In the above redox reaction, use oxidation numbers to identify the element oxidized, the element reduced, the oxidizing agent and the reducing agent. name of the element oxidized: H3ASO4 + Ni²+NiO₂ + HASO₂+ 2H+ formula of the oxidizing agent: name of the element reduced: formula of the reducing agent:
Science behind corrosion-test
Corrosion is defined as an activity that transforms refined metals into more chemically stable forms such as oxide, hydroxide, carbonate, or sulfide. It refers to the slow decomposition of things (typically metals); thanks to chemical and/or electrochemical reactions with their surroundings. Corrosion engineering is the science of preventing and controlling corrosion.
Corrosion
Corrosion is defined as an activity that transforms refined metals into more chemically stable forms such as oxide, hydroxide, carbonate, or sulfide. It refers to the slow decomposition of things (typically metals); thanks to chemical and/or electrochemical reactions with their surroundings. Corrosion engineering is the science of preventing and controlling corrosion.
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![**Educational Content on Redox Reactions**
In the chemical reaction:
\[ \text{H}_3\text{AsO}_4 + \text{Ni}^{2+} \rightarrow \text{NiO}_2 + \text{HAsO}_2 + 2\text{H}^+ \]
we are focusing on the redox (reduction-oxidation) process. This reaction involves changes in the oxidation states of elements, which allows us to determine which elements are oxidized and reduced, as well as identifying the oxidizing and reducing agents.
**Instructions**:
Use the oxidation numbers in the above reaction to fill in the following information:
- **Name of the element oxidized**: [Input Box]
- **Name of the element reduced**: [Input Box]
- **Formula of the oxidizing agent**: [Input Box]
- **Formula of the reducing agent**: [Input Box]
Understanding which elements have been oxidized or reduced is central to grasping the concepts of redox reactions. The element whose oxidation state increases is being oxidized, while the element whose oxidation state decreases is being reduced. The oxidizing agent is the species that gets reduced, and the reducing agent is the species that gets oxidized. These concepts are foundational for analyzing chemical reactions in both laboratory and practical applications.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fc59929d2-245b-4a65-870a-b2f34cf83609%2F3c0866de-0719-4b0c-8238-ba45b72adde8%2Fo15r99gn_processed.png&w=3840&q=75)
![**Redox Reaction Analysis**
**Reaction:**
\[ \text{Al} + \text{Cr}^{3+} \rightarrow \text{Al}^{3+} + \text{Cr} \]
In the above redox reaction, use oxidation numbers to identify the element oxidized, the element reduced, the oxidizing agent, and the reducing agent.
| Description | Input |
|-------------------------------------|-----------------------------------------------------------------------|
| **Name of the element oxidized:** | [Input Box] |
| **Name of the element reduced:** | [Input Box] |
| **Formula of the oxidizing agent:** | [Input Box] |
| **Formula of the reducing agent:** | [Input Box] |](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fc59929d2-245b-4a65-870a-b2f34cf83609%2F3c0866de-0719-4b0c-8238-ba45b72adde8%2Fjqs29ki_processed.png&w=3840&q=75)
-> The element that has oxidation state increases that is oxidized whereas , element that has oxidation state decreases that is reduced.
-> The species which is oxidized that is reducing agent and species which is reduced that is oxidizing agent.
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