https://file.aiquickdraw.com/mathbot/file/17215143173367bgbgjek.png

Write a balanced equation for the oxidation half-reaction in this overall process.

To write the balanced equation for the oxidation half-reaction in the given overall process, we need to identify the species being oxidized and the species being reduced in the overall reaction:

\[ 2 \text{Cu} (s) + \text{Cl}_2 (aq) \rightarrow 2 \text{CuCl} (s) \]

In this reaction, copper (Cu) is being oxidized and chlorine (\(\text{Cl}_2\)) is being reduced.

1. **Oxidation Half-Reaction:**
Copper (Cu) is being oxidized from an oxidation state of 0 to +1 in \(\text{CuCl}\). This can be represented as:
\[ \text{Cu} (s) \rightarrow \text{Cu}^+ (aq) + e^- \]

Since there are 2 moles of copper in the overall reaction, the oxidation half-reaction is:
\[ 2 \text{Cu} (s) \rightarrow 2 \text{Cu}^+ (aq) + 2 e^- \]

2. **Reduction Half-Reaction:**
Chlorine (\(\text{Cl}_2\)) is being reduced from an oxidation state of 0 to -1 in \(\text{CuCl}\). This can be represented as:
\[ \text{Cl}_2 (aq) + 2 e^- \rightarrow 2 \text{Cl}^- (aq) \]

Combining these half-reactions, the balanced overall redox reaction is:
\[ 2 \text{Cu} (s) + \text{Cl}_2 (aq) \rightarrow 2 \text{Cu}^+ (aq) + 2 \text{Cl}^- (aq) \]

Then, the \(\text{Cu}^+\) and \(\text{Cl}^-\) ions combine to form \(\text{CuCl}\):
\[ 2 \text{Cu}^+ (aq) + 2 \text{Cl}^- (aq) \rightarrow 2 \text{CuCl} (s) \]

So, the oxidation half-reaction for this process is:
\[ 2 \text{Cu} (s) \rightarrow 2 \text{Cu}^+ (aq) + 2 e^- \]

Would you like further details or have any questions? 

Here are 5 numbered questions you might consider asking next:
1. How do you determine the oxidation state of an element in a compound?
2. What is the difference between oxidation and reduction in a redox reaction?
3. How do you balance a redox reaction in acidic and basic conditions?
4. What are some common methods to prevent corrosion of copper pipes?
5. Can you explain the role of electrons in redox reactions?

**Tip:** When balancing redox reactions, it can be helpful to separate the oxidation and reduction processes into half-reactions, balance each for mass and charge, and then combine them back together.

Learn how to write a balanced equation for the oxidation half-reaction in a redox process. Understand oxidation states, half-reactions, and how to balance redox equations step-by-step. Suitable for advanced high school students and chemistry enthusiasts.

Math Problem Statement

Solution

Ask a new question for Free

By Image

Math Problem Analysis

Mathematical Concepts

Formulas

Theorems

Suitable Grade Level

Related Recommendation