating gold through the reduction of gold ions (\(\text{Au}^{3+}\)) to solid gold (\(\text{Au}\)). The balanced chemical reaction shows that three electrons (\(3\text{e}^-\)) are required for each gold ion reduced. Using principles of electrochemistry and stoichiometry, calculations can be performed to determine the current, using the given mass of gold and time.
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