1. equilibrium expression a) CH4(g) + 2O2 (g)
CO2 (g) + 2H2O (l)
b) P4(g) + 5O2 (g)
P4O10 (s)
c) BaSO3 (s)
BaO (s) + SO2 (g)
d) CH4(g) + Cl2 (g)
CH3Cl (g) + HCl (l)
2. !"#$%
& # reaction
quotient (
()(
*
+*
,-
a) 2SO3(g)
2SO2 (g) + O2 (g) (K = 0.230), [SO3] = 0 M, [SO2] = 1.00 M, [O2] = 1.00 M
b) 2SO3(g)
2SO2 (g) + O2 (g) (Kp = 16.5), P *: SO3 = 1.00, SO2 = 1.00, O2 = 1.00
atm
2NOCl (g) (K = 4.6 x 104), [NO] = 1.00 M, [Cl2] = 1.00 M, [NOCl] = 0
c) 2NO (g) + Cl2 (g)
M
d) N2(g) + O2 (g)
2NO (g) (Kp = 0.050), P *: NO = 10.0 atm, N2 = O2 = 5.0 atm
3. SO3(g)
SO2(g) + O2(g), ∆H = 600 kJ # SO3 *
*
a) +*
. Ar
b) -#",
c) "
/
4. 0
-1
2
1 . 3"
/ 1 +
(*-
1/3 (
.* #
K CH3CH2OH (aq) + CH3COOH (aq)
CH3COOCH2CH3 (aq) + H2O (l)
5. 4
,
CH4 (g) + H2O (g)
CO (g) + 3H2 (g) *
0
a) H2O (g) is removed
b) The temperature is increased
c) An innert gas is added
d) CO (g) is removed
6. K (* 427 oC & Na2O (s)
2Na (l) + ½O2 (g)
K1 = 2 x 10-25
NaO (g)
Na (l) + ½O2 (g)
K2 = 2 x 10-5
Na2O2 (s)
2Na (l) + O2 (g)
K3 = 5 x 10-29
NaO2 (s)
Na (l) + O2 (g)
K4 = 3 x 10-14
#
K a) Na2O (s) + ½O2 (g)
Na2O2 (s)
b) NaO (g) + Na2O (s)
Na (l) + Na2O2 (s)
c) 2NaO (g)
Na2O2 (s)
7. * !
H2 (*- 3 41.38 kJ + H2 (g) + CO2 (g)
H2O (g) + CO (g)
a. CO2
d. H2O
b. e. +*-#",
c. "
/
8. (*-
(*-#",
4 4 ,
H2 (g) + I2 (g)
2HI (g)
Kc = 66.9 (* 350 oC = 50.0 (*
450 oC
9. +
#
N2O4 (g)
2NO2 (g) (* 50 oC 3"
/ 1 L (*-+
NO2 =
0.20 mol N2O4 = 2.00 mol
9.1 #
K ( 0.020)
9.2 0
+* N2O4 # 1.0 mol "
/ #
. NO2 N2O4 *
,-35* ( NO2 = 0.24 mol N2O4 = 2.98 mol)
3C (g)
10. A (s) + 2B (g)
a. *3 A 1.00 mol B 2.50 mol 3"
/ 2.0 L * ,- +
[C] = 0.75
mol/L Kc ( Kc= 0.75)
b. C (*-3 0
3 A 1.00 mol B 10.0 mol 3 a ( [C] = 1.50
mol/L)
1. ,
NH3 (aq) + HF (aq)
NH4+ (aq) + F- (aq)
2. 3%5* [H+] 3.2 x 10-4 M *I(5*+
[H+] 1.0 x 10-3 M pH
%I3 I( (3.0)
3. # pH 2 1.0 mol/L (* 25 0C Ka = 1.81 x10-5
(2.38, 0.42)
4. pH 0.100 M HA (
2.85 Ka (2.0 x 10-5)
5. # 0.60 M HF (Ka = 7.1 x 10-4 ) (3.4 %)
6. # pH NH3 0.01M 25* 4.0% (10.6)
