Question

Assume a reaction takes place in a basic solution to form the given products:MnO4–(aq) + Cl–(aq) --> MnO2(s) + Cl2(g) (unbalanced). Do each step individually:1. Balance the given half-reactions for atoms and charge.MnO4– + H2O -->MnO2 + OH– andCl– --> Cl2.2. Multiply to balance the charges in the reaction.3. Add the equations and simplify to get a balanced equation.

Answer 1

To balance the given redox reaction in a basic solution, follow these steps: balance the atoms and charges in each half-reaction, multiply each half-reaction by a factor that will make the total charge on each side of the equation equal, and add the two balanced half-reactions to obtain the final balanced equation. If the reaction takes place in a basic solution, add OH- ions to both sides of the equation to neutralize H+ ions.

Step-by-step explanation:

To balance the given redox reaction in a basic solution, follow these steps:

Balance the atoms and charges in each half-reaction.

Multiply each half-reaction by a factor that will make the total charge on each side of the equation equal.

Add the two balanced half-reactions to obtain the final balanced equation.

If the reaction takes place in a basic solution, add OH- ions to both sides of the equation to neutralize H+ ions.

For the given reaction:

MnO4–(aq) + Cl–(aq) → MnO2(s) + Cl2(g)

The balanced half-reactions are:

Oxidation: MnO4– + H2O → MnO2 + OH-

Reduction: 2Cl– → Cl2 + 2e-

Adding the half-reactions and simplifying gives the final balanced equation:

MnO4– + 2Cl– + H2O → MnO2 + Cl2 + OH-

Answer 2

Explanations:

What is redox reaction?

Redox reaction is the reaction that occurs between an oxidizing and reducing substrates.

Given the chemical equation below;

`MnO_4^-(aq)+Cl^-\rightarrow MnO_2(s)+Cl_2(g)`

Separate into half reactions

`\begin{gathered} MnO_4^-\rightarrow MnO_2 \\ Cl^-\rightarrow Cl_2 \end{gathered}`

1) Balance the charges by adding the equivalent electrons

`\begin{gathered} MnO_4^-+2H_2O+3e^-\rightarrow MnO_2+4OH^- \\ 2Cl^-\rightarrow Cl_2+2e^- \end{gathered}`

2) Multiply to balance the charge

3) Add the equations and simplify to get a balanced equation to have;

`6Cl^-(aq)+2MnO_4^-(aq)+4H_2O(l)\rightarrow3Cl_2(g)+2MnO_2(s)+8OH^-(aq)`

This gives the balanced equation.