Nitryl fluoride is an explosive compound that can be made by oxidizing nitrogen dioxide with fluorine:
2 NO2(g) + F2(g) → 2 NO2F(g)
Several kinetics experiments, all done at the same temperature and involving formation of nitryl fluoride, are summarized in this table:
- (a) Write the rate law for the reaction.
- (b) Determine what the order of the reaction is with respect to each reactant and each product.
- (c) Calculate the rate constant k and express it in appropriate units.
(a)
Interpretation:
The rate law for the reaction has to be written.
Explanation of Solution
Suppose the rate law of the above reaction is as follows,
Where,
Carefully examining the table, it can be said that
Now, on dividing both the equations, the value of j can be found out.
Similarly, carefully examining the table, it can be said that
Now, on dividing both the equations, the value of i can be found out.
Similarly, carefully examining the table, it can be said that
Now, on dividing both the equations, the value of h can be found out.
Therefore, the rate law for the reaction is
(b)
Interpretation:
The order of the reaction with respect to each reactant and each product has to be determined.
Explanation of Solution
The rate law for the reaction is
Therefore, the order of the reaction with respect to
(c)
Interpretation:
The rate constant
Answer to Problem 95QRT
The average of the rate constant is
Explanation of Solution
The rate constant can be expressed as shown below.
For first experiment the rate constant can be calculated by plugging all the data given in the table.
In the first experiment, the initial concentration of
Now, the rate constant for first experiment is given below.
Similarly, the rate constant for rest of the experiments can be calculated. The calculated rate constant values are given in the table below.
Initial rate |
Rate constant | ||
The average of the rate constant is
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Chapter 11 Solutions
OWLv2 for Moore/Stanitski's Chemistry: The Molecular Science, 5th Edition, [Instant Access], 1 term (6 months)
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