Module 06: Phases of Matter Flashcards by carla klaasen

06.01 Kinetic Molecular Theory

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06.01 Kinetic Molecular Theory

Define Kinetic Theory of Matter

describes the physical properties of matter in terms of the motion of its particles

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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)

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06.01 Kinetic Molecular Theory

Describe the flow of thermal energy in the Kinetic Theory:

Absord heat → faster

Release heat → slower

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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

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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)

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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

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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

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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

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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

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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

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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]

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06.01 Kinetic Molecular Theory

What is the pressure of the gas?

Collision of moving gas particles

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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)

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06.01 Kinetic Molecular Theory

What is an ideal gas?

behaves according all assumptions of kinetic molecualr theory

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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)

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06.02 Phase Changes

06.02 Phase Chagnes

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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)

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06.02 Phase Changes

What is dew?

Water vapor in air condenses to liquid

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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

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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

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06.03 Gas Laws

06.03 GAS LAWS

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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

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# 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?

1. Volume (V) 2. Pressure (P) 3. Temperature (T) 4. Number of particles (n)

# 06.03 Gas Laws What are the 7 **Gas Laws**?

1. Changes to V, n, and T will affect pressure, kinetic energy, and the number of collisions within a sample. 2. If the volume of a sample is large, the pressure will be low, and there will be few particle collisions. 3. If the volume of a sample is small, the pressure will be higher, and more collisions will occur. 4. If the number of particles decreases, the number of collisions will decrease. 5. If the number of particles increases, the number of collisions will increase. 6. If temperature increases, the number of collisions will increase. 7. 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) 1. Increasing temperature 2. Adding more neon gas 3. Increasing the volume of the container 4. 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) 1. 0.00150 mL 2. 0.00200 mL 3. 155 mL 4. 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) 1. 2.3 L 2. 4.8 L 3. 7.5 L 4. 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) 1. 2.86 atm 2. 3.09 atm 3. 3.31 atm 4. 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? ## Footnote *2CO_(g) + O_2(g) → 2CO_2(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 1. Standard Temperature: *273 K* 2. 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) 1. 11 L 2. 22 L 3. 47 L 4. 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) 1. 305 L H₂ 2. 639 L H₂ 3. 948 L H₂ 4. 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)→ ZnCl_2(aq) + H_2(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) 1. 2.29 L H2 2. 3.32 L H2 3. 4.58 L H2 4. 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) 1. 5.60 liters 2. 4.20 liters 3. 2.10 liters 4. 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) 1. 17.2 grams 2. 15.8 grams 3. 12.3 grams 4. 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) 1. Pressure 2. Temperature 3. Volume 4. Type of particles

4. 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:_** 1. temperature increases 2. gas lower molar mass 3. particles are moving quickly **_Diffusion/Effusion decreases_**: 1. temperature decreases 2. gas has higher molar mass 3. 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? ## Footnote **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?

1. Ideal gas law PV = nRT (n = moles) 2. 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** ## Footnote _Step 01:_ Identify variables _Step 02:_ Solve

# 06.06 Honors Gas Behavior How can density be derived from the ideal gas laws?

1. Ideals gas laws: *n = PV/RT* 2. Replace moles (n) with mass (m)) over molar mass (M) → *m/M = PV/RT* 3. Use algebra allows us swap positions of M and V to give *m/V = PM/RT* 4. 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?

1. **Very high pressure** (additional volume becomes significant under high pressure) 2. **Very low temperatures** (intermolecular forces is significant - less kinetic energy to overcome intermolecular forces)