The following data was collected for the reaction CO + Cl2 → COCl2
   Experiment
 [CO]
 [Cl2]
 Initial rate (M/s)
   1
 0.0100
 0.0100
 6.6 x 103
   If CO is first order and Cl2 is second order, calculate the value of the rate constant, k. Enter your answer with no units.

The rate law for the reaction \( \text{CO} + \text{Cl}_2 \rightarrow \text{COCl}_2 \) can be written as:

\[
\text{Rate} = k [\text{CO}]^1 [\text{Cl}_2]^2
\]

Given:
- \(\text{Rate} = 6.6 \times 10^{-3} \, \text{M/s}\)
- \([\text{CO}] = 0.0100 \, \text{M}\)
- \([\text{Cl}_2] = 0.0100 \, \text{M}\)

We can substitute these values into the rate law equation to solve for \( k \).

\[
6.6 \times 10^{-3} = k \times (0.0100)^1 \times (0.0100)^2
\]

Calculating \( (0.0100)^1 \) and \( (0.0100)^2 \):

\[
6.6 \times 10^{-3} = k \times 0.0100 \times 0.0001
\]

Now, multiply \(0.0100\) and \(0.0001\):

\[
6.6 \times 10^{-3} = k \times 1 \times 10^{-6}
\]

Finally, solve for \( k \):

\[
k = \frac{6.6 \times 10^{-3}}{10^{-6}} = 6.6 \times 10^{3}
\]

So, the value of the rate constant \( k \) is:

\[
\boxed{6.6 \times 10^{3}}
\]

---

Would you like a more detailed breakdown of any step, or do you have further questions?

1. How is the order of a reaction determined experimentally?
2. What are the units of a rate constant for different reaction orders?
3. How does the rate constant \( k \) change with temperature?
4. What is the significance of a reaction being first order in one reactant and second order in another?
5. Can this method of calculating \( k \) be used for reactions of any order?

**Tip:** Always check the units to ensure they align with the expected reaction order.

The following data was collected for the reaction CO + Cl2 → COCl2: [CO] = 0.0100, [Cl2] = 0.0100, Initial rate (M/s) = 6.6 x 10^3. If CO is first order and Cl2 is second order, calculate the value of the rate constant, k. Enter your answer with no units.

Explore the calculation of the rate constant k for the reaction CO + Cl2 → COCl2. Given initial concentrations of CO and Cl2, and an initial rate of 6.6 x 10^3 M/s, learn how to derive k using the rate law. This solution is suitable for advanced chemistry students.

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