BASIC PRINCIPLES

Hint

The units of k depend on the order of the reaction.
The units of the rate of reaction are always mol dm^-3 s^-1.
The units of concentration are mol dm^-3.

Example:

For the experimentally determined rate of reaction, r = k[CH₃NC]

Units{r} = Units{k} x Units{Concentration of CH₃NC}

mol dm^-3 s^-1 = Units{k} x mol dm^-3

Units{k} = mol dm^-3 s^-1 / mol dm^-3 = s^-1

Review Question

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

mol dm^-3 s^-1

mol dm^-3

s^-1