Chemistry
Name:________________________
Final Exam Review Packet
1.
2.
Date:__________________
Name the following:
a.
b.
Na2SO4 ________________________________
CaBr2 ________________________________
c.
KNO3
________________________________
d.
NH4Cl
________________________________
e.
f.
P4O10
CS2
________________________________
________________________________
List the conjugate acid or base for the following pairs
acid
base
H3O+
H 2O
OHNH3
HC2H3O2
H2SO4
PO43-
3.
Which one of the following 1 M solutions would have a pH of 0?
a.
Ca(OH)2
b. H2O
c.
NaOH
d. HCl
4.
If the pH of a solution is _____ the solution is slightly acidic
a.
7
b. 10
c.
2
d. 5
5.
pH is a measure of
a.
b.
c.
d.
hydroxide ion concentration.
hydrolysis.
hydrogen ion concentration.
hydrogen gas concentration.
6.
Water and a salt are always the products of a(n):
a.
b.
c.
d.
7.
acid and a base
combustion reaction
synthesis reaction
single replacement reaction
A compound formed in solution from the negative ion of an acid and the positive ion of a
base is a __________.
a. soap
b. glycerin
c. detergent
d. salt
8.
A solution with a bitter taste and slippery feel is most likely _______
a.
a base
b.
a salt
c.
a hydrate
d. an acid
9.
Organic substances that change color in the presence of an acid or base are called
___________.
a.
acids
b. bases
c.
indicators
d. soaps
10.
The particle that remains after a proton has been released by an acid is the
a.
conjugate base
b. amphoteric substance
c.
polyprotic acid
d. conjugate acid
11.
Water
a.
b.
c.
d.
and carbon dioxide are always the products of a(n):
acid and a base
combustion reaction
synthesis reaction
single replacement reaction
12.
The empirical formula for hexane (C6H12) is:
a. C6H12
b. CH
c. C3H6
d. CH2
13.
What is the mass of 0.0150 moles of Cu?
a.
0.953 g
b. 0.000236 g
c.
6.02 x 1023 g
d. 22.4 g
14.
The molar mass of the compound Sr(CN)2 is:
a.
87.62 g/mol
b. 113.64 g/mol
c.
127.65 g/mol
d. 139.66 g/mol
15.
20.0 g of NH4F represents ___?___ moles of NH4F.
a.
0.588
b. 0.540
c.
0.500
d. 37.05
16.
How many moles of water are there in 18.0 g of water?
a.
2.00 moles
b. 2.50 moles
c.
1.00 moles
d. 1.50 moles
17.
How many atoms are there in 2.00 moles of gold?
a.
6.02 x 1026 atoms
b. 2 atoms
c.
6.02 x 1023 atoms
d. 1.20 x 1024 atoms
18.
A salt lover decided to flavor her meal by adding 1.80 moles of sodium chloride, better
known as table salt, to her French fries. She has just added ____?____ g of salt to
her fries.
a.
b.
c.
d.
19.
105
58.5
5.00
58.44
A compound has the empirical formula of CH2O and its molar mass is 120 g. What is its
molecular formula?
a.
C3H6O3
b. C4H8O4
c.
CH2O
d. C2H3O2
20.
Which of the following statements is INCORRECT?
a.
Reactants are substances written to the left of the arrow.
b. Coefficients indicate the relative number of moles of each substance in a
chemical reaction.
c.
An equation is balanced by changing subscripts as needed.
d. Chemical equations are balanced to show that matter is conserved.
21.
What percentage of ammonium phosphate, (NH4)3PO4, is oxygen?
a.
10.7%
b. 8.1 %
c.
42.9 %
d. 28.2 %
22.
To balance the following reaction, what are the correct coefficients?
NO +
a.
2,1,1
b. 3,1,3
c.
2,2,2
d. 2,1,2
O2 →
NO2
23.
What law would be used to solve the following problem?
A gas sample in a 5.00 L container has a pressure of 1.00 atm. If the pressure is changed to
3.50 atm, what is the new volume?
a.
Boyle’s Law
b. Charles Law
c.
Gay-Lussac’s Law
d. Ideal Gas Law
24.
The reaction between sodium chloride and potassium ________ occur.
a.
will
b. will not
c.
can’t
d. there is not enough information to complete the statement
25.
