Summary
Summary - Unit 11 - Equilibrium II
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EQUILIBRIA II- I
Conc .
I
I
I rate-rate
FORWARD REACTION
- reactants intially l equilibrium dynamic equilibrium
used up
quickly and I reached Conc= constant
Slow as their I
concentration drops
I
I
I
BACKWARD REACTION-reactants intially
formed slowly and
I
speed up as ther I
concentration increases
3
time(s)
key :
~ reactants
-
products
LE CHATIER'S PRINCIPLE
If a raction at equilibria is subjected to a
change is pressure , temperative or ,
concertatio
the position of equilibra will move to contract the .
charge
SItIFT more
SHIFT To More >
- TO THE I
products
- LEFT
=
reactants RIGHT
will shift to
will shift a e
positio i
↑ essure position
the side with the fewest
MR
CATALYSTS
↳ yield
no effect on the position of equilibrium or
↳ speed up rate
↳ no effect on UC or Up
Kc EXPRESSIONS IHOMOLOGOUS Kc EXPRESSIONS /HETEROGENOUS
O(g)Ec02191
[S0 , ]
-
-
2502(g) +
02(g) = 250- [0,] [S0 ]" ,
(is) +
no solids or
pure liquids
I conc remains constant)
Mol du
-3 Kc = 1 equilibri
A + B = C =
nc = [B] = Cutan-sn =
an
=
mol" au
Kc = 100 equilibri
Uc = 0 . 01 equilibri
moles at
Start
2O .
3 0 .
O Kc = 1010 reaction
change -o 8 .
-
0 S .
+0. S ↑ temp of e Nic Uc =
10-10 reactio
equilibrin 1 2 . 2 2 . 0 S .
Kp EQUATIONS
EXAMPLE :
wA .
+
xB = y) + 2D so , Cle decomposes into SO2 and Ch under heating
.
502(2(g) = S02(g) +
(ly(g)
At equilibrium the reaction vessel contains 263upa of Cl2 . The t
in the vessel is 714kPa
.
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