Gases and Their Properties
4. The kinetic molecular theory describes the motion of atoms and molecules
and explains the properties of gases. As a basis for understanding this
concept:
a. Students know the random motion of molecules and their collisions with a
surface create the observable pressure on that surface.
b. Students know the random motion of molecules explains the diffusion of
gases.
c. Students know how to apply the gas laws to relations between the
pressure, temperature, and volume of any amount of an ideal gas or any
mixture of ideal gases.
d. Students know the values and meanings of standard temperature and
pressure (STP).
e. Students know how to convert between the Celsius and Kelvin
temperature scales.
f. Students know there is no temperature lower than 0 Kelvin.
g.* Students know the kinetic theory of gases relates the absolute
temperature of a gas to the average kinetic energy of its molecules or
atoms.
h.* Students know how to solve problems by using the ideal gas law in the
form PV = nRT.
Using , H2 + O2  H2O, how many
grams of water could form from
the reaction of 64.0g of O2?
A)10.0g
B)36.0g
C)64.0g
D)72.0g
E)None of the above
What causes a gas to expand when it is
heated?
A. The particles in the gas move around
faster and spread out.
B. The gas becomes bigger.
C. Particles in a high temperature state
rise up and push the low temperature
ones down.
D. The actual particles themselves swell
so that the whole gas becomes larger
when heated.
Why does a gas decrease in pressure when
the container it is in becomes larger?
A. A larger container causes the particles of gas
to hit the boundaries less often, therefore they
exert less pressure.
B. The particles slow down when the container
increases in size, therefore causing the
particles to hit the walls with less force.
C. Because the particles swell and become
heavier, so that they move slower and hit the
boundaries less often.
D. Some gas always escapes when a container
expands and therefore, the pressure inside
goes down.
At absolute zero, which best describes
the motion of all gas particles?
A.
B.
C.
D.
They become absolutely still.
They turn into ice.
They disappear.
They become very cold and frost grows
on top of the atoms.
What is the temperature of a metal at
435OC in the Kelvin scale?
A.162 K
B. 567 K
C.708 K
D.1.59 K
E. 312 K
What are the values for STP?
A.273OC and 1 atm
B. 0 K and 1 atm
C.0 OC and 1 atm
D.273 K and 360 mmHg
A 30ml cylinder changes from 27OC to
127OC, what will the cylinder’s new
volume be if pressure remains
constant?
A.15ml
B. 40ml
C.630ml
D.75ml
E. None of the above
The air in the room is at 25°C and has
a pressure of 101kPa. How many
moles of gas are in the room, if the
room has a volume of 20 dm3?
(R = 8.31)
A.
B.
C.
D.
230.0 mol
1.61 mol
0.816 mol
76.0 mol
What is the volume of 2 moles of
methane gas at STP?
A.22.4 L
B. 470.0 L
C.11.2 L
D.44.8 L
Acids and Bases
5. Acids, bases, and salts are three classes of compounds that
form ions in water solutions. As a basis for understanding
this concept:
a. Students know the observable properties of acids, bases, and
salt solutions.
b. Students know acids are hydrogen-ion-donating and bases
are hydrogen-ion-accepting substances.
c. Students know strong acids and bases fully dissociate and
weak acids and bases partially dissociate.
d. Students know how to use the pH scale to characterize acid
and base solutions.
e.* Students know the Arrhenius, Bronsted-Lowry, and Lewis
acid-base definitions.
f.* Students know how to calculate pH from the hydrogen-ion
concentration.
What is not a property of Bases?
A.
B.
C.
D.
Feel Slippery
Sour in taste
Conduct an electric current
Form a salt and water when combined
with an acid
E. All of the above
According to Brønsted-Lowry, acids
and bases are:
A. Acids contain hydrogen ions and bases
contain hydroxide ions.
B. Acids are proton donors and bases are
proton acceptors.
C. Acids accept electron pairs and bases
donate electron pairs.
An unknown solution in the lab has a
pH of 13, which best describes the
solution?
A.A
B. A
C.A
D.A
E. A
strong acid
weak acid
neutral solution
strong base
weak base
What happens when equal amounts of
a 1M acid and a 1M base are mixed?
