For the reaction cyclopropane(g) → propene(g) at 500◦C, a plot of ln[cyclopropane] vs t gives
a straight line with a slope of −0.00067 s−1
.
What is the order of this reaction and what is
the rate constant?
To determine the order of the reaction and the rate constant, we need to use the given information about the plot of ln[cyclopropane] vs t.
The rate law for a reaction can be written as:
rate = k [cyclopropane]^n
where:
rate is the rate of the reaction
k is the rate constant
[cyclopropane] is the concentration of cyclopropane
n is the order of the reaction
From the given information, we know that the plot of ln[cyclopropane] vs t gives a straight line with a slope of -0.00067 s^-1. This slope, -0.00067 s^-1, represents the value of k.
Since the plot of ln[cyclopropane] vs t gives a straight line, we can determine the order of the reaction by looking at the coefficient in front of [cyclopropane] in the rate law equation. In this case, the coefficient is 1 (as it is not explicitly stated in the question).
Therefore, we can conclude that the reaction is first order. Hence, the order of the reaction is 1 and the rate constant is -0.00067 s^-1.