Which of the following oxides of chlorine is obtained by passing dry chlorine over silver chlorate at `90^(@)C`.

Options

A. `Cl_(2)O`
B. `ClO_(3)`
C. `ClO_(2)`
D. `ClO_(4)`

Explanation

To determine which oxide of chlorine is obtained by passing dry chlorine over silver chlorate at 90°C, we can follow these steps:

### Step 1: Identify the Reactants
We are given silver chlorate, which has the chemical formula AgClO3, and dry chlorine, which is represented as Cl2.

### Step 2: Write the Reaction
When dry chlorine (Cl2) is passed over silver chlorate (AgClO3) at a temperature of 90°C, a chemical reaction occurs. The reaction can be represented as follows:

\[ \text{AgClO}_3 + \text{Cl}_2 \rightarrow \text{AgCl} + \text{ClO}_2 + \text{O}_2 \]

### Step 3: Identify the Products
From the reaction, we can see that the products formed are:
- Silver chloride (AgCl)
- Chlorine dioxide (ClO2)
- Oxygen (O2)

### Step 4: Determine the Oxide of Chlorine
Among the products formed, we need to identify the oxide of chlorine. The oxide of chlorine produced in this reaction is ClO2.

### Step 5: Conclusion
Thus, the oxide of chlorine obtained by passing dry chlorine over silver chlorate at 90°C is ClO2.

### Final Answer
The correct answer is **ClO2** (Option C).

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