The rate of the decomposition of hydrogen peroxide, H2O2, depends on the concentration of iodide ion present. The rate of decomposition was measured at constant temperature and pressure for various concentrations of H2O2and of KI. The data appear below. Determine the order of reaction for each substance, write the rate law, and evaluate the rate constant.
Rate | [H2OJ | [Kll |
(mL min-’) | (mol L ’) | (mol L ’) |
0.090 | 0.15 | 0.033 |
0.178 | 0.30 | 0.033 |
0.184 | 0.15 | 0.066 |
To determine:
Order of reaction of each substance, rate law and rate constant
Explanation of Solution
Let following chemical reaction
Rate law for this reaction can be written as
The rate law for the given reaction can be written as
You have given three set of data. Put each in the above equation
So,
Putting these values on equation, you get
Putting these value in equation you, get
Putting these value in equation you, get
Hence
Hence overall order of reaction
Rate law can be written as
Putting the value
Hence rate law can be written as
It is the initial rates experiment method.
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Chapter 11 Solutions
Chemistry for Engineering Students
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