2 ClO2(aq) + 2 OH (aq) → ClO3°(aq) + CIO2°(aq) + H201) [CI02]o (mol/L) [ОН 10 (mol/ L) Initial Rate (mol/L*s) 0.150 0.200 5.75 x 10-2 0.300 0.200 2.30 x 10-1 0.300 0.100 1.15 х 10-1 а. Determine the rate law and the value of the rate constant b. What would the initial rate be for an experiment with [CIO2]o = 0.350 mol/L and [OH-]o = 0.169 mol/L? %3D
Catalysis and Enzymatic Reactions
Catalysis is the kind of chemical reaction in which the rate (speed) of a reaction is enhanced by the catalyst which is not consumed during the process of reaction and afterward it is removed when the catalyst is not used to make up the impurity in the product. The enzymatic reaction is the reaction that is catalyzed via enzymes.
Lock And Key Model
The lock-and-key model is used to describe the catalytic enzyme activity, based on the interaction between enzyme and substrate. This model considers the lock as an enzyme and the key as a substrate to explain this model. The concept of how a unique distinct key only can have the access to open a particular lock resembles how the specific substrate can only fit into the particular active site of the enzyme. This is significant in understanding the intermolecular interaction between proteins and plays a vital role in drug interaction.
The following data were obtained for the reaction:
![### Reaction and Experimental Data
The chemical reaction under study is:
\[ 2 \text{ClO}_2(aq) + 2 \text{OH}^-(aq) \rightarrow \text{ClO}_3^-(aq) + \text{ClO}_2^-(aq) + \text{H}_2\text{O}(l) \]
#### Experimental Data Table:
| \([\text{ClO}_2]_0\) (mol/L) | \([\text{OH}^-]_0\) (mol/L) | Initial Rate (mol/L\*s) |
|------------------------------|-----------------------------|-------------------------|
| 0.150 | 0.200 | \(5.75 \times 10^{-2}\) |
| 0.300 | 0.200 | \(2.30 \times 10^{-1}\) |
| 0.300 | 0.100 | \(1.15 \times 10^{-1}\) |
### Problems to Solve:
a. **Determine the rate law and the value of the rate constant.**
b. **Calculate the initial rate for an experiment with \([\text{ClO}_2]_0 = 0.350 \, \text{mol/L}\) and \([\text{OH}^-]_0 = 0.169 \, \text{mol/L}\).**
### Explanation of the Table:
The table presents the initial concentrations of the reactants, \([\text{ClO}_2]_0\) and \([\text{OH}^-]_0\), along with the observed initial reaction rates. This data is used to determine the reaction's rate law, which explains how the reaction rate depends on the concentration of reactants. By analyzing the changes in concentration and corresponding rates, one can deduce the order of the reaction for each reactant and calculate the rate constant.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fdd238cd0-c9a3-4ed0-beef-ef3a3d7f045e%2F47bb42a4-b6d6-4b7e-8b62-34774b1a1c90%2Fz4wy0p7_processed.png&w=3840&q=75)
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