For a certain reaction,a plot of ln [A] vs.time gives a straight line with a slope of -1.46 s^-1 and a y-intercept of 4.30.What is the order of the reaction?

Question

Quizplus · Accepted Answer

The slope of the ln[A] vs. time plot is equal to -k, where k is the rate constant for the reaction. Thus, -k = -1.46 s^-1, so k = 1.46 s^-1. For a first-order reaction, the rate law is ln[A] = -kt + ln[A]0, where [A]0 is the initial concentration of A. Comparing this to the equation for the line given, we can see that the slope (-k) matches, so the reaction must be first-order.

For a Certain Reaction,a Plot of Ln [A] Vs