Module 06: Phases of Matter Flashcards
06.01 Kinetic Molecular Theory
06.01 Kinetic Molecular Theory
06.01 Kinetic Molecular Theory
Define Kinetic Theory of Matter
describes the physical properties of matter in terms of the motion of its particles
06.01 Kinetic Molecular Theory
What basic assumptions is the Kinetic Theory based on?
- Matter composed small particles (ions, atoms, molecules)
- Particles in matter are organized in different arrangements based on state of matter
- Particles of matter constant motion (different amount of kinetic every)
06.01 Kinetic Molecular Theory
Describe the flow of thermal energy in the Kinetic Theory:
Absord heat → faster
Release heat → slower
06.01 Kinetic Molecular Theory
Why is temperature measured in “average kinetic energy?”
Any time, one particles could have different kinetic energy than neigbor
Always averagee kinetic energy all particles
06.01 Kinetic Molecular Theory
According to kinetic theory, how is motion and arrangement influenced?
- Kinetic energy
- Intermolecular forces
Solid: tightly arranged → more force & less kinetic
Liquid and gasses: loose arrangement → strong kinetic (can break intermolecular forces)
06.01 Kinetic Molecular Theory
Solids: (Arrangement of particles, Motion, Shape, Volume, Compressibility)
Arrangement of particles:
- close together
- difinite pattern
Motion:
- vibrate
- fixed position
Shape: definite
Volume: definite
Compressibility: low
06.01 Kinetic Molecular Theory
Liquid: (Arrangement of particles, Motion, Shape, Volume, Compressibility)
Arrangement of particles:
- close together
- random pattern
Motion:
- slide past one another
Shape: not definite
Volume: definite
Compressibility: low
06.01 Kinetic Molecular Theory
Gases: (Arrangement of particles, Motion, Shape, Volume, Compressibility)
Arrangement of particles:
- far apart
- random pattern
Motion: quick movement any direction
Shape: not definite
Volume: not definite
Compressibility: high
06.01 Kinetic Molecular Theory
Plasma: (Arrangement of particles, Motion, Shape, Volume, Compressibility)
Arrangement of particles:
- far appart
- pattern influenced attraction of ions
Motion: quick movement any direction
Shape: not definite
Volume: not definite
Compressibility: high
06.01 Kinetic Molecular Theory
What are the 5 basic properties of gases (under normal conditions)?
-
Density
- low compared to liquid or solid
- far apart each other
-
Compressibility
- can be compressed smaller volumes (due to space between particles)
-
Expansion
- spread out fill entire container
-
Diffusion
- spread out and mix with other particles without being stirred
-
Fluidity
- easily glide part eachother
06.01 Kinetic Molecular Theory
Whta characteristics of a gas is needed to fully describe a sample?
- Volume (V) [liters]
- Pressure (P) [atomspheres (atm)]
- Temperature (T) [Kelvin]
- Number of particles (n) [moles]
06.01 Kinetic Molecular Theory
What is the pressure of the gas?
Collision of moving gas particles
06.01 Kinetic Molecular Theory
What are Pascal, atmospheres, and millimeters of mercury? What is the conversion factor?
- Pascal (Pa): one newton per square meter
- Atmostpheres (atm)
- Millimeters of mercury (mm Hg) or torr
1 atmosphere (atm)
= 760 mm Hg
= 760 torr
= 101.3 kilopascals (kPa)
06.01 Kinetic Molecular Theory
What is an ideal gas?
- behaves according all assumptions of kinetic molecualr theory
06.01 Kinetic Molecular Theory
What is the Kinetic Molecular Theory of Gases (5)?
- Particles gas are in constant motion
- Large number of tiny particles
- Collisions between partciles are elastic (no gain of loss of kinetic energy due to collision)
- No forces of attraction or repulsion are experienced between particles (moves fast enough so attractive forces are negligible)
- Average kinetic energy of particles of a gas is directly proportional to temperature (higher the temperature, greater kinetic energy)
06.02 Phase Changes
06.02 Phase Chagnes
06.02 Phase Changes
What are the 4 transition points from one state of matter to another?
