BASIC PRINCIPLES

Review

For the experimentally determined rate of reaction, r = k[F•][H₂], the units of the rate constant (k) will be dm³ mol^-1 s^-1.

Zero, First and Second Order Reactions

Order	Example	Rate Equation	Integrated Rate Equation	Units of k
0	-	d[A]/dt = -k	[A]0 - [A]t = kt	mol dm-3 s-1
1	A → B	d[A]/dt = -k[A]	ln([A]0/[A]t) = kt	s-1
2	2A → B	d[A]/dt = -2k[A]2	(2[A]t)-1 - (2[A]0)-1 = kt	dm3 mol-1 s-1

Review Question

The Rate Constant (k), can be determined from the Slope of a plot of ln([A]_t) versus Time, for a

Zeroth Order Reaction

First Order Reaction

Second Order Reaction