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.
I need help with these para rice problems. Thank you!
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**Balancing Redox Reactions and Calculating Cell Potentials**
**[1] In basic solution, balance the redox reaction:**
\[ \text{MnO}_4^{2-} (aq) \rightarrow \text{MnO}_4^{-} (aq) + \text{MnO}_2 (s) \]
**Final balanced reaction equation:**
*Provide the balanced equation here.*
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**[2] In acidic solution, balance the redox reaction:**
\[ \text{Xe} (g) + \text{Cr}_2\text{O}_7^{2-} (aq) \rightarrow \text{XeO}_3 (s) + \text{Cr}^{3+} (aq) \]
**Final balanced reaction equation:**
*Provide the balanced equation here.*
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**[3] Given the Standard Reduction Potentials at 25°C, Mn\(^{2+}\) + 2e\(^{-}\) → Mn E° = -1.185V and Hg\(^{2+}\) + 2e\(^{-}\) → Hg E° = +0.851V, what is the spontaneous reaction between these two half-cells and what is the potential of the cell?**
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**[4] For the reaction:**
\[ \text{Sn} (s) + 2\text{Cu}^{2+} (aq) \rightarrow \text{Sn}^{2+} (aq) + 2\text{Cu}^{+} (aq) \]
The calculated E° = +0.291V, calculate ΔG° and K for this reaction. R = 8.314 J/mol·K.
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**[5]** *(Work on the back)*
For the reaction:
\[ \text{Cu} (s) + 2\text{Ag}^{+} \rightarrow \text{Cu}^{2+} + 2\text{Ag} (s) \]
E° = +0.462 V. Calculate the potential of the following cell shown in cell notation. Is this non-standard cell spontaneous?
\[ \text{Cu}(s) | \text{Cu}^{2+} (0.0037M) || \text{Ag}^{+} (0.016M) | \text{Ag}(s) \]
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