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Summary Equilibrium HL IB
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EQUILIBRIUMTopic position of equilibrium
:
Le Chatelier's
principle if a system at equilibrium -
is subjected to change the position of equilibrium,
will shift in order to minimize the
change
3He(g) +
Ne(g) = 2NH3
1 .
Change in pressure
-if NH3
increases
volume of container is reduced , pressure
4 mol of gas 2md of gas
then position of equilibrium shifts to the right
hand side-forward reaction is faster than reverse
reaction
?
wat It
There are less gaseous moles on right hand
side of the reaction
Questions :
1) a) 3 = 5 -
left
2 = 3 -
left
2 1- right
, 2 .
Change in temperature
- produces heat
3H2(g) +
N2(g) NHL -0
/
absorbs heat
R
~ 25 Increasing temperature shifts equilibrium
to left hand side because
:
75 C reverse
↑ ↑
hot water added reaction is endothermic
Questions :
2) a) Rop-left
b) pendop-right
c) Rop-left
3
. Adding or removing substances
3H2(g) +
N2(g) >
-
2NH3 (g)
-
add reactants , equilibrium - NH3
>
N2- NH3
shifts to the
right HINs At lava
~
-
, equilibrium
add products
shifte to the left
2-
MSOsiag)
+
H gr-(aq) + SO3
removing H so equilibrium
+
NaOH added
T
x
H2O
shifts to the right
, Questions :
3) a) CaCO3(s) Ca0(s) + Ca(g)-right
b) NHy"--H ++ NH3-left
c) CHyCOON (aq) *
CHzCOag) Minal-right
+
d) 312(aq) +
3H20() = 5HI(ag) + HIOz (aq) adding NaOH
-
right
Catalyst speeds both reactions by the same
factor -
does not affect equilibrium
Topic Reversible reactions
:
·
Chemical reactions
[
<(g)
+
Hz(g) >
-
2HI(g) He HI Reversible reaction can
Ha
towards reactants
En occur
HI +
,g
HI(
g
>
-
F2(g) Ha(g)
+ and products
.
All reactions in closed systems are reversible
forward
= 2HI
Fx(g) +
H2(g)reverse/backward
Dynamic equilibrium
- forward and reverse
reactions have the same rate (the rate is equal)
-
concentrations of reactants and products do not change
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