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17-1
Kinetics applies to the speed of a reaction, the concentration of product that appears (or of reactant that disappears) per unit time.
Equilibrium applies to the extent of a reaction, the concentration of product that has appeared after an unlimited time, or once no further change occurs.
At equilibrium:
rateforward = ratereverse
A system at equilibrium is dynamic on the molecular level; no further net change is observed because changes in one direction are balanced by changes in the other.
17-2
Reaching equilibrium on the macroscopic and molecular levels.
N2O4(g)
17-3
2NO2(g)
Equilibrium ≠ Equal
• the rates of the forward and reverse reactions are equal at equilibrium
• …ver más…
SOLUTION:
[NO2]4[O2]
(a) 2 N2O5(g) ⇌ 4 NO2(g) + O2(g)
Qc =
[N2O5]2
[CO2]3[H2O]
(b)
17-8
C3H8(g) +
5O2(g)
⇌
3CO2(g) +
4H2O(g)
Qc =
[C3H8][O2]5
4
Q - The Reaction Quotient
At any time, t, the system can be sampled to determine the amounts of reactants and products present.
Q is calculated in the same manner as K c [D]d
[A]
Q=
[C]
a
[B]b
We use the molar concentrations of the substances in the reaction. This is symbolised by using square brackets - [ ].
For a general reaction aA + bB ⇌ cC + dD where a, b, c, and d are the numerical coefficients in the balanced equation, Q
(and K) can be calculated as
17-9
Calculating Variations on Q and K
aA + bB ⇌ cC + dD
[C] c [D]d
Qc =
[A]a [B]b
cC + dD ⇌ aA + bB
Q’ =
1
Qc
n
aA + bB ⇌ cC + dD
Qc’ = (Qc)n
For a sequence of equilibria, Qoverall = Q1 x Q2 x Q3 x …
17-10
Sample Problem 17.2
Writing the Reaction