- 1 d[A] = - 1 d[B] = 1 d[C] = 1 d[D] - ---- - ---- - ---- - ---- a dt b dt c dt d dtThe "d" prefix means the change in concentration or time.
Order of Component:
The order of a component is the power to which the
concentration of the component is raised in the rate law
equation. The order tells us the extent to which the reaction
depends on the concentration of a particular component.
Calculating simple orders:
(rateh/ratel) = order for 1st order and some
(conch/concl) second order reactions
A general equation to calculate orders:
We know the the ratio of the rates is related to the ratio of
the concentrations by:
(rateh/ratel) = (conch/concl)N
where N = the order for the particular component.
taking logarithms:
log(rateh/ratel) = N·log(conch/concl)
solving for N:
N = log(rateh/ratel)
log(conch/concl)
This equation will work for all orders of reaction including
zeroth orders.
Examples:
1. H+(aq) + OH-(aq) ---> H2O(l)
[H+] M | rate M min-1 |
1.0 | 1.0 x 10 -4 |
2.0 | 1.0 x 10 -4 |
Using equation above:
N = log{(1.0 x 10-4)/(1.0 x 10-4)}
log(2.0/1.0)
= log(1) = 0 = 0 so order of reaction wrt log(2) 0.301 [H+] is zeroth.2. H2O2(l) ---> H2O(l) + 1/2 O2(g)
[O2] M | rate M min-1 |
0.5 | 1.0 x 10 -6 |
1.0 | 2.0 x 10 -6 |
N = log{(2 x 10-6)/(1 x 10-6)}
log(1.0)/0.5)
= log(2) = 0.301 = 1 so order of reaction wrt log(2) 0.301 [O2(g)] is first.3. NOBr(g) ---> 2NO(g) + Br2(g)
[NOBr] M | rate M min-1 |
0.20 | 0.80 |
0.80 | 12.80 |
N = log(12.80/0.80)
log(0.80/0.20)
= log(16) = 1.204 = 2 so order of reaction wrt log(4) 0.602 [NOBr(g)] is second.Using the Rate Law