Use the information given here to answer both questions (4 and 5). For the fictitious reaction: AB → A + B Some data was collected measuring the [AB] at certain time intervals. This data was then graphed as described below. A graph of 1/[AB] versus time (s) gives a straight line with the equation: y = 0.0052x + 0.1135 and a R2 = 0.9995. A graph of ln[AB] versus time (s) gives a straight line with the equation: y = -0.0068x + 1.725 and a R2 = 0.8925. Assume the data doesn't fit a zero order reaction. What is the rate law for this reaction? Select one: a. Rate = k[AB]2 b. Rate = k[A][B] c. Rate = k[AB] d. Rate = k Using the data from the previous question. What is the value of the rate constant for the given reaction? Select one: a. k = 0.0052 M-1s-1 b. k = 0.0157 Ms-1 c. k = 0.0068 s-1 d. There is no way to determine the value of the rate constant from the given information.
Use the information given here to answer both questions (4 and 5).
For the fictitious reaction: AB → A + B
Some data was collected measuring the [AB] at certain time intervals. This data was then graphed as described below.
A graph of 1/[AB] versus time (s) gives a straight line with the equation: y = 0.0052x + 0.1135 and a R2 = 0.9995. A graph of ln[AB] versus time (s) gives a straight line with the equation: y = -0.0068x + 1.725 and a R2 = 0.8925. Assume the data doesn't fit a zero order reaction.
What is the rate law for this reaction?
Using the data from the previous question.
What is the value of the rate constant for the given reaction?
From the given information, it is clear that the graph of 1/[AB] versus time (s) gives a straight line with the equation: y = 0.0052x + 0.1135
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