## graph

$\frac{d[R]}{dt}=-k[R]; \ln [R]=-kt + \ln [R]_{0}; t_{\frac{1}{2}}=\frac{0.693}{k}$

Ruiting Jia 4D
Posts: 65
Joined: Fri Sep 28, 2018 12:27 am

### graph

Why is it that when graphing first order reactions, it is either exponentially decaying or linear?

almaochoa2D
Posts: 67
Joined: Fri Sep 28, 2018 12:23 am

### Re: graph

It changes based on whether it is integers or in ln form.

Samantha Kwock 1D
Posts: 61
Joined: Fri Sep 28, 2018 12:24 am

### Re: graph

For first order reactions, the graph of the concentration of reactant vs time is exponentially decaying. However, a linear plot is obtained when graphing the natural log of the reactant concentration vs time.

Lisa Werner 2F
Posts: 72
Joined: Fri Sep 28, 2018 12:17 am

### Re: graph

the actual concentration of A in first order reactions is exponentially decaying; however, we plot the y axis using ln, which gives us a linear graph with a slope