CHEMISTRY COMMUNITY

Which of the following plots will be linear?
(a) [A] against time for a reaction that is first order in A;
(b) [A] against time for a reaction that is zero order in A;
(c) ln[A] against time for a reaction that is first order in A;
(d) 1/[A] against time for a reaction that is second order in A;
(e) k against temperature;
(f) initial rate against [A] for a reaction that is fi rst order in A;
(g) half-life against [A] for a reaction that is zero order in A;
(h) half-life against [A] for a reaction that is second order in A.

How do I go about answering this question? Thanks in advance!

For a majority of these, you can look at the corresponding formula on the formula sheet, and if the formula is in a y=mx+b form, you know it will be linear. For instance, B is linear because [R]=-kt + [R](initial) because this fits the y=mx+b form for [R] against time regarding a zero-order reaction.

However, A in not linear because a first order reaction follows the form y=mx+b when we compare ln[R] with time, not just [R] with time since the integrated rate law for first order is ln[R]=-kt+ln[R](initial)