7. X(OH)2 0.1M 10% # Kb (4.44 x 10-5)
8. H2CO3 0.1M 200 cm3 (
KOH 0.2M 300 cm3 ,#% * mol/L # pH (!" KOH 0.04 M, pH = 12.6)
9. *
*
4 *
a) KNO3
b) NH4NO3
c) KCN
d) NH4CN
10. # % hydrolysis KCN 0.1 M Ka HCN = 4.8 x 10-10
11. #
3
(* CaCO3 .3/
2 g 20 mL HCl 1.0M 20 mL ef5 -
5
100 mL 10 mL ((
NaOH 0.1M .3/ methyl orange 4% j
3/ NaOH 10
mL %/wt CaCO3 3
12. # pH ee%(*
HCN 0.005 . KCN 0.005 . 3
500 cm3 (Ka KCN = 5x10-10)
13. # pH ee% NH3 0.2M NH4Cl 0.4M (Kb NH3 = 1.8 x 10-5)
14. 3/ NaOH *! NH4Cl 5.35 g +*4
ee% pH 9 500 cm3
)**+*,
1. Mg(OH)2 3
0.00912 g/L (* 25oC Ksp Mg(OH)2
2. Ksp PbSO4 = 1.6 x 10-8 (* 25oC (
PbSO4 0 3
* mol/L (* 25oC
3. 03
a) BaSO4 (Ksp = 1.0 x 10-10 ) AgCl (Ksp = 1.8 x 10-10) ZnS (Ksp = 1.6 x 10-23)
b) CuS (Ksp = 8.5 x 10-45 ) Ag2S (Ksp = 1.6 x 10-49) Bi2S3 (Ksp = 1.1 x 10-73)
4. #
Ksp Bi2S3 25*
(*-#", 25°C (
1.0 x 10-15 mol/L
5. PbF2 (*-#", 25°C (
0.53 g/L #
Ksp * PbF2
6. #
(mol/L) SrCO3 3
*
Ksp SrCO3 = 9.3x10-10
7. 3 Ksp AgCl (
1.7x10-10 AgCl (*
! 0.005 mol/L
AgNO3 100 cm3 0.005 mol/L NaCl 400 cm3 #!,#!
8. !3 7 9. 3
(*
!-
.(* 10. (*-
a) Ag3PO4
b) Fe3(PO4)2
c) Ca(IO3)2
d) Li2CO3
11. #
PbCl2 3
(* 25 oC (Ksp = 1.7 x 10-5)
PbCl2
Pb2+ +
2Cl12. #
PbCl2 3 1.00 M HCl
13. * 0
0.01M NaCl 3
* AgCl
-,: 1. Ksp = 1.55 x 10-11 2. 1.26 x 10-4
3. a) AgCl > BaSO4 > ZnS b) Bi2S3 > Ag2S >
-73
-8
CuS
4. 1.1 x 10
5. 4.0x10
6. 3.05x10-5 mol/L 7. 4.0x10-6 8. 10.
a) Ksp = [Ag+]3[PO43-] c) Ksp = [Ca2+][IO3-]2 11. 1.6 x 10-2 12. 1.7 x 10-5 (
03
*(
3
) 13. AgCl /01
1. 22 I . S O 3I- (aq )+ S2O82- (aq) → I3- (aq) + 2 SO42- (aq)
s
22 8
−
0
dI
dt
= 4.5 x 10-3 mol⋅dm-3⋅s-1 #
2-
dSO 4
dt
3 mol⋅dm-3⋅s-1
2. +& A → 2B A → C .
B 4 0.6
mol/s C 4 0.2 mol/s *
5.00 mole 3/
* (5
,#% *0
(* (
3. )5t
I-(aq) + OCl-(aq) → IO-(aq) + Cl-(aq) +
,
[I-] mol dm-3
[OCl-] moldm-3
* mol dm-3s-1
7.91 x 10-2
0.12
0.18
0.06
0.18
3.95 x 10-2
0.09
9.88 x 10-3
0.03
0.09
7.91 x 10-2
0.24
a) j
b) !
( 0
+* [I-] 4 4 (
+* [OCl-] 4 2 (
+*5*(
4. *)5t
2A(g) + B(g) → C(g) + 2D(g) (* 25 oC !
