Exam 2 - Gas laws

Question 1

What is the Kinetic Theory of Matter?

Answer 1

It predicts how matter behaves based on certain assumptions and approximations, explaining differences between solids, liquids, and gases.

Question 2

What are the three states of matter and their particle behavior?

Answer 2

Solids have tightly bound particles (vibrate), liquids have free space to move but particles are still attracted, and gases have particles that are far apart and move freely.

Question 3

What causes phase changes in matter?

Answer 3

Increases in kinetic energy, typically in the form of heat.

Question 4

What are the common physical properties of gases?

Answer 4

Gases expand to fill their containers, are highly compressible, have low densities, and form homogeneous mixtures.

Question 5

How do gas molecules behave in terms of movement and interaction?

Answer 5

Gas molecules move independently with no forces keeping them together or pushing them apart.

Question 6

What are the main points of the Kinetic Theory of Gases?

Answer 6

Gases consist of molecules in continuous random motion, the volume of molecules is negligible, and attractive/repulsive forces are weak.

Question 7

How does temperature affect the kinetic energy of gas molecules?

Answer 7

The average kinetic energy of gas molecules depends only on the temperature, and energy is transferred during collisions but the average does not change if temperature is constant.

Question 8

What are the different types of molecular speed in gases?

Answer 8

Most probable speed (ump), average speed (uav), and root mean squared speed (urms).

Question 9

How does molar mass affect the speed of gas molecules?

Answer 9

At a given temperature, gases with lower molar masses have higher speeds.

Question 10

What are the four properties that define the state of a gas sample?

Answer 10

Temperature (K), Pressure (atm), Volume (L), and Amount of gas (mol).

Question 11

What is pressure in terms of gases?

Answer 11

Pressure is the amount of force applied to an area.

Question 12

What does Boyle’s Law state?

Answer 12

The pressure of a gas is inversely related to its volume when temperature is constant. P1V1 = P2V2

Question 12

How is atmospheric pressure defined?

Answer 12

It is the weight of air per unit of area.

Question 13

What are the major gas laws?

Answer 13

Boyle’s Law, Charles’s Law, Gay-Lussac’s Law, Avogadro’s Law, Ideal Gas Law, Dalton’s Law, Graham’s Law, Henry’s Law, and the van der Waals Equation.

Question 14

What is the Combined Gas Law?

Answer 14

It combines Boyle’s, Charles’s, and Gay-Lussac’s laws to relate pressure, volume, and temperature when the amount of gas is constant.

Question 14

What does Charles’s Law state?

Answer 14

The temperature of a gas is directly related to its volume, with pressure and the amount of gas constant.

Question 15

What does Gay-Lussac’s Law state?

Answer 15

The pressure of a gas is directly related to its temperature, with volume and amount of gas constant.

Question 16

What does Avogadro’s Law state?

Answer 16

The volume of a gas is directly related to the number of moles of gas, with temperature and pressure constant. At STP, one mole of gas occupies 22.4 L.

Question 17

What is the Ideal Gas Law equation?

Answer 17

PV=nRT, where R = 0.08206L x atm x mol-1 x K-1

Question 18

What does Dalton’s Law state?

Answer 18

The total pressure of a gas mixture is the sum of the partial pressures of each gas. Each gas behaves as if it were alone in the container.

Question 19

What does Graham’s Law state?

Answer 19

The rate of effusion or diffusion of a gas is inversely proportional to the square root of its molar mass. Lighter gases move faster.

Question 20

What does Henry’s Law state?

Answer 20

The solubility of a gas in a liquid is directly proportional to the partial pressure of that gas in equilibrium with the liquid.

Question 21

How do real gases differ from ideal gases?

Answer 21

Real gases deviate from ideal behavior at high pressure and low temperature due to intermolecular forces and the volume occupied by gas molecules.

Question 22

What is the van der Waals Equation?

Answer 22

It adjusts the Ideal Gas Law to account for molecular volume and intermolecular forces

Question 23

How does atmospheric pressure change with altitude?

Answer 23

As altitude increases, atmospheric pressure decreases.

Question 24

Pneumonic for gas laws

Answer 24

Boyles a Pervert = pressure/volume is inverse
Charles law - Charles likes tv: temp =volume
Gay lussac- physical therapy is gay: pressure = temp
Combined: those 3 combined - BCG
Avogadros law: rotten avocados take up space - volume = moles
Ideal gas law: BCA - Boyles Charles avogadro
Grahams law: decreased molecular mass = increased speed (smaller equals faster)
Henrys law: ???
Henry Dalton’s law: gasses dont mix, they act as separate gasses.
Van der waals: real gasses such as oxygen, break down at increased pressure and/or decreased temp