- Melting (solid → liquid)
- Freezing (liquid → solid)
- Boiling (liquid → gas)
- Condensation (gas → liquid)
06.02 Phase Changes
What is dew?
Water vapor in air condenses to liquid
06.02 Phase Changes
How does water change its phase?
- 0 C to 100C: liquid state & temperature and kinetic energy of molecules increase
- large amount energy needed overcome intermolecular forces between water molecules
- then break appart one another and move at high speeds and water becomes gas
Melting & boiling = temperature momentarily contant
- break bonds
energy must be greater than potential energy of bonds between molecules
06.02 Phase Changes
What are heating curves and cooling curves? What is the purpose?
-
Heating Curve: line graph represents phase changes matter starting with solid and heating to a gas
- contant heating
- gain energy
-
Cooling Curve: graph of phase changes of matter starting with gas and cooling to solid
- contant cooling
- loose energy
Model temperature changes and phase transitions
06.03 Gas Laws
06.03 GAS LAWS
06.03 Gas Laws
Define Scientific Laws:
Generalization that describes a variety of behaviors in nature but does not attempt to explain them (why not how).
- based on observations and experimentation
- tested agian and peer reviewed
06.03 Gas Laws
What is Newton’s Law of Universal Gravitation?
- force of attraction between any two option
- attraction in mathematcis terms (not why it exists)
06.03 Gas Laws
What is Kepler’s Laws of Planetary Motion?
- 3 mathematics laws describe motion planets in solar system
06.03 Gas Laws
What is Gas Law?
There are laws that predict the behavior of gases. These gas laws describe the relationship between volume, temperature, pressure, and mole amount, and how all gases will act under certain conditions.
06.03 Gas Laws
What 4 factors causes changes in gases?
- Volume (V)
- Pressure (P)
- Temperature (T)
- Number of particles (n)
06.03 Gas Laws
What are the 7 Gas Laws?
- Changes to V, n, and T will affect pressure, kinetic energy, and the number of collisions within a sample.
- If the volume of a sample is large, the pressure will be low, and there will be few particle collisions.
- If the volume of a sample is small, the pressure will be higher, and more collisions will occur.
- If the number of particles decreases, the number of collisions will decrease.
- If the number of particles increases, the number of collisions will increase.
- If temperature increases, the number of collisions will increase.
- If temperature decreases, the number of collisions will decrease.
06.03 Gas Laws
What are the variables and their meating in the Gas Laws?
Initial Quantities:
P1 = initial pressure
V1 = initial volume
T1 = initial temperature
n1 = initial number of moles
Final Quantities:
P2 = final pressure
V2 = final volume
T2 = final temperature
n2 = final number of moles
06.03 Gas Laws
What is Boyle’s Law?
Pressure and Volume
- Relationship: P1V1 = P2V2
-
Gas Behavior: Inverse relationship between pressure of gas and volume
- ↑P↓V and ↓P↑V
- Contants: Temperature and numbers of moles are held constant
06.03 Gas Laws
What is Charles’s Law?
Volume and Temperature
- Relationship: V1÷T1=V2÷T2
-
Gas Behavior: Direct relationship between volume of gas and temperature
- ↑V↑T and ↓V↓T
- Constants: pressure and number moles constant
06.03 Gas Laws
What is Gay-Lussac’s Law?
Pressure and Temperature
- Relationship: P1÷T1=P2÷T2
-
Gas Behavior: Direct relationship between presssure of a gas and temperature
- ↑P↑T and ↓P↓T
- Constants: Volume and number of moles of gas are held constant
06.03 Gas Laws
What is Avogadro’s Law?
