7.
Write
a balanced equation for the following reactions:
a. combustion of butane
b. aqueous nitric acid + solid aluminum hydroxide
c. aqueous calcium nitrate
+ aqueous potassium phosphate
8.
Calculate
the mass of silver nitrate needed to react with 10.0 g of calcium chloride.
9.
Calculate
the mass of acetic acid needed to neutralize 3.22 g of sodium carbonate.
10.
Calculate
the molarity of a solution that contains 1.25 g of sodium chloride per 250.0 mL
of solution.
11.
Calculate
the mL of 0.252 M sodium hydroxide needed to neutralize 10.0 mL of 1.3 M
sulfuric acid.
12.
Calculate
the mass of sodium bicarbonate needed to neutralize 2.33 mL of 0.85 M
phosphoric acid.
13.
Calculate
the concentration of sodium acetate in a solution prepared by dissolving 25 mL
of 0.159 M sodium acetate in enough water to give a total volume of 120.0 mL.
14.
Calculate
the volume of 0.222 M acetic acid needed to prepare 125 mL of 0.100 M acetic
acid.
15.
Calculate
the concentration of acetic acid in a solution prepared by mixing 10.0 ml of
0.360 M acetic acid and 15.0 mL of 0.220 M sodium acetate.
16.
For
each of the following, (1) draw a valid Lewis structure, (2) give the name of
the electron domain geometry for the central atom, (3) give the name of the
molecular geometry for the central atom, and (4) identify the hybrid orbitals
used by the central atom.
a. PCl5
b. BrF5
c. COCl2
d. CN-
17.
Calculate
the enthalpy change when 2.5 g of KClO3 decomposes according to the
reaction:
2 KClO3 (s) à 2 KCl (s) +
3 O2 (g) DH = -89.4 kJ
18.
A
closed system absorbs 125 J of energy from the surroundings while it performs
0.110 kJ of work. What is the change in
internal energy for the system?
19.
Calculate
the enthalpy change that occurs when 125 g of steam at 105oC is
cooled to 25oC. The specific
heat of steam is 2.080 J/gK while the specific heat of water is 4.18 J/gK. The specific heat of ice is 2.05 J/gK. The heat of fusion of water is 6.01 kJ/mole while the heat of vaporization of water is
40.79 kJ/mol.
20.
A
26.4 g sample of metal at 99.0oC is added to 25.0 g of water in a
constant pressure calorimeter. If the
initial temperature of the water was 20.0oC and the equilibrium
temperature is 27.0oC, what is the specific heat of the metal?
21.
When
5.0 g of KBr is dissolved in 30.0 g of water, the temperature drops from 21.0oC
to 15.3oC. What is the molar
heat of solution of KBr in kJ/mole?
Assume that the specific heat of the solution is 4.18 J/g-K.
22.
Identify
all intermolecular forces present between two molecules of the same substance
for each of the following compounds.
a. CH3CH2CH3
b. CH3CH2CH2CH2OH
c. CH3CH2NH2
d. CH3CH2OCH2CH3
e. CBr4
f.
23.
List
the following compounds in order of increasing boiling point.
24.
List
the compounds shown in the previous question in order of increasing vapor
pressure at ambient (room) temperature.
25.
Use
the phase diagram below to answer the following questions.
a. What phase change occurs
going from point B to A?
b. What phase change occurs
going from pont G to H?
c. What physical state(s) is/are present
at point F?
d. What physical state(s) is/are present
at point D?
e. What physical state(s) is/are present
at point E?
f. Which point represents the critical
point of the substance?
g. Which point represents the triple point
of the substance?
26.
A
solution is prepared by dissolving 10.2 g of HCl (g) in 100.0 g of DI
water. Calculate the concentration of
HCl in the following units:
a. mass %
b. mole %
c. molality
27.
Given
the following equation and data, write the rate law equation, including the
value of the rate constant. (Make sure
you include the correct units for the rate law.) What is the overall order of the reaction? 4 NO (g)
+ O2 (g) à 2 N2O3
|
Expt. |
[NO] (M) |
[O2] (M) |
Initial rate (M/s) |
|
1 |
0.012 |
0.020 |
0.102 |
|
2 |
0.018 |
0.020 |
0.2295 |
|
3 |
0.018 |
0.040 |
0.459 |
28.
