The reaction was studied at a series of different temperatures. A plot of ln(k) vs. 1/T gave a straight line relationship with a slope of -693 and a y-intercept of -0.425. Additionally, a study of the concentration of A with respect to time showed that only a plot of ln[A] vs. time gave a straight line relationship. What is the initial rate of this reaction when [A] = 0.41 at 271 K?

Here is the correct question:

The reaction A → products was studied at a series of different temperatures. A plot of ln(k) vs. 1/T gave a straight line relationship with a slope of -693 and a y-intercept of -0.425. Additionally, a study of the concentration of A with respect to time showed that only a plot of 1/[A] vs. time gave a straight line relationship. What is the initial rate of this reaction when [A] = 0.41 at 271 K ?

the initial rate of this reaction is 0.0216275  M/sec

Explanation:

Using the formula:

Since vs time is a straight line relationship;

Therefore, it is a second order reaction

rate = K[A]²

rate = 5.275 × 10⁻² × (0.41)

rate = 0.0216275  M/sec

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