Volume and Moles
- Relationship: V1÷n1=V2÷n2
-
Gas Behavior: direct relationshiip between volume of gas and number of moles of a gas
- ↑V↑n and ↓V↓n
- Constant: Pressure and temperature are constant
06.03 Gas Laws
A scientific law is the explanation of multiple scientific theories. (1 point)
True
False
False
06.03 Gas Laws
Which of the following would not cause an increase in the pressure inside a sealed container of neon gas? (4 points)
- Increasing temperature
- Adding more neon gas
- Increasing the volume of the container
- Adding helium gas
3. Increasing the volume of the container
06.03 Gas Laws
At 0.750 atm, the volume of a gas is 300.0 mL. If the temperature remains constant and the pressure is changed to 0.600 atm, what is the new volume of the gas? (4 points)
- 0.00150 mL
- 0.00200 mL
- 155 mL
- 375 mL
4. 375 mL
06.03 Gas Laws
A 6.0 L sample of nitrogen gas contains 0.50 mole of a gas. If enough gas is added to make a total of 0.75 moles at the same pressure and temperature, what is the resulting total volume of the gas? (4 points)
- 2.3 L
- 4.8 L
- 7.5 L
- 9.0 L
4. 9.0 L
A gas at constant volume has a pressure of 3.20 atm at 300. K. What will be the pressure of the gas at 290. K? (4 points)
- 2.86 atm
- 3.09 atm
- 3.31 atm
- 3.56 atm
2. 3.09 atm
06.04 Ideal Gas Law
06.04 Ideal Gas Law
06.04 Ideal Gas Law
Define Ideal Gas Law:
the state of an ideal gas follows the equation PV = nRT
06.04 Ideal Gas Law
What is the equation in the Ideal Gas Law?
PV = nRT
- P = pressure (atm)
- V = volume (V)
- n = number of moles (mol)
- R = ideal gas constant = 0.0821 (L x atm)÷(mol x K)
- T = temperature (K)
06.04 Ideal Gas Law
How can ideal gas relationships predict the volume of gases in a chemical reaction?
-
Volume ratio same steps as mole ratios
*
06.04 Ideal Gas Law
What is the Volume ratio?
the ratio of volume of one gaseous reactant or product to the volume of another determined using the coefficients in a balanced equation
06.04 Ideal Gas Law
Assuming all volume measurements are made at the same temperature and pressure, how many milliliters of carbon dioxide gas can be produced when 206.5 milliliters of oxygen gas react with excess carbon monoxide?
2CO(g) + O2(g) → 2CO2(g)
The coefficients in this balanced equation provide a volume ratio between gases when they are all at the same temperature and pressure. A ratio of 1:2 of O2 to CO2 means that a given volume of oxygen gas will react with twice the volume of carbon dioxide.
206.5 mL O2 × [2 mL CO2]÷[1 mL O2] = 413.0 mL CO2 can be produced
The ideal gas law uses the liter as the unit of volume for gas; however, this works for any unit of volume if the units are the same as the units in the volume ratio and both substances are gases under the same conditions.
06.04 Ideal Gas Law
What are the standard conditions for gases?
STP: an abbreviation that represents standard temperature and pressure
- Standard Temperature: 273 K
- Standard Pressure: 1 atm
06.04 Ideal Gas Law
What is the volume to mole conversion factors?
1 mole of gas / 22.4 L or 22.4 L / 1 mole of gas
06.04 Ideal Gas Law
To use the gas law constant R = 0.0821, the unit for temperature should be Kelvin and the unit for volume should be milliliters. (2 points)
True
False
False
06.04 Ideal Gas Law
What is the volume of 2.1 moles of nitrogen gas at standard temperature and pressure (STP)? (3 points)
- 11 L
- 22 L
- 47 L
- 82 L
3. 47 L
06.04 Ideal Gas Law
A reaction is expected to produce 28.3 moles of hydrogen gas. If the hydrogen is collected at 297 K and 1.08 atm, what is the volume? (3 points)
- 305 L H2
- 639 L H2
- 948 L H2
- 1,240 L H2
2. 639 L H2
06.04 Ideal Gas Law
Zinc metal and hydrochloric acid react together according to the following equation:
2HCl(aq) + Zn(s) → ZnCl2(aq) + H2(g)
If 5.98 g Zn reacts with excess HCl at 298 K and 0.978 atm, what volume of H2 can be collected? (3 points)
- 2.29 L H2
- 3.32 L H2
- 4.58 L H2
- 7.41 L H2
1. 2.29 L H2
06.04 Ideal Gas Law
Read the given equation.
