**Title:** Writing Balanced Half-Reactions for a Redox Reaction**Objective:** Learn how to write balanced half-reactions for given redox reactions.**Redox Reaction:**\[ I_2(s) + 2 \text{NO}_2(g) + 2 \text{H}_2\text{O}(l) \rightarrow 2 \text{I}^- (aq) + 2 \text{NO}_3^- (aq) + 4 \text{H}^+ (aq) \]**Task:** Write the balanced half-reactions for the above reaction.**Reduction Half-Reaction:**- Identify the substance being reduced and show the gain of electrons.**Oxidation Half-Reaction:**- Identify the substance being oxidized and show the loss of electrons.**Instructions:**Draw rectangles around the area for filling in each half-reaction (This is likely an interactive area to input responses).**Tool Icons:**- A tool is provided to help balance chemical equations. Other icons include arrows and an electron symbol (e⁻), which are used to indicate electron transfer in redox reactions.**Tips:**1. Determine which elements change oxidation states.2. Write separate equations for oxidation and reduction.3. Balance the number of atoms and charges by adding electrons.Use this framework to input and check your balanced half-reactions for completeness and correctness.

Answer:Word Redox is the combination of Red (from reduction) and Ox (from oxidation), that's why…

Answered: Write balanced half-reactions for the…

Write balanced half-reactions for the following redox reaction: 1₂(s) +2 NO₂(g) + 2 H₂O(1) reduction: oxidation: 0 21 (aq) + 2NO3(aq) + 4H* (aq) ローロ e X 2 4

Chemistry

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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

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Concept explainers

Electrolysis

Electrolysis is defined as the process of breaking down ionic compounds into their constituent elements by passing a direct electric current through the compound in a fluid state. The cathode reduces cations, while the anode oxidizes anions. An electrolyte, electrodes, and some form of external power source are the main components required for conducting electrolysis. A partition, such as an ion-exchange membrane or a salt bridge, may also be used, but this is optional. These are primarily used to prevent the products from diffusing near the opposing electrode.

Question

**Title:** Writing Balanced Half-Reactions for a Redox Reaction

**Objective:** Learn how to write balanced half-reactions for given redox reactions.

**Redox Reaction:**

\[ I_2(s) + 2 \text{NO}_2(g) + 2 \text{H}_2\text{O}(l) \rightarrow 2 \text{I}^- (aq) + 2 \text{NO}_3^- (aq) + 4 \text{H}^+ (aq) \]

**Task:** Write the balanced half-reactions for the above reaction.

**Reduction Half-Reaction:**

- Identify the substance being reduced and show the gain of electrons.

**Oxidation Half-Reaction:**

- Identify the substance being oxidized and show the loss of electrons.

**Instructions:**

Draw rectangles around the area for filling in each half-reaction (This is likely an interactive area to input responses).

**Tool Icons:**

- A tool is provided to help balance chemical equations. Other icons include arrows and an electron symbol (e⁻), which are used to indicate electron transfer in redox reactions.

**Tips:**

1. Determine which elements change oxidation states.
2. Write separate equations for oxidation and reduction.
3. Balance the number of atoms and charges by adding electrons.

Use this framework to input and check your balanced half-reactions for completeness and correctness.

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