The rate law for a reaction is determined by the reaction's mechanism and is generally of the form: rate = k[A]^m[B]^n, where A and B are the reactants, m and n are their respective orders, and k is the rate constant.

In this case, the reaction is: ClCH2CH2Cl - CH2CHCl + HCl. Since there is only one reactant (ClCH2CH2Cl), the rate law is: rate = k[ClCH2CH2Cl]^n.

To determine the order of the reaction (n), we can use the method of initial rates. This involves comparing the rate of reaction at two different concentrations of the reactant.

Let's use the data from time 0 and time 10 seconds:

At time 0, [ClCH2CH2Cl] = 0.800 M.
At time 10, [ClCH2CH2Cl] = 0.359 M.

The rate of reaction is the change in concentration over the change in time. So, the rate at time 0 is (0.800 - 0.359) M / 10 s = 0.0441 M/s, and the rate at time 10 is (0.359 - 0.232) M / 10 s = 0.0127 M/s.

Now, we can set up the following equation using the rate law:

0.0441 = k(0.800)^n
0.0127 = k(0.359)^n

Dividing the first equation by the second gives:

(0.0441 / 0.0127) = (0.800 / 0.359)^n

Solving for n gives a value close to 1, so this is a first-order reaction. Therefore, the rate law is: rate = k[ClCH2CH2Cl].

To find the rate constant k, we can use the rate law and the data from any time point. Let's use time 0:

0.0441 = k(0.800)

Solving for k gives k = 0.0441 / 0.800 = 0.0551 s^-1.

So, the rate constant k is approximately 0.055 s^-1, rounded to two significant digits.

Question

The rate law for a reaction is determined by the reaction's mechanism and is generally of the form: rate = k[A]^m[B]^n, where A and B are the reactants, m and n are their respective orders, and k is the rate constant.

In this case, the reaction is: ClCH2CH2Cl -> CH2CHCl + HCl. Since there is only one reactant (ClCH2CH2Cl), the rate law is: rate = k[ClCH2CH2Cl]^n.

To determine the order of the reaction (n), we can use the method of initial rates. This involves comparing the rate of reaction at two different concentrations of the reactant.

Let's use the data from time 0 and time 10 seconds:

At time 0, [ClCH2CH2Cl] = 0.800 M.
At time 10, [ClCH2CH2Cl] = 0.359 M.

The rate of reaction is the change in concentration over the change in time. So, the rate at time 0 is (0.800 - 0.359) M / 10 s = 0.0441 M/s, and the rate at time 10 is (0.359 - 0.232) M / 10 s = 0.0127 M/s.

Now, we can set up the following equation using the rate law:

0.0441 = k(0.800)^n
0.0127 = k(0.359)^n

Dividing the first equation by the second gives:

(0.0441 / 0.0127) = (0.800 / 0.359)^n

Solving for n gives a value close to 1, so this is a first-order reaction. Therefore, the rate law is: rate = k[ClCH2CH2Cl].

To find the rate constant k, we can use the rate law and the data from any time point. Let's use time 0:

0.0441 = k(0.800)

Solving for k gives k = 0.0441 / 0.800 = 0.0551 s^-1.

So, the rate constant k is approximately 0.055 s^-1, rounded to two significant digits.

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