Answered

Explore Westonci.ca, the leading Q&A site where experts provide accurate and helpful answers to all your questions. Connect with a community of professionals ready to help you find accurate solutions to your questions quickly and efficiently. Get precise and detailed answers to your questions from a knowledgeable community of experts on our Q&A platform.

A student is asked to balance an equation using the half-reaction method. He determines the two half-reactions as shown below:

[tex]\[
\begin{array}{l}
2 \text{Br} ^{-} \longrightarrow \text{Br}_2 + 2 e^{-} \\
\text{Cl}_2 + 2 e^{-} \longrightarrow 2 \text{Cl} ^{-}
\end{array}
\][/tex]

What should he write as the final, balanced equation?

A. [tex]\(\text{Cl}_2 + 2 \text{Br} ^{-} \longrightarrow \text{Br}_2 + 2 \text{Cl} ^{-}\)[/tex]

B. [tex]\(\text{Cl}_2 + 2 \text{Br} ^{-} + 2 e^{-} \longrightarrow \text{Br}_2 + 2 \text{Cl} ^{-}\)[/tex]

C. [tex]\(\text{Cl}_2 + 2 \text{Br} ^{-} \longrightarrow \text{Br}_2 + 2 \text{Cl} ^{-} + 2 e^{-}\)[/tex]

D. [tex]\(\text{Cl}_2 + \text{Br} ^{-} + 2 e^{-} \longrightarrow \text{Br}_2 + \text{Cl} ^{-} + 2 e^{-}\)[/tex]

Sagot :

GinnyAnswer
To balance the given redox reaction using the half-reaction method, we need to follow these steps:

1. Write the oxidation and reduction half-reactions:
- Oxidation: [tex]\(2 Br^{-} \rightarrow Br_{2} + 2 e^{-}\)[/tex]
- Reduction: [tex]\(Cl_{2} + 2 e^{-} \rightarrow 2 Cl^{-}\)[/tex]

2. Equalize the number of electrons in both half-reactions:
- Both half-reactions already have 2 electrons, so they are balanced in terms of electrons.

3. Add the half-reactions together to cancel out the electrons:
[tex]\[ (2 Br^{-} \rightarrow Br_{2} + 2 e^{-}) + (Cl_{2} + 2 e^{-} \rightarrow 2 Cl^{-}) \][/tex]

When we add these two reactions, the electrons [tex]\(2 e^{-}\)[/tex] on each side will cancel out:
[tex]\[ 2 Br^{-} + Cl_{2} + 2 e^{-} \rightarrow Br_{2} + 2 e^{-} + 2 Cl^{-} \][/tex]

4. Simplify the equation to get the final balanced reaction:
[tex]\[ Cl_{2} + 2 Br^{-} \rightarrow Br_{2} + 2 Cl^{-} \][/tex]

Thus, the final balanced equation is:
[tex]\[ Cl_{2} + 2 Br^{-} \rightarrow Br_{2} + 2 Cl^{-} \][/tex]

So, the correct answer is:
[tex]\[ Cl_{2} + 2 Br^{-} \longrightarrow Br_{2} + 2 Cl^{-} \][/tex]
We appreciate your visit. Hopefully, the answers you found were beneficial. Don't hesitate to come back for more information. Thank you for your visit. We're dedicated to helping you find the information you need, whenever you need it. We're glad you visited Westonci.ca. Return anytime for updated answers from our knowledgeable team.