mol dm^-3 s^-1

rate = the rate of the reaction

k = the rate constant

[A] = the concentration of reactant A

m = the reaction order with respect to reactant A

[B] = the concentration of reactant B

n = the reaction order with respect to reactant B

The overall order is the sum of the reaction orders for all reactants in the rate equation.

The order of a reaction specifies how the concentration of a particular reactant affects the rate of the reaction.

It is denoted by the exponent in the rate equation for that reactant.

The units for the rate constant (k) depend on the overall order of the reaction.

The units of k are s^-1 for a first order reaction, and mol^-1 dm³ s^-1 for a second order reaction.

A rate equation shows how the rate of a chemical reaction depends on the concentrations of the reactants.

The rate of reaction is independent of the reactant concentration.

Changing the reactant concentration has no effect on the rate.

The rate of reaction is directly proportional to the reactant concentration.

Doubling the reactant concentration doubles the rate.

k

Increasing the temperature increases the value of the rate constant.

The rate of reaction is proportional to the square of the reactant concentration.

Doubling the reactant concentration quadruples the rate.

The rate constant increases exponentially as temperature increases. 

For many reactions, the rate constant doubles for each 10°C rise in temperature.