A chemistry graduate student is studying the rate of this reaction:→2Cl2O5g+2Cl2g5O2gHe fills a reaction vessel with Cl2O5 and measures its concentration as the reaction proceeds:time(seconds) Cl2O50 0.0200M10. 0.0139M20. 0.00966M30. 0.00671M40. 0.00466MUse this data to answer the following questions.Write the rate law for this reaction. rate =k Calculate the value of the rate constant k.Round your answer to 2 significant digits. Also be sure your answer has the correct unit symbol. =k

The rate law for a reaction is determined by the reaction's mechanism and can be written in the form of: Rate = k[A]^x[B]^y, where A and B are the reactants, x and y are their respective orders, and k is the rate constant.

In this case, the reaction is: 2Cl2O5(g) → 2Cl2(g) + 5O2(g)

The rate law for this reaction would be: Rate = k[Cl2O5]^x

To determine the order of the reaction with respect to Cl2O5 (x), we can use the method of initial rates. This involves comparing the rates of reaction at two different initial concentrations of Cl2O5.

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

At time 0s, [Cl2O5] = 0.0200M At time 10s, [Cl2O5] = 0.0139M

The rate of reaction at time 0s (Rate1) can be calculated as (0.0200M - 0.0139M) / 10s = 0.00061 M/s The rate of reaction at time 10s (Rate2) can be calculated as (0.0139M - 0.00966M) / 10s = 0.000424 M/s

We can then set up the following equation using the rate law:

Rate2 / Rate1 = (k[Cl2O5 at 10s]^x) / (k[Cl2O5 at 0s]^x)

Substituting the known values:

0.000424 M/s / 0.00061 M/s = ([0.0139M]^x) / ([0.0200M]^x)

Solving this equation for x will give us the order of the reaction with respect to Cl2O5.

Once we have the order of the reaction, we can substitute the known values into the rate law to solve for the rate constant k.

Please note that the units of k will depend on the order of the reaction. For a first-order reaction, the units of k are s^-1, for a second-order reaction, the units are M^-1s^-1, and so on.

This is a simplified explanation and the actual calculations may require more complex mathematical methods.

The rate law for a reaction is determined by the reaction's mechanism and can be written in the form of: Rate = k[A]^x[B]^y, where A and B are the reactants, x and y are their respective orders, and k is the rate constant.

In this case, the reaction is: 2Cl2O5(g) → 2Cl2(g) + 5O2(g)

The rate law for this reaction would be: Rate = k[Cl2O5]^x

To determine the order of the reaction with respect to Cl2O5 (x), we can use the method of initial rates. This involves comparing the rates of reaction at two different initial concentrations of Cl2O5.

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

At t = 0 s, [Cl2O5] = 0.0200 M At t = 10 s, [Cl2O5] = 0.0139 M

The rate of reaction can be calculated as the change in concentration over the change in time:

Rate1 = (0.0200 M - 0.0139 M) / (10 s - 0 s) = 0.00061 M/s Rate2 = (0.0139 M - 0.00966 M) / (20 s - 10 s) = 0.000424 M/s

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

Rate2/Rate1 = (k[Cl2O5]2^x) / (k[Cl2O5]1^x)

Substituting the known values:

0.000424 M/s / 0.00061 M/s = (0.0139 M)^x / (0.0200 M)^x

Solving this equation will give us the order of the reaction with respect to Cl2O5 (x).

Once we have the order of the reaction, we can calculate the rate constant (k) by rearranging the rate law equation and substituting the known values:

k = Rate / [Cl2O5]^x

The units of the rate constant will depend on the order of the reaction. For a first-order reaction, the units are s^-1; for a second-order reaction, the units are M^-1s^-1; and for a zero-order reaction, the units are M/s.

Please note that the above calculations are based on the assumption that the reaction is either zero, first, or second order. If the reaction order is not an integer, the calculations would be more complex and may require the use of logarithms or other mathematical techniques.