What current is needed to deposit 0.500 g of chromium metal from a solution of Cr3+ in a period...
Question:
What current is needed to deposit 0.500 g of chromium metal from a solution of {eq}Cr^{3+} {/eq} in a period of 1.00 hr?
Electrolysis:
Some important components which make the process of electrolysis possible are listed below.
- Electrode
- External power source
- Electrolyte
This process usually happens in an electrolytic cell. This electrolytic cell is made up of electrodes (negatively and positively charged). These electrodes are placed apart from each other in a solution that contains negatively and positively charged ions. Electric current flows through these electrodes.
Answer and Explanation: 1
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View this answerGiven Data:
- The mass of chromium metal is 0.500 g.
- The time required is 1 hour =3600 s.
The current required to deposit the given amount of metal...
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Electrolysis | Definition & Process
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Chapter 3 / Lesson 16
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Learn the definition of electrolysis and what electrolytes are, as well as an explanation of the electrolysis process and real-world examples of where it is applied.
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