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To write the rate law for the given reaction, we need to consider that the reaction represents an elementary step. For an elementary reaction, the rate law can be written directly from the stoichiometry of the reactants.

Given reaction:
\[ \text{SO}_2\text{Cl}_2 \rightarrow \text{SO}_2 + \text{Cl}_2 \]

For this elementary step, the rate law is:
\[ \text{Rate} = k[\text{SO}_2\text{Cl}_2] \]

where \( k \) is the rate constant and \([\text{SO}_2\text{Cl}_2]\) is the concentration of the reactant \(\text{SO}_2\text{Cl}_2\).

Do you need more details or have any questions?

Here are 5 related questions you might find helpful:
1. How is the rate constant \( k \) determined experimentally?
2. What is the difference between an elementary reaction and a complex reaction?
3. How does the order of reaction relate to the rate law?
4. Can the rate law for a complex reaction be determined from the stoichiometry?
5. What factors affect the rate constant \( k \)?

**Tip:** When writing rate laws for elementary reactions, the exponents in the rate law are equal to the stoichiometric coefficients of the reactants.

Explore the rate law for elementary chemical reactions with a focus on stoichiometry and rate constants. This problem involves deriving the rate law equation for a given reaction, providing insights into chemical kinetics and reaction rates.

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