le chatelier's principle rate yield compromises K expressions
↳ concentration of reactants ↑ ↳ haber process ↳ K is equilibrium constant
shifts to aA bBEcC dD
RHS N2 3H2(9) = 2NH3
+
=> =>
(9) + (g) : -
NH +
↳ concentration of products
4 => temperature decrease in yield & Ke : SDJd
( C) '
,
Shifts to CHS
=> => pressure ↑ ,
increase in yield [A]"(B) b
pressure 4 high cost
°
↳ => 450 C -
higher means low yield
=> shifts to side with fewer moles - lower means slow rate & KC of a reaction only changes if
of gas => 300atm - higher means small increase + high cost temperature changes
↳ temperature & e lower means slow rate ↳
homogeneous reactants + products are
=> shifts to endo thermic direction ↓ contact process in same physical state
↳ catalyst has no effect on equilibrium - S0219) +
E0219)
-
> SO319) : -
WH
↳ heterogeneous reactions + products
position are not in same physical state
↳ solids are ignored in K > expressions
Dynamic equilibrium - Kc 1 => equilibrium is half way
EQUI
=
↳ reactants + products are constantly 32 U ↳ K 1 => equilibrium lies On RHS
moving ↳ more product
↳ rate of toward = rate of backwards - O ↳ KC < 1 => equilibrium lies on LHS
↳ concentration of reactants + products is ↳ more reactants
constant calculations
↳ closed system
↳ 0 .
100 mol of ethylethanoate are added to 0 100
.
mol of water
. reaction conditions equilibrium constant
↳ isolated system the mixture is made up to Idm3. At equilibrium 0 0654 mol of .
water ↳ 2H((g) =H2(g) + (2(g) + WH
(H2) [12]
↳ reaction is reversible is present Calculate . Kc :
kc =
kp = P(H2) p((z)
[H1]2 2
P(H1)
CH3100CzH5 /K + H2OCK - CH3COOH(1) + CzH5OH(I)
kp expressions ni 0 100 temperature & [H2][12] increases
↓ +004) Forsted
.
0 .
100 n ,
4
↳ kp is
aA(g) + bB(g) =
equilibrium
c((g)
constant
+ dD(g)
in terms
nc
ne
-
0
0 0654
.
.
0346
↓ -
0 0346
.
0 0654
.
0 0346
.
0 6346
.
↳
CH1] decreases
works the same for kp
: KI &
partial pressure [Se 0 0654/1 0 0654/1 0 0346/, 0 0346/ & KC and kp only affected by
.
of are
. .
.
d
↳
kp P(((g)'p(D(g)
= temperature
KC [CHyCOOH] [CzH50H]
p(A(g)" P(B(g) :
: 0 0346 X0 8346
.
.
= 0 28
.
(CH310U(zHj] CH20] 0 0654
.
x 0 0654
. unitless
& for heterogeneous reaction : solids
+
liquids are ignored ↳ forkp :
P(A) =
P+ x
1
- total pressure x mole traction
n
kp only changes if temperature :
(A :
RA/H-
changes
↳ concentration of reactants ↑ ↳ haber process ↳ K is equilibrium constant
shifts to aA bBEcC dD
RHS N2 3H2(9) = 2NH3
+
=> =>
(9) + (g) : -
NH +
↳ concentration of products
4 => temperature decrease in yield & Ke : SDJd
( C) '
,
Shifts to CHS
=> => pressure ↑ ,
increase in yield [A]"(B) b
pressure 4 high cost
°
↳ => 450 C -
higher means low yield
=> shifts to side with fewer moles - lower means slow rate & KC of a reaction only changes if
of gas => 300atm - higher means small increase + high cost temperature changes
↳ temperature & e lower means slow rate ↳
homogeneous reactants + products are
=> shifts to endo thermic direction ↓ contact process in same physical state
↳ catalyst has no effect on equilibrium - S0219) +
E0219)
-
> SO319) : -
WH
↳ heterogeneous reactions + products
position are not in same physical state
↳ solids are ignored in K > expressions
Dynamic equilibrium - Kc 1 => equilibrium is half way
EQUI
=
↳ reactants + products are constantly 32 U ↳ K 1 => equilibrium lies On RHS
moving ↳ more product
↳ rate of toward = rate of backwards - O ↳ KC < 1 => equilibrium lies on LHS
↳ concentration of reactants + products is ↳ more reactants
constant calculations
↳ closed system
↳ 0 .
100 mol of ethylethanoate are added to 0 100
.
mol of water
. reaction conditions equilibrium constant
↳ isolated system the mixture is made up to Idm3. At equilibrium 0 0654 mol of .
water ↳ 2H((g) =H2(g) + (2(g) + WH
(H2) [12]
↳ reaction is reversible is present Calculate . Kc :
kc =
kp = P(H2) p((z)
[H1]2 2
P(H1)
CH3100CzH5 /K + H2OCK - CH3COOH(1) + CzH5OH(I)
kp expressions ni 0 100 temperature & [H2][12] increases
↓ +004) Forsted
.
0 .
100 n ,
4
↳ kp is
aA(g) + bB(g) =
equilibrium
c((g)
constant
+ dD(g)
in terms
nc
ne
-
0
0 0654
.
.
0346
↓ -
0 0346
.
0 0654
.
0 0346
.
0 6346
.
↳
CH1] decreases
works the same for kp
: KI &
partial pressure [Se 0 0654/1 0 0654/1 0 0346/, 0 0346/ & KC and kp only affected by
.
of are
. .
.
d
↳
kp P(((g)'p(D(g)
= temperature
KC [CHyCOOH] [CzH50H]
p(A(g)" P(B(g) :
: 0 0346 X0 8346
.
.
= 0 28
.
(CH310U(zHj] CH20] 0 0654
.
x 0 0654
. unitless
& for heterogeneous reaction : solids
+
liquids are ignored ↳ forkp :
P(A) =
P+ x
1
- total pressure x mole traction
n
kp only changes if temperature :
(A :
RA/H-
changes
