Question

If plotting `ln[A]` vs. time gives a straight line, what is the order of reaction?

Answer 1

You may want to re-read this...

What is the value for the rate constant `k` at this temperature?

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Well, a default rate law would include the reactant(s) in the reaction

`A -> B + C`

and so, one would write

`r(t) = k[A]^m`

as a first guess. And we know that the first-order integrated rate law is

`overbrace(ln[A])^(y) = overbrace(-k)^(m)overbrace(t)^(x) + overbrace(ln[A]_0)^(b)`,

with `[A]` being the concentration of reactant `A` at time `t`, and `k` being the rate constant. `[A]_0` is then the initial concentration of `A` at time zero.

Since using the first-order integrated rate law by plotting `ln[A]` vs. `t` yielded a straight line, this reaction has a rate law of:

`color(blue)(r(t) = k[A])`

because we know `m = 1` at this point. What therefore does `m` signify?