( 3
[A] mol⋅L[B] mol⋅L
C mol⋅L-⋅s-1
0.010
0.010
1.20 x 10-3
0.020
0.010
2.40 x 10-3
0.030
0.010
3.60 x 10-3
0.020
1.44 x 10-2
0.030
a) j
b) #
(*
c) #
D * [A] [B] = 0.010 mol/dm3
5. +
#
- A + 2B → 3C + 5D +
A B +
C
D , 250 kJ 0
+
%
(
510 kJ +
%
(
3 *+
3 (,
)
6. 0
5*4 34
34 intermediate
2Cl(g)
Cl2(g)
2NO(g) + 2Cl(g) → N2(g) + 2ClO(g)
2ClO(g) → Cl2(g) + O2(g)
7. .+(2%, [NO2]+[NO3]- 4y *3
(* 32 oC, 1 atm
f N2O5 25*
4f
.2% 2 [NO2]+[NO3]- (s) → N2O5 (g)
2N2O5 (g) → 4NO2 (g) + O2 (g)
* N2O5 -(
NO2 N2O5
8. 3
.(* +* 5 2 (
*-#",+* 5 10 K #
+
-
* +*-#",
25 oC 4 35 oC
9. z33
(*!(
3
*3()(
a) +*+(*! b) 3
c) +*
d) +*-#",
e) +* "
/ (*f) +*
g) +*+
%
10. (*
(k) 5*(* 20 oC (
2.0 x 10-3 s-1 0
+
- 4 20.0 kJ/mol k (s-1) (* 30 oC
11. 5* (*
4.6 x 10-2 s-1 8.1 x 10-2 s-1 (* 0 oC 20 oC #
+
-
12. A 4
5* *
!
120 ( A
50% 3/
(
35 10%
13. (*
(k) 2NO(g) + O2(g) → 2NO2(g) ,
((*
1
2
3
4
5
*
NO (M) O2 (M)
0.01
0.01
0.01
0.02
0.01
0.03
0.02
0.03
0.03
0.03
NO2
(M/s)
0.007
0.014
0.021
0.084
0.189
14. ,
(
2A + B + 3C → 3D (* 25 oC
[A]
0.1
0.2
0.2
0.2
[B]
0.1
0.1
0.2
0.2
[C]
0.1
0.1
0.1
0.2
(mol dm-3s-|)
0.3
0.6
1.2
1.2
a) b) 
15. 33(*4
a) 2NO2(g) → 2NO(g) + O2(g)
rate = k[NO2]2
b) NO(g) + O3 → NO2(g) + O2(g)
rate = k[NO][O3]
c) 2NO(g) + F2(g) → 2ONF(g)
rate = k[NO][F2]
16. 1
-!(*
.(* +*5*+*-#",
17. 3& * (
3
+* 5 1
18. 2A → 4B + C 4
5* *( A k = 0.1 s-1
a) j
b) j
(
e
+ 3 /
(
3
c) 0
A +*5
2 M 4 6M +*5*(
19. 2H2(g) + 2NO(g) → 2H2O(g) + N2(g)
2NO(g)
N2O2(g)
fast equilibrium
k
N2O2(g) + Hk 2 (g) →
N2O(g) + H2O (g)
slow
k
k
N2O (g) + H2 (g) → N2(g) + H2O(g)
fast
a) intermediate 3
b) 34
20. 2NO2Cl → 2NO2 + Cl2 NO2Cl → NO2 + Cl
Cl + NO2Cl → NO2 + Cl2
a) intermediate 3
b) 34 bimolecular step
3
1
2
4
-, 1. 3.0 x 10-3 mol⋅dm-3⋅s-1 2. 10 s 3. a) rate = k [I-] [OCl-], = 4 b) 8 (
4. a) rate = k[A] [B]2 b) 1.2 x 103 L2⋅mol-2⋅s-1 c) 2.4 x 10-3 mol⋅dm-3⋅s-1 5. 760 kJ, ,
6. = Cl2, intermediate = Cl, ClO 7. Rate = −
∆[ N 2 O5 ]
d [ N 2 O5 ]
, NO2 = 2 (
=−
∆t
dt
N2O5 8. 5.3 x 104 J⋅mol- 9. b, c, d. f 10. rate = k[NO]2 [O2],
k= 7.0 x 103 L2⋅mol-2⋅s-1 12. 2.62 x 10-3 s-1 13. 18.8 kJ 14. 398.7 ( 15. a, b 18. a) rate = k [A] b) ln
[A] , slope = -0.1 c) 3 (
19. a) N2O2, N2O b) (* 2 20. a) Cl b) (*