It looks like the question asks you to **determine the rate law** for the reaction: \[ \text{CO} + \text{Cl}_2 \rightarrow \text{COCl}_2 \] at 300 K, using initial rates data for different initial pressures of the reactants. However, the image does **not include the actual data table** (the initial pressures and corresponding rates), which is essential for solving the problem. **Could you please provide the table or the data?** Once you share the data, I will break down the steps and explain each step with reasoning, then give the final answer. --- **General Steps (to be used once data is available):** 1. **Write the general rate law:** \( \text{Rate} = k[\text{CO}]^m[\text{Cl}_2]^n \) 2. **Compare experiments:** Use the given data to compare experiments where only one reactant concentration changes, to determine the order with respect to each reactant. 3. **Calculate the exponents (m and n):** Use ratios of rates and concentrations to solve for m and n. 4. **Write the final rate law:** Substitute the values of m and n into the general rate law. --- **Please send the table/data, and I'll provide a stepwise solution!**