Unit 5 - States of Matter and Gas Laws
23) It may be difficult to determine the shape and structure of a crystalline solid just by looking at it because:
a crystalline solid may consist of one crystal or many crystals fused together a crystal may have fractured or may be worn down, which distorts its shape
20) Nonmetallic elements that bond to create giant molecules arranged in a crystal lattice form __________ crystals.
covalent network
46) The ____________ point is the temperature and pressure where the boundary between the liquid and gas state ceases to exist.
critical
23) The temperature above which a substance cannot exist as a liquid is called ______________.
critical temperature
12) If a substance is a(n)_______________ it melts at a specific temperature and pressure but if the substance is amorphous, liquefaction may take place gradually over a range of temperatures.
crystalline solid
17) A solid substance whose particles are arranged in orderly, geometric, repeating patterns called crystals is called ________________.
crystalline solid
particles in each unit cell are all located the same distance from each other and are oriented at 90° angles particles in each unit cell form square bases and four rectangular faces particles in each unit cell form 6 rectangular faces with hexagon-shaped bases particles in each unit cell form rhombus-shaped bases and four rectangular faces particles in each unit cell form rectangular bases and four rectangular faces particles in each unit cell form rectangular bases, two rectangular faces, and two faces that are parallelograms particles in each unit cell form bases and four faces with little or no symmetry
cubic crystal system tetragonal crystal system hexagonal crystal system trigonal crystal system orthorhombic crystal system nonoclinic crystal system triclinic crystal system
A process that requires the addition of heat energy is____________a process that releases heat energy is_______________
endothermic / exothermic
Liquefaction of a solid is a(n)______________process (requires heat) whereas solidification is a(n) ____________ process (releases heat).
endothermic / exothermic
31) Changing from a liquid to a vapor or a gas at temperatures and pressures below the boiling point is ______________.
evaporation
12) One law that describes the relationship between pressure, volume, temperature, and number of moles of a gas is called _______.
ideal gas law
3) A(n) ________ relationship is one in which one value increases by a certain factor if the other value decreases by the same factor.
inverse
1) The theory that explains the physical states of matter, based on the combined movements and interactions of the particles within a substance, is called the ______________ of matter.
kinetic-molecular theory
Particular motion of the tiny particles that make up matter is___________ in solids,___________in liquids and greatest in gases.
least / greater
9) Changing from solid to a liquid at or above melting point is _____________.
liquefaction
16) As the temperature of a solid rises, the particles move faster and farther apart until the temperature of the solid reaches a specific temperature called the melting point, at which the particles overcome the intermolecular forces, and the solid turns into a _________.
liquid
38) Changes in equilibrium vapor pressure can be measured with a(n):
manometer
21) Atoms of metallic elements that are arranged in a crystal lattice form ___________ crystals.
metallic
39) When water vapor begins to boil, pockets of vapor form at ______________, which are microscopic bumps, ridges, and cracks on the surface of the pan.
microfissures
18) A naturally occurring, inorganic substance with a definite chemical composition and a crystalline structure is called a(n) ___________.
mineral
6) The ____________ volume is the volume of a mole of any gas at standard temperature and pressure.
molar
10) Amount of heat energy required to change one mole of a solid at melting point to a liquid is its _____________.
molar enthalpy of fusion
21) The amount of heat energy required to change one mole of a liquid to a gas at its boiling point and at a constant pressure is ________________.
molar enthalpy of vaporization
25) During heating, once the temperature of a substance reaches the boiling point, the temperature will not rise again until additional heat called the _________________ has been added.
molar enthalpy of vaporization
16) According to Graham's law of effusion, the rate of diffusion or effusion of two gases under the same conditions of temperature and pressure are inversely proportional to the square root of the _______ of each gas.
molar mass
16) If two containers of gas at the same temperature and pressure are connected, the gas with the lower ___________ will diffuse faster.
molar mass
a crystal with symmetry of a≠b≠c and∝=γ=90∘≠β a crystal with symmetry of a≠b≠c and ∝≠β≠γ≠90∘ structure formed by silicon dioxide when it is melted and cooled rapidly glass, rubber, and plastic elements such as sulfur, carbon, and phosphorus; exhibit more than one structural form in the solid state
nonoclinic triclinic amorphous amorphous solids allotropic
50) The method of showing the particular states (phases) in which a substance will exist at different conditions of temperature and pressure is a ________________.
