## Problem 15.99

$aR \to bP, Rate = -\frac{1}{a} \frac{d[R]}{dt} = \frac{1}{b}\frac{d[P]}{dt}$

Anne 2L
Posts: 35
Joined: Fri Sep 29, 2017 7:05 am

### Problem 15.99

Which of the following plots will be linear?

(f) initial rate against [A] for a reaction that is first 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

I'm not sure how to conceptually or mathematically determine if the plots would be linear.

Ethan-Van To Dis2L
Posts: 50
Joined: Fri Sep 29, 2017 7:05 am

### Re: Problem 15.99

F and and G are linear because if you have a first order reaction, the rate law is r=k{A} which is like y=mx. The initial rate (y) depends on the concentration (x) with a constant slope (k or m).

G is linear because if you look at the equation of the half life of a zero order, you get t1/2=$\frac{[A]}{2k}$ This here you can also consider it as y=mx, where m=1/2k and x is the initial concentration, and y is the half-life.

H isn't linear because it resembles y=1/x which is a curve