Calculate
the average reaction rate for the disappearance of reactant A in the time
interval from 20 min. to 50 min. using the following data. A à 2 B
|
Time
(min) |
[A]
(M) |
|
0.0 |
1.00 |
|
10.0 |
0.74 |
|
20.0 |
0.54 |
|
30.0 |
0.40 |
|
40.0 |
0.30 |
|
50.0 |
0.22 |
29.
Write
an expression that relates the rate of disappearance of Br2 (g) with
the rate of appearance of NOBr (g) in the following reaction.
2 NO (g) + Br2
(g) à
2 NOBr (g)
30.
Using
the equation from the previous question, calculate the rate of disappearance of
bromine when the rate of appearance of NOBr is 1.6 x 10-3 M/s.
31.
Draw
a reaction energy diagram for an endothermic reaction with an
activation energy of 15 kJ/mol and a heat of reaction of 3 kJ/mol. Label the reactants, products, transition
state on the diagram and show the activation energy and heat of reaction.
32.
Write the equilibrium constant expressions (Kc)
for the following reactions.
a.
2
SO2 (g) + O2 (g)
2 SO3 (g)
b.
FeO
(s) + H2 (g) Fe
(s) + H2O (g)
33.
Write the equilibrium constant expression (Kp) for reaction (a) in the previous question.
34. 
At equilibrium, the reaction N2(g)
+ 3H2(g) 2NH3(g)
had the following concentrations: [N2]
= 0.0850 M, [H2] = 3.10 x 10-3 M, and [NH3] =
0.0310 M. What is the value of Kc ?
35.
Calculate
the concentration of silver ions and sulfate ions present in a saturated
solution of silver sulfate if Ksp = 1.5 x 10-5
.
36.
A
2.000 L reactor is filled with 1.000 mol H2 (g) and 1.000 mol I2
(g) at 448oC. The value of
the equilibrium constant, Kc, for the reaction H2 (g) + I2
(g) 2 HI (g) at 448oC
is 50.5. What are the
concentrations of H2, I2, and HI at equilibrium?
37.
Given
the reaction NO (g) + O3 (g)
NO2 (g) + O2 (g)
DH = -199 kJ, what happens when:
a.
NO is added?
b.
NO2 is added?
c.
The volume of the container is doubled?
d.
The reaction is heated?
e.
O3 is removed?
f.
NO2 is removed?
38. What
are the [H+], [OH-], pH, and pOH for a 1.65 x 10-4
M HCl?
39. What
are the [
40. What
is the pH for a 0.200 M HC7H5O2 solution? (Ka = 6.3 x 10-5)
41.
The
following titration curve was obtained from the titration of 0.525 g of an
unknown acid using 0.125 M KOH Use this
information to find the following information:
(a) the number of equivalence points; (b) the volume of base needed to
neutralize the acid; (c) the molar mass of the acid; (d) the values of the
pKa(s) for the acid.
42.
Identify
the Bronsted-Lowry acid and base as well as the conjugate acid and conjugate
base.
NH2OH + C5H5NH+
à
NH3OH+ + C5H5N
43.
Balance
the following redox reaction:
MnO4-
(aq) + Cl- (aq) à Mn2+ (aq) + Cl2
(g) (acidic solution)
44.
Identify
the element oxidized, element reduced, oxidizing agent, and reducing agent in
the previous question.
45.
Use
the standard reduction potentials in your text to calculate the standard cell
potential for a galvanic cell incorporating an Al3+|Al half cell and
a Cu2+|Cu half cell.
46.
Write
the balanced equation for the reaction occurring in the galvanic cell from the
previous question.
47.
Predict
whether DS will be positive,
negative, or nearly zero for each of the following:
a. shredding a piece of paper
b. Ag+ (aq) + Cl- (aq) à AgCl (s)
c. melting a piece of ice
48.
Use
the standard free energies of formation from your text to calculate the value
of Go for the following reaction
N2 (g) + 3 H2
(g) à
2 NH3 (g)
49.
Calculate
the concentrations of silver ion and phosphate ion present in a saturated
solution of silver phosphate if DGo
for the dissolution of silver phosphate in water is 100.3
kJ/mole at 298K.
50.
Circle
and name the functional groups present.
51.
Name
each of the following compounds.
52.
Draw
each of the following compounds.
a. 5-bromo-2,2-dimethly-4-propyloctane
b. trans-2,3,4-trimethyl-3-hexene
c.
cis-4,5-dichloro2-heptene
d.
4-ethyl-2,3-dimethyl-3-hexanol
e.
1-bromo-4,4-dimethyl-2-nonyne