From the information in the table, determine the experimental rate law for the reaction in number 1
Experiment number
[NO]initial (M)[H2]initial (M) Initial rate (M/s)
1 0.1 0.1 1.23E10-3
2 0.1 0.2 2.46E-03
3 0.2 0.1 4.92E-03
a. r = k [NO]3 [H2] b. k [NO]2 [H2] c. k [NO]3 [H2]2 d. k [NO]3 [H2]3
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From the information in the table, determine the experimental rate law for the reaction in number 1
exp # [NO2]initial [H2]initial initial m/s
1 .1 .1 1.23*10^-3
2 .1 .2 2.46E-3
3 .2 .1 4.92E-3
To determine the experimental rate law for the reaction in question 1, we can compare the initial rates of the reaction under different initial concentrations of the reactants. By examining the table, we can see that the initial rate doubles when the initial concentration of [H2] is doubled while keeping the initial concentration of [NO] constant. This suggests that the rate of the reaction is directly proportional to the concentration of [H2].
Given that the initial rate is directly proportional to [H2], we can eliminate answer choice d since it suggests that the rate is proportional to [H2] cubed. Similarly, answer choice b suggests that the rate is proportional to [NO] squared, which contradicts the fact that the rate is only directly proportional to [H2].
Next, we can compare the initial rates when the initial concentration of [NO] is doubled while keeping the initial concentration of [H2] constant. We can see that the initial rate increases by a factor of 4, which suggests that the rate is proportional to the concentration of [NO] squared.
Based on this analysis, we can conclude that the experimental rate law for the reaction in number 1 is:
r = k [NO]² [H2]
Therefore, the correct answer is c. k [NO]³ [H2]².