A. The solution is neutralized.
B. A salt and water are formed.
C. The [H3O+] and [OH-] are equal.
D. All of the above
E. Both A and B
When a strong acid or base are mixed
with water they separate fully into
separate ions, this process is called:
A.Disintegration
B. Degeneration
C.Dissolution
D.Dissociation
E. None of the above
An acid solution has a hydronium
concentration of [H3O+] = 0.001M,
what is the pH of the solution?
A.1
B. 2
C.3
D.4
E. 5
Solutions
6. Solutions are homogenous mixtures of two or more
substances. As a basis for understanding this
concept:
a. Students know the definitions of solute and solvent.
b. Students know how to describe the dissolving
process at the molecular level by using the concept
of random molecular motion.
c. Students know temperature, pressure, and surface
area affect the dissolving process.
d. Students know how to calculate the concentration
of a solute in terms of grams per liter, molarity,
parts per million, and percent composition.
10g of Sodium Chloride is added to
100ml of water, which is the solute?
A.Water
B. Sodium Chloride
C.Water and Sodium Chloride
D.Both A and C
How does water dissolve a polar
solute?
A. By surrounding the charges of the
solute with the positive and negative
poles of the water molecules.
B. By filling the gaps between the
molecules
C. Water does not dissolve polar solutes.
D. Water gets broken down into H+1 and
OH-1 and these attach to the charges
of the polar solute
Heating a solid solute helps the
dissolving process by:
A. Melting the solute therefore creating a
liquid that mixes easily with the solvent
B. Spreading the molecules away from each
other so empty spaces are filled
C. Increasing the speed of the solute
therefore increasing the collisions
D. All of the above
Which of the following is not a way to
increase the rate at which a solid
solute dissolves?
A. Stirring
B. Crushing the solute first
C. Adding pressure
D. Increasing the temperature
1.5 mol of CuCl2 are dissolved into 50L
of water, what is the Molarity of
solution?
A.75.0 M
B. 3.0 M
C.0.03 M
D.0.75 M
Explain why heating a gas solute will
not help it dissolve.
A. Because the gas molecules are too small to
be affected by the increase in heat.
B. Because the gas molecules are too hard to
stir and heating is just like stirring on the
molecular level.
C. Gas molecules move faster when heated
and this causes them to move out of the
solution so they don’t dissolve.
D. Gas molecules are lower in energy than
water, therefore when the gas molecules are
heated they have an increase in their total
enthalpy of dissolution which requires an
increase in the molecular status.
Chemical Thermodynamics
7. Energy is exchanged or transformed in all chemical
reactions and physical changes of matter. As a basis for
understanding this concept:
a. Students know how to describe temperature and heat
flow in terms of the motion of molecules (or atoms).
b. Students know chemical processes can either release
(exothermic) or absorb (endothermic) thermal energy.
c. Students know energy is released when a material
condenses or freezes and is absorbed when a material
evaporates or melts.
d. Students know how to solve problems involving heat
flow and temperature changes, using known values of
specific heat and latent heat of phase change.
Which of the following is the best
description of the temperature of a
substance?
A. The temperature is the average kinetic
energy of the individual particles in the
substance.
B. The temperature is best described as how
hot a substance is.
C. The temperature is the total amount of
kinetic energy from all of the particles in a
substance.
D. Temperature is best defined as the absence
of cold.
E. None of the above
When a reaction releases energy (in
other words energy is a product)
this reaction can be described as:
A.
B.
C.
D.
E.
Endothermic
Exothermic
Either condenses or freezes
Both B and C
None of the above
How much energy is needed to raise
the temperature of 10g of water
from 20OC to 40OC?
A.200.0 J
B. 836.8 J
C.2510.4 J
D.418.4 J
E. None of the above
What is the ΔHvap for water?
A.334 J/g
B. 4.184 J/g OC
C.2260 J/g
D.1 cal/g OC
How much energy does it take to get
260g of water at its freezing point
to solidify?
A.
B.
C.
D.
E.
