Predict product(s) in the following reaction,
`Cl_(2)+OH^(-) overset(hot)to`?

Options

A. `Cl^(-)`
B. `ClO_(2)`
C. `OC l^(-)`
D. `ClO_(3)^(-)`

Answer

To predict the products of the reaction between chlorine gas (Cl₂) and hydroxide ions (OH⁻) under hot conditions, we can follow these steps:

### Step-by-Step Solution:

1. **Identify the Reactants**: The reactants given are chlorine gas (Cl₂) and hydroxide ions (OH⁻).

2. **Determine the Reaction Conditions**: The reaction is specified to occur under hot conditions. This is important as it influences the type of reaction that will take place.

3. **Recognize the Type of Reaction**: In hot conditions, the reaction between chlorine and hydroxide ions typically leads to a disproportionation reaction. Disproportionation is a type of redox reaction where an element in a single compound is both oxidized and reduced.

4. **Assign Oxidation States**:
- In Cl₂, the oxidation state of chlorine is 0.
- In the products, we will have Cl⁻ (oxidation state -1) and ClO₃⁻ (oxidation state +5).

5. **Write the Balanced Reaction**: The balanced reaction for the disproportionation of chlorine in the presence of hydroxide ions can be written as:
\[ 3Cl_2 + 6OH^- \rightarrow 5Cl^- + ClO_3^- + 3H_2O \]
Here, chlorine gas is being converted into chloride ions (Cl⁻) and chlorate ions (ClO₃⁻).

6. **Identify the Products**: From the balanced equation, we can identify the products:
- Chloride ion (Cl⁻)
- Chlorate ion (ClO₃⁻)

### Final Answer:
The products of the reaction between Cl₂ and OH⁻ under hot conditions are:
- Cl⁻ (chloride ion)
- ClO₃⁻ (chlorate ion)