Na2O2 + CO2 → Na2CO3 + O2
What volume of O2 gas is produced from 2.80 liters of CO2 at STP? (3 points)
- 5.60 liters
- 4.20 liters
- 2.10 liters
- 1.40 liters
4. 1.40 liters
06.04 Ideal Gas Law
Read the given equation.
2Na + 2H2O → 2NaOH + H2
During a laboratory experiment, a certain quantity of sodium metal reacted with water to produce sodium hydroxide and hydrogen gas. What was the initial quantity of sodium metal used if 8.40 liters of H2 gas were produced at STP? (3 points)
- 17.2 grams
- 15.8 grams
- 12.3 grams
- 10.0 grams
1. 17.2 grams
06.04 Ideal Gas Law
Which of the following factors does not determine the movement of particles in the atoms or molecules of a gas according to the ideal gas law? (3 points)
- Pressure
- Temperature
- Volume
- Type of particles
- Type of particles
06.06 Honors Gas Behavior
06.06 Honors Gas Behavior
06.06 Honors Gas Behavior
Define Effusion:
- movement of gas particles through a small opening in container wall due to pressure and particle movement inside the container
06.06 Honors Gas Behavior
When does Diffusion and Effusion increase and decrease?
both dependent on velocity of gas particles (influenced by temperature and molar mass of gas)
Diffusion/Effusion increase:
- temperature increases
- gas lower molar mass
- particles are moving quickly
Diffusion/Effusion decreases:
- temperature decreases
- gas has higher molar mass
- particles moving slowly
06.06 Honors Gas Behavior
: We can also make comparisons of velocity, rate of effusion, or rate of diffusion based on molar mass. Gas particles with less mass have higher velocities (and rates of effusion and diffusion) than gas particles with greater mass. Which sample of gas would effuse the fastest under the same temperature and pressure conditions?
CH4
Cl2
O2
Ne
CH4 would effuse the fastest because it has the lowest molar mass of the gases above.
06.06 Honors Gas Behavior
What information can be used to compare the molar masses and velocity of different gases?
Less massive gas particles move faster with an increase in temperature
06.06 Honors Gas Behavior
What is Graham’s Law?
law stating that the rates of diffusion and effusion of a gas are inversely proportional to the square root of the density of the gas
06.06 Honors Gas Behavior
What is the steps to solve a problem with Graham’s Law?
Step 01: Setup equation with given rate comparison
Step 02: Substitute known molar masses
Step 03: Solve the molar mass for the unknown variable
06.06 Honors Gas Behavior
How can the mole ratio and ideal gas law be used to determine a substance molarity?
- Ideal gas law PV = nRT (n = moles)
- Stoichiometry: moles of sample (n) = mass sample (m)/ molar mass substance (M)
M = mRT/PV
06.06 Honors Gas Behavior
What is the formula for molar mass (derived from ideal gas laws)?
M = mRT/PV
Step 01: Identify variables
Step 02: Solve
06.06 Honors Gas Behavior
How can density be derived from the ideal gas laws?
- Ideals gas laws: n = PV/RT
- Replace moles (n) with mass (m)) over molar mass (M) → m/M = PV/RT
- Use algebra allows us swap positions of M and V to give m/V = PM/RT
- Density of gas is mass perunit volume → d = m/v
d = PM/RT
06.06 Honors Gas Behavior
How do real gasses deviate from the ideal gas concept?
- finite volume
- interact through intermolecular forces
06.06 Honors Gas Behavior
Name two extreme conditions that results in a deviation from ideal conditions?
- Very high pressure (additional volume becomes significant under high pressure)
- Very low temperatures (intermolecular forces is significant - less kinetic energy to overcome intermolecular forces)
