Final answer:
The rate constant k for the given reaction, which is first-order with respect to CH3CH2Cl, is calculated using the rate law rate = k[CH3CH2Cl]. From Experiment 1, we derive that k = 1.6 × 10^-6 s^-1.
Step-by-step explanation:
The value of the rate constant k for a chemical reaction can be found after determining the rate law for the reaction. In this reaction, after comparing experiments and observing how the rate changes with concentration, it is determined to follow a first-order law. A first-order reaction implies that the rate is directly proportional to the concentration of the reactant. In the example provided, the rate law expression is rate = k[CH3CH2Cl], indicating that the reaction is first-order with respect to [CH3CH2Cl].
To find the rate constant k, we can use any set of data points from the given experiments. For instance, from Experiment 1, we have:
1.60 × 10^-8 M/s = k(0.010 M)
Solving for k gives us:
1.6 × 10^-6 s^-1 = k
Thus, the rate constant k for this reaction is 1.6 × 10^-6 s^-1.