587600 J
86840 J
1087.8 J
3340.6 J
None of the above
Reaction Rates and Chemical Equilibrium
8. Chemical reaction rates depend on factors that influence the
frequency of collision of reactant molecules. As a basis for
understanding this concept:
a. Students know the rate of reaction is the decrease in concentration of
reactants or the increase in concentration of products with time.
b. Students know how reaction rates depend on such factors as
concentration, temperature, and pressure.
c. Students know the role a catalyst plays in increasing the reaction rate.
d.* Students know the definition and role of activation energy in a
chemical reaction.
9. Chemical equilibrium is a dynamic process at the molecular level. As a
basis for understanding this concept:
a. Students know how to use LeChatelier's principle to predict the effect
of changes in concentration, temperature, and pressure.
b. Students know equilibrium is established when forward and reverse
reaction rates are equal.
c.* Students know how to write and calculate an equilibrium constant
expression for a reaction.
The Reaction rate for a chemical
reaction relies on:
A. The decrease in reactants conc. and the
increase in products conc.
B. A change in temperature, pressure, and
surface area.
C. The presence of a catalyst
D. All of the above
Describe how adding pressure to solid
reactants effects the rate of
reaction?
A catalyst increases the rate of a
reaction by:
A. Increasing the speed of individual
particles so they hit harder.
B. Breaks the reactants into smaller pieces.
C. Lowering the activation energy.
D. Telling the reactants to react together.
E. Both C and D
Describe how adding pressure will
increase the rate of a reaction for a
gas reactants?
Which factor does not effect the
equilibrium of a reaction?
A.
B.
C.
D.
E.
Temperature
Catalyst
Pressure
Concentration
None of the Above
In a sealed bottle that is half full of
water, equilibrium will be attained
when water molecules
A. Cease to evaporate
B. Begin to condense
C. Are equal in number for both the liquid
and the gas phase
D. Evaporate and condense at equal rates
In the reaction:
N2 + 3H2  2NH3
Where would the equilibrium shift if
Pressure is increased?
A.
B.
C.
D.
Left
The side with the more moles of gas
The side with the least moles of gas
Both A and B
What is the formula you would use to
calculate the Equilibrium constant of
a reaction?
Draw a Heat curve and label where a
liquid, a gas, and freezing occurs
Zn (s) + 2HCl
(g)
 H2 (g) + ZnCl2
(aq)
+ HEAT
Write the Equilibrium
expression/constant for the above
reaction.
Zn (s) + 2HCl
(g)
 H2 (g) + ZnCl2
(aq)
+ HEAT
What would happen to the equilibrium
if H2 gas is removed?
Zn (s) + 2HCl
(g)
 H2 (g) + ZnCl2
(aq)
+ HEAT
What would happen to the equilibrium
if the reaction is placed on ice?
Zn (s) + 2HCl
(g)
 H2 (g) + ZnCl2
(aq)
+ HEAT
What would happen to the equilibrium
if the volume the reaction is in
increased?
Why does a more concentrated solution
react at a faster rate?
A hot piece of Iron is placed into a tub of
water at room temp. Which one losses
energy?
In Thermochemistry, which term is used to
describe a reaction that is cold in
temperature.
2Na + Cl2  2NaCl
If 3.64 moles of Na is reacted with an
excess of chlorine gas, how many
moles of NaCl will be produced?
A. 1.28 mol
B. 3.64 mol
C. 7.28 mol
D. 10.92 mol
2H2 + O2  2H2O
If 8 g of oxygen reacts with an
unlimited amount of hydrogen, how
many grams of water will be
produced?
A. 9 g
B. 16 g
C. 18 g
D. 36 g
A mass of 5.4 grams of aluminum (Al) reacts
with an excess of copper (II) chloride
(CuCl2 ) in solution, as shown below.
3CuCl2 + 2Al  2AlCl3 + 3Cu
What mass of solid copper (Cu) is
produced?
A.
B.
C.
D.
0.65 g
8.5 g
13 g
19 g

Which statement best describes the
density of an atom’s nucleus?
A. The nucleus occupies most of the atom’s
volume but contains little of its mass.