phase diagram
4) If liquid hydrogen is subjected to extreme ___________, it becomes a solid with a hexagonal crystalline system, and it takes the properties of a metal, which is another reason why it is placed in Group 1 of the Periodic Table.
pressure
11) The amount of heat required to change to raise the temperature of one gram of a substance by one kelvin (or Celsius degree) the _____________ of a substance.
specific heat
1) Liquids are fairly uncommon in the rest of the universe because liquids can exist only in a narrow range of _______________ found in very few places in the known universe.
temperatures
27) Condensation is an exothermic process because:
the same amount of energy is released during condensation as was gained during vaporization
20) According to Dalton's law of partial pressures, the total pressure of a mixture of unreactive gases is _________________ the partial pressures of each component gas.
the sum of
26) Crystal systems are determined by __________________________.
the symmetry of the crystal the shape of the crystal the arrangement of the particles within the crystal
19) The general term for changing from a liquid to a vapor or a gas is _____________.
vaporization
24) Boiling and evaporation are both forms of ______________, which is the process of changing the physical state of a substance from a liquid to a gas or a vapor.
vaporization
3) A change from a liquid to a gas or a vapor is _____________.
vaporization
7) The correct technical term that explains why maple syrup flows less easily than water is _____________.
viscosity
the ability of a liquid to resist flowing
viscosity
During an experiment, 575 mL of neon gas at 101 kPa were compressed in a cylinder to a volume of 144 mL. What was the new pressure of the gas, if the temperature remained constant?
403 kPa
A tank of methane gas contains 2.8 m3 of the gas at 20°C. The tank has a pressure-release valve that releases gas into a secondary tank that will hold 0.2 m3 of gas if the pressure rises. At what Celsius temperature will the methane fill both tanks?
41°C
17) Calculate the amount of heat required. You will need to use your Periodic Table and Table B-3 below. How much heat is required to raise the temperature of 475 grams of solid aluminum from room temperature (295K) to liquid aluminum at 1050K? Aluminum melts at 933.47K
521.65 kJ
) Solve this problem using the appropriate law. A researcher at McMurdo Station on Ross Island near Antarctica was conducting an experiment that involved collection of carbon dioxide gas by water displacement. It was a little chilly in the lab at the time of collection (16°C). Allowing for the vapor pressure of water, what was the pressure of the CO2 collected? Use Table B-6 from the CRG.
98 kPa
Solve this problem using the appropriate law. An average incandescent light bulb with a volume of 0.130 L contains 0.216 grams of argon gas. After the bulb had been burning for a few minutes, the temperature of the gas reached 100 °C. What was the pressure of the gas at that temperature? (Hint: first find the number of moles)
1.37 atm
Ice Station Bravo near the North Pole launched a helium-filled balloon to check atmospheric conditions. At sea level (1.0 atm) where the balloon was launched, it had a volume of 0.93m3 . It rose to an altitude of 18 000m where the atmospheric pressure dropped to 0.072atm . What is the volume of the balloon at that altitude assuming that the temperature was the same at sea level?
12.9 m^3
3) Solve this problem using the appropriate law.A sample of air with a volume of 25.0 mL, a pressure of 100 kPa, and a temperature of 22°C is compressed to 11.5 mL and a pressure of 225 kPa. What is its new Celsius temperature?
32°C
What is the volume of 7.25 g of oxygen gas at STP?
5.08 L
9) A chemical reaction produced 177.3 grams of chlorine gas ( Cl2). What was the volume of the gas?
56.01 L
36) What happens to equilibrium vapor pressure as temperature increases?
As temperature increases, equilibrium vapor pressure also increases.
4) ___________ is an inverse relationship of volume and pressure of a gas.
Boyle's Law
11) ___________ is a direct relationship between the volume and temperature of a gas.
Charles's Law
13) Why do liquids form spherical drops?
Cohesive forces between particles at the surface of the liquid create surface tension that pulls inwardly and laterally until the liquid forms a sphere.
18) _______________ states that the total pressure of a mixture of unreactive gases is the sum of the partial pressures of all of the component gases.
Dalton's law of partial pressures
______________ is transferred between particles when they collide, but the collisions are____________ with no net loss of energy.
Energy / elastic
17) ___________ is a direct relationship between temperature and pressure of a gas.
Gay-Lussac's Law
15) _______________ states that the rates of diffusion or effusion of two gases under the same conditions of temperature and pressure are inversely proportional to the square root of the molar mass of each gas.
