When dry chlorine gas is passed through silver chlorate heated to `90^@C`, then which of the oxides of chlorine is obtained ?

Options

A. `ClO_2`
B. `Cl_2O`
C. `Cl_2O_3`
D. `Cl_2O_5`

Answer

To solve the problem, we need to analyze the reaction that occurs when dry chlorine gas is passed through silver chlorate (AgClO3) at a temperature of 90°C.

### Step-by-Step Solution:

1. **Identify the Reactants**: The reactants in this reaction are silver chlorate (AgClO3) and dry chlorine gas (Cl2).

2. **Write the Balanced Chemical Equation**: When dry chlorine gas is passed through silver chlorate, the reaction can be represented as follows:
\[ 2 \, \text{AgClO}_3 + \text{Cl}_2 \rightarrow 2 \, \text{AgCl} + 2 \, \text{ClO}_2 + \text{O}_2 \]
Here, silver chloride (AgCl), chlorine dioxide (ClO2), and oxygen gas (O2) are produced.

3. **Identify the Chlorine Oxides Produced**: From the balanced equation, we can see that one of the products is chlorine dioxide (ClO2), which is an oxide of chlorine.

4. **Conclusion**: The oxide of chlorine that is obtained from this reaction is chlorine dioxide (ClO2).

### Final Answer:
The oxide of chlorine obtained is **ClO2 (Chlorine Dioxide)**.

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