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impor needed for this question. (1) Identify each of the following half-reactions as either an oxidation half-reaction or a reduction half-reaction. half-reaction 2+ Cu²+ (aq) + 2e™ →Cu(s) Ni(s) Ni2+ (aq) + 2e™ identification ✪ (2) Write a balanced equation for the overall redox reaction Use smallest possible integer

impor needed for this question. (1) Identify each of the following half-reactions as either an oxidation half-reaction or a reduction half-reaction. half-reaction 2+ Cu²+ (aq) + 2e™ →Cu(s) Ni(s) Ni2+ (aq) + 2e™ identification ✪ (2) Write a balanced equation for the overall redox reaction Use smallest possible integer

Chemistry
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
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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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# Redox Reactions Educational Exercise ### Instructions Use the references to access important values if needed for this question. ### Problem 1 **Identify each of the following half-reactions as either an oxidation half-reaction or a reduction half-reaction.** #### Table: Half-Reaction Identification | Half-Reaction | Identification | |-----------------------------------|-----------------------| | \( \text{Cu}^{2+} (aq) + 2e^- \rightarrow \text{Cu} (s) \) | (Dropdown for selection) | | \( \text{Ni} (s) \rightarrow \text{Ni}^{2+} (aq) + 2e^- \) | (Dropdown for selection) | ### Problem 2 **Write a balanced equation for the overall redox reaction. Use the smallest possible integer coefficients.** --- #### Explanation - **Cu Half-Reaction**: This reaction involves the gain of electrons (\( 2e^- \) by \( \text{Cu}^{2+} \) ions to form elemental copper (\( \text{Cu} (s) \)). This is typically a reduction process. - **Ni Half-Reaction**: This reaction shows the loss of electrons from elemental nickel (\( \text{Ni} (s) \)) to form \( \text{Ni}^{2+} (aq) \) ions. This is typically an oxidation process. These exercises help understand electron transfer in redox processes by distinguishing between oxidation and reduction.
Transcribed Image Text:# Redox Reactions Educational Exercise ### Instructions Use the references to access important values if needed for this question. ### Problem 1 **Identify each of the following half-reactions as either an oxidation half-reaction or a reduction half-reaction.** #### Table: Half-Reaction Identification | Half-Reaction | Identification | |-----------------------------------|-----------------------| | \( \text{Cu}^{2+} (aq) + 2e^- \rightarrow \text{Cu} (s) \) | (Dropdown for selection) | | \( \text{Ni} (s) \rightarrow \text{Ni}^{2+} (aq) + 2e^- \) | (Dropdown for selection) | ### Problem 2 **Write a balanced equation for the overall redox reaction. Use the smallest possible integer coefficients.** --- #### Explanation - **Cu Half-Reaction**: This reaction involves the gain of electrons (\( 2e^- \) by \( \text{Cu}^{2+} \) ions to form elemental copper (\( \text{Cu} (s) \)). This is typically a reduction process. - **Ni Half-Reaction**: This reaction shows the loss of electrons from elemental nickel (\( \text{Ni} (s) \)) to form \( \text{Ni}^{2+} (aq) \) ions. This is typically an oxidation process. These exercises help understand electron transfer in redox processes by distinguishing between oxidation and reduction.
**(1)** Identify each of the following half-reactions as either an **oxidation** half-reaction or a **reduction** half-reaction. | half-reaction | identification | |------------------------------------|-------------------| | Cu²⁺(aq) + 2e⁻ → Cu(s) | [Reduction] | | Mn(s) → Mn²⁺(aq) + 2e⁻ | [Oxidation] | **(2)** Write a balanced equation for the overall redox reaction. **Use smallest possible integer coefficients.** \[ \text{Cu}^{2+}(aq) + \text{Mn}(s) \rightarrow \text{Cu}(s) + \text{Mn}^{2+}(aq) \]
Transcribed Image Text:**(1)** Identify each of the following half-reactions as either an **oxidation** half-reaction or a **reduction** half-reaction. | half-reaction | identification | |------------------------------------|-------------------| | Cu²⁺(aq) + 2e⁻ → Cu(s) | [Reduction] | | Mn(s) → Mn²⁺(aq) + 2e⁻ | [Oxidation] | **(2)** Write a balanced equation for the overall redox reaction. **Use smallest possible integer coefficients.** \[ \text{Cu}^{2+}(aq) + \text{Mn}(s) \rightarrow \text{Cu}(s) + \text{Mn}^{2+}(aq) \]
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