Graham's law of effusion
16) _____________ will not freeze even at absolute zero unless a pressure of 2.5 MPa is applied.
Helium
6) ______________ forces are strong enough to give a liquid its definite volume, but not strong enough to hold it in a definite shape.
Intermolecular
9) How does the density of a liquid compare to the density of the same substance as a solid?
It is slightly less for most substances, except for water.
If fuel oil with a density of 0.89 g/cm3 was added to a mixture of the above substances, where would it float?
It would float on top of the vegetable oil but under the methanol.
7) Select what represents Boyle's Law:
PV= k
14) The molar fusion of enthalpy must be added to a substance in order to melt that substance because:
The equilibrium between the rate of liquefaction and the rate of solidification must be upset. Melting involves breaking intermolecular bonds. Melting involves a gain of kinetic energy.
24) ___________ is the study of the three-dimensional arrangement of particles and their orientation to each other within a crystalline structure by examining X-ray diffraction patterns.
X-ray Crystallography
26) The opposite of vaporization is ______________, which is the changing of the physical state of a substance from a gas or a vapor to a liquid at or below its boiling point.
condensation
22) If the temperature of any covalent compound is brought down low enough, it will freeze and form _________ crystals.
covalent molecular
a crystal with symmetry of a=b=c and∝=β=γ=90∘ a crystal with symmetry of a=b≠c and ∝=β=γ=90∘ a crystal with symmetry of a=b≠c and ∝=β=90∘≠γ a crystal with symmetry of a=b=c and ∝=β=γ≠90∘ a crystal with symmetry of a≠b≠c and ∝=β=γ=90∘
cubic tetragonal hexagonal trigonal orthorhombic
2) Which physical properties of liquids are similar to those of solids?
definite volume high density incompressibility
6) A direct change from gas or a vapor to solid is _____________.
deposition
5) What type of relationship is one in which one value changes by a certain factor if the other value changes by the same factor?
direct
17) While driving your car, you run over a nail that punctures the tire, and the air flows out of the hole, giving you a flat tire. This is an example of:
effusion
12) If the total kinetic energy of two particles after the collision is the same as the kinetic energy before the collision, the collision is _________.
elastic
3) A collision is _________ if the total kinetic energy of two particles after the collision is the same as the total kinetic energy of two particles before the collision.
elastic
35) When the rate of evaporation of a liquid in a closed container equals the rate of condensation, the liquid has achieved ______________.
equilibrium
8) The pressure at which a substance in its gaseous state can exist in equilibrium with the same substance in its liquid state at a given temperature is _____________ vapor.
equilibrium
) The particles of a liquid are in constant motion just like the particles in a solid, but the particles of a liquid move_______ are__________ apart, and have fewer _____________ than the particles of a solid.
faster, farther, interactions
15) Which physical properties of liquids are similar to those of gases?
fluidity diffusion
Particles of a_____________have little or no interaction, particles of a_______________have greater interaction, particles of a____________have the greatest interaction
gas / liquid / solid
15) Particles of one solid will not, for all practical purposes, mix with the particles of another solid when they are placed in contact because they ___________________.
have an extremely low rate of diffusion
14) If you try to squeeze rocks, they will not change because they ___________________.
have incompressibility
11) The _______________ states that the product of the pressure and volume of a fixed amount of gas is inversely proportional to the product of the number of moles of the gas, the ideal gas constant, and the absolute temperature of the gas.
ideal gas law
5) The ability of a substance to resist being forced into a smaller space is ______________.
incompressibility
11) The physical properties of solids can be explained with the kinetic-molecular theory of matter. Some of the properties of solids include:
incompressibility a definite shape and volume low rate of diffusion a definite melting point high density
19) Cations and anions arranged in a crystalline structure form ______________ crystals.
ionic
51) Some of the properties of a supercritical fluid include:
it can act like an organic solvent like a liquid it can diffuse like a gas
8) The temperature of a substance is determined by the average _________ energy of the particles within the substance.
kinetic
33) A device used to measure the pressure of a gas is a(n) ______________.
manometer
8) You can use the ____________ of a gas to find the mass of the gas at STP if you know the volume.
molar volume
2) All matter is made up of tiny particles called __________, __________, and __________.
molecules ions atoms
13) Every substance has its own ________________, which is the amount of heat required to change or raise the temperature of one gram of a substance by one kelvin (or Celsius degree).
specific heat
44) Changing from a solid to a gas or a vapor directly is ______________.