What word replaces equals in the following statement?
phosphorus tribromide equals phosphorus and bromine
a.
reactants
b. products
c.
yields
d. occurs
26.
Which of the following could be a precipitate?
a.
Pb(NO3)2
b. (NH4)3PO4
c.
d.
27.
Al2(SO4)3
AlPO4
If an equation requires heat, what symbol is written above the yields sign?
a.
Pt
b. ∆
c.
Pd
d. (aq)
28.
Which of the following is not a diatomic element?
a.
fluorine
b. chlorine
c.
carbon
d. iodine
29.
A catalyst speeds up a reaction by _____________ the activation energy of a
chemical reaction.
a.
heightening
b. lowering
c.
eliminating
d. producing
30.
In the single replacement reaction below, which statement is true?
Mg + PbBr2 →
a.
Br2 will be a product
b. PbMg will be a product
c.
Pb will be a product
d. there are no products because the reaction will not occur
31.
The net ionic equation between Al2(SO4)3 and LiOH contain which of the following
a.
lithium ions
b. aluminum ions
c.
sulfate ions
d. lithium sulfate
32.
In the reaction in number 31, which of the following will be a spectator ion?
a.
SO42-
b. Al3+
c.
OH-
d. Al(OH)3
33.
Which of the following is not one of the main assumptions of the Kinetic Theory?
a.
collisions between the particles is perfectly elastic
b. matter cannot be created or destroyed
c.
all matter is composed of small particles
d. the small particles are in constant, rapid, random motion
34.
Charles’ Law states that temperature and volume are _______________ related.
a.
not
b. if temperature decreases, the volume does not change
c.
inversely
d. directly
35.
In Boyle’s Law, _____________ remains constant.
a.
pressure
b. size of container
c.
temperature
d. volume
36.
What Kelvin temperature is equal to 25°C?
a. 100 K
b. 25 K
c. 248 K
d. 298 K
37.
Convert 680. mm Hg to kPa:
a.
0.895 kPa
b. 90.7 kPa
c.
13.2 kPa
d. 101.325 kPa
38.
Which of the following is true about absolute zero?
a.
Cold flows towards warm areas
b. all molecular motion ceases
c.
water begins to freeze
d. all of the above
39.
You have 22.4 liters of an ideal gas at STP. The number of molecules of gas in this
sample is:
a.
b.
c.
d.
40.
6.02 x 1023
22.4
3.01 x 1023
11.2
A sample of gas has a volume of 50.0 L at a temperature of 300.K. What temperature
would be needed for this sample to have a volume of 60.0 L if its pressure remains
constant?
a. 87oC
b. 250 K
c. 400 K
d. 360oC
41.
The temperature and pressure at which the solid, liquid and gaseous states of a
substance are in equilibrium is the
a. critical temperature
b. critical pressure
c.
triple point
d. melting point
42.
The energy required to change one mole of a solid to a liquid at its melting point is
called:
a.
specific heat capacity
b. heat of fusion (ΔHfusion)
c.
heat of vaporization (ΔHvaporization)
d. enthalpy
43.
When the particles of a solid gain enough kinetic energy to break their ordered
arrangement and slip past one another, the solid
a.
vaporizes
b. melts
c.
deposits
d. freezes
44.
In the three common states of matter, the strongest intermolecular forces between
particles is observed in a
a.
solid
b. liquid
c.
gas
d. vapor
45.
Energy is released in order for a substance to
a.
freeze
b. sublimate
c.
melt
d. all of the above
46.
The phase change represented by the equation CO2 (g) → CO2 (l) is called:
a. condensation
b. melting
c. boiling
d. sublimation
47.
Ionic salts dissolve well in water because of water’s
a.
polarity
b. viscosity
c.
boiling point
d. freezing point
48.
Which of the following solutions would be an electrolyte?
a.
KI
b. NaCl
c.
C12H22O11
d. a and b
49.
Why are molecular compounds non-electrolytes?
a.
they never dissolve in water
b. they dissociate into ions when they dissolve
c.
they dissolve as a whole molecule
d. there is a movement of ions when they dissolve
50.
Why is water a polar molecule?
a.
O is more electronegative than H
b. H is more electronegative than O
c.
O and H have the same electronegativity value
d. O and H share the electrons in the bond equally