B. The nucleus occupies very little of
the
atom’s volume but contains little of its
mass.
C. The nucleus occupies most of the atom’s
volume but contains most of its mass.
D. The nucleus occupies very little of the
atom’s volume but contains most of its
mass.
D
 Which
part of the atom has the
least amount of mass?
A.
B.
C.
D.
electron cloud
nucleus
neutrons
proton
A
How many outer shell electrons
(valence electrons) does iron
have?
2
Draw the Lewis electron
dot diagram for
nitrogen.
N
Elements X has the following electron
configuration:
1s22s22p63s23p64s23d104p65s24d105p6.
Which of the following describes this
element?
 A.
unstable metal
 B.
unstable nonmetal
 C.
stable metal
 D.
stable nonmetal
D
Which of the following elements
has the largest radius?
A.F
B.Br
C.As
D.N
E.S
C
Where are the alkali earth
metals?
2nd
Group
If aluminum becomes an ion,
does it become larger or
smaller?
Smaller – it
lost electrons
(3+)
What is Nuclear Fusion?
When a nucleus
breaks down into
smaller ones
An isotope of uranium emits a particle
composed of two protons and two
neutrons. What remains after the
isotope emits the particle?
A. a new element that has a mass smaller than
the uranium mass
B. a new element that has a mass greater than
the uranium mass
C. a new isotope of uranium that has a mass
greater than the starting mass
D. a new isotope of uranium that has a mass
smaller than the starting mass
A
What are the three types of nuclear
decay?
Alpha,
beta,
gamma
How is a positive ion formed?
By losing
electrons
What element is in group 4 and period 5?
A. Magnesium
B. Zirconium
C. Vanadium
D. Boron
B
If a circuit for a light bulb is bridged by a
glass of pure water, what will happen?
A.
B.
C.
D.
The light bulb will glow because water
conducts electricity
The light bulb wont glow because the
water needs to have ions
Hard to say it depends on the
temperature of the water
Only if a catalyst is available will it light
B
Ionic materials are best described as:
A. Gaseous masses with weak interparticle
forces
B. Solids made of atoms sharing electrons
in order to complete the valance shells of
the participating elements
C. Solids made of a repeating pattern of
ions held by electrostatic forces
D. Liquids that have weaker intermolecular
bonds so that the molecules can easily
pass each other.
C
Which of the following best explains how
covalent bonding occurs?
A. Atoms exchange electrons forming
positive and negative ions
B. Metals share electrons forming molecules
C. Nonmetals share electrons forming
molecules
D. Marvin Gaye plays “Let’s get it on” and
the atoms tumble into each others arms.
C
Which of the following elements is filling the
“s” sublevel?
A.
B.
C.
D.
Cu
Fe
Ca
Ne
What family is Bromine in?
If the unbalanced equation is:
C3H8 + O2 → CO2 + H2O, then what is the
best whole number ratio between the
propane and the oxygen.
A.
B.
C.
D.
E.
1
1
3
3
8
to
to
to
to
to
5
1
8
2
2
A
The mole is best defined as:
The number of hydrogen atoms in a
water molecule
B. The number of carbon atoms in 12g
of carbon-12
C. The mass of a single atom
D. The number of atoms it takes to get
the molar equivalent of an atoms
mass
B
A.
What is the molar mass of sodium
hydroxide, NaOH?
40 g/mol
How many moles is 46.5g of
sodium hydroxide?
A)1860mol
B).860mol
C)40.0mol
D)1.16mol
E)None of the above
D
What is the molar mass of
(NH4)2Cr2O7?
252 g/mol
How many grams of
(NH4)2Cr2O7 are in 5.50mol of
ammonium dichromate?
1386 g
If a room at STP has 300L of CO
in it, how many grams of
carbon monoxide are in the
room?
375 g
What type of chemical reaction
always produces carbon dioxide
and water?
Combustion
What is ionization energy?
Energy needed
to take 1
electron away
from an atom
Why do metals create different
colors when heated?
The electrons get
excited, jump to a
higher level, fall
back down and
release the energy