sublimation
47) A substance that exists at a pressure and temperature higher than its critical point is a _______________.
supercritical fluid
3) Which physical properties of liquids are unique to liquids?
surface tension viscosity capillarity
14) The surface of water forms a concave meniscus in a glass tube because ___________________ of the water for the glass is greater than the cohesive force between water molecules at the surface.
the adhesion
27) These terms: simple, body-centered, face-centered, and base-centered for a cubic crystal refer to:
the arrangement of particles within a crystal system
42) A pressure cooker will cook food faster because the increased pressure inside the container causes __________________________.
the boiling temperature to increase so that the water boils at higher temperatures
49) The temperature and pressure at which a substance can exist in all three states is called ____________.
triple point
30) A(n) ______________ is the smallest portion of a crystal lattice that still retains the crystalline structure.
unit cell
12) Select what represents the general mathematical equation of an inverse relationship:
x/y = k
6) Select what represents the general mathematical equation of a direct relationship:
xz = k
A canister contains 3.25 L of nitrogen gas at -150°C at a pressure of 506kPa. When the canister was allowed to warm up, the gas inside reached a pressure of 1214 kPa. What was the new Celsius temperature of the gas? The volume remained constant.
22°C
48) A graph that shows the particular states (phases) in which a substance will exist at different conditions of temperature and pressure is a _________________.
phase diagram
10) Tiny particles that make up matter are in constant motion which is ________ and _________.
rapid / random
8) The ability of a liquid to resist flowing is based on the attractive forces between particles of the liquid and the __________ of the particles of the liquid.
size
2) A change from a liquid to a solid is _____________.
solidification
13) Which one is not a measurement of the ideal gas constant?
°C
18) Select what represents Gay-Lussac's Law:
P/T = k
8) Which formula compares a sample of a gas under two different conditions of pressure and volume, if the temperature is constant?
P1V1 = P2V2
43) Changing from a gas or a vapor directly to a solid is ______________.
deposition
45) The formation of frost on a cold morning when the outside temperature is below freezing is an example of ______________.
deposition
4) The mixing of particles of one substance with particles of another substance when the two substances are placed in contact is ___________.
diffusion
2) A(n) ________ relationship is one in which one value changes by a certain factor if the other value changes by the same factor.
direct
13) Most solids will not float in water because they ________________.
have a high density
10) If you need to calculate one of the conditions of pressure, volume, temperature, and number of moles of a gas, use ________.
ideal gas law
13) Select what represents Charles's Law:
V/T = k
40) We cannot see water vapor that has evaporated but we can see water vapor that rises from water that is boiling because (50%)
When water evaporates, the vapor consists of individual molecules, which are invisible. When water evaporates, many molecules break through the top layer of the water and combine so we can see the vapor rising.
32) An element that can exhibit more than one structural form in the same state-solid, liquid, or gas, is _____________.
allotropic
31) A(n) _____________ is a substance whose particles are arranged in a random manner.
amorphous solid
34) The most significant force that holds particles in a liquid state is ________________.
atmospheric pressure
32) Changing from a liquid to a vapor or a gas at or above the boiling point is ______________.
boiling
1) The ________________ states that the product of the pressure and volume of a fixed amount of gas varies directly with its absolute temperature.
combined gas law
2) If you need to make calculations involving the pressure, volume, and temperature of a gas, use ________.
combined gas law
20) Changing from a vapor or a gas to a liquid is _____________.
condensation
1) A(n) ___________ is a number with a fixed value in a specific mathematical context.
constant
22) A condition in which two opposing changes occur at an equal rate is ______________.
equilibrium
Solve this problem using the appropriate law. A weather balloon with a volume of 50.4 L was launched from a U.S. Navy ship in the Indian Ocean where the temperature was 30 °C and the pressure was 100 kPa. At an altitude of 9000 m the temperature dropped to -48°C and atmospheric pressure had dropped to 30.8 kPa. What was the volume of the balloon at that altitude?
122 L
11) Why is the density of a liquid less at a higher temperature than it is at a lower temperature?
At higher temperatures, the particles of a liquid move faster and collide more frequently. As a result, the particles are pushed farther apart, which reduces the density of the liquid.
5) _______________ states that equal volumes of gases at the same temperature and pressure contain the same number of particles.
Avogadro's law
7) The fact that equal volumes of gases contain the same number of particles is described in ________.
Avogadro's law
