Gas Phase

Question 1

SI unit for pressure

Answer 1

pascal

Question 2

units of pressure relationships

Answer 2

1 atm= 760 mmHg= 760 torr= 101.325 kPa

Question 3

sphygmomanometers

Answer 3

an instrument used to measure blood pressure (mmHg)
sphygmo-: relating to the pulse or pulsation.

Question 4

STP

Answer 4

273 K (0 celcius) and 1 atm

Question 5

standard state conditions and what are they used for

Answer 5

used for standard enthalpy, entropy, free energy changes, and electrochemical cell voltage
H,S,G,Emf, His Great Elephant Socks or EFEE
298K (25 celcius), 1 atm, 1 M concentrations

Question 6

ideal gas

Answer 6

no intermolecular forces and occupies no volume

Question 7

When do real gases deviate from ideal behavior?

Answer 7

Under high pressure, low volume and temperature conditions.

Question 8

Combined gas law

Answer 8

Question 9

Avogrado’s principle Equation

Answer 9

Question 10

Boyle’s law

Answer 10

Question 11

Charle’s law

Answer 11

Question 12

Gay-Lussac’s law

Answer 12

Question 13

Dalton’s law

Answer 13

(total pressure from partial pressure)

Question 14

Henry’s law equation

Answer 14

Question 15

vapor pressure

Answer 15

pressure exerted by evaporated particles above the surface of a liquid

Question 16

Average kinetic energy of a gas

Answer 16

Question 17

Root-mean squared speed

Answer 17

Question 18

Graham’s law equation

Answer 18

Question 19

Van der Waals equation of state

Answer 19

Is used to correct the ideal gas law for intermolecular attractions and molecular volume.

a is for attractive forces
b is for big particles

if a and b are both 0, then the van der Waals equation of state reduces to the ideal gas law

Question 20

Gaseous state defined by 4 variables:
(variables)

Answer 20

We can define the state of a gaseous sample by four variables:

1) Pressure (P)
2) Volume (V)
3) Temperature (T)
4) # of Moles (n)

Question 21

Gas Pressure (units?)

Answer 21

Expressed in:

1 ATM = 760 mmHg (equv. to torr) = 100 kPa

The SI unit for pressure is the pascal (Pa)

Question 22

Standard temperature and pressure (STP)

Answer 22

The conditions under which the volume of a gas is usually measured:

1) 273 K or 0 C.
2) 1 ATM or 101 kPa

1 mole ideal gas = 22.4 L space

Question 23

Ideal gas

Answer 23

A hypothetical gas that has no intermolecular forces and occupies no volume.

Although real gases deviate from this idea at high temp or low volume, it is still a close estimate

Question 24

Ideal gas law

Answer 24

Shows the relationship among four variables that define a sample of gas:

PV=nRT

R is the ideal gas constant, which is 8.21x10^-2
and has units of ( L x atm / mol x K)
or may also be seen as 8.314 ( J / K x mol)

Question 25

Ideal gas constant

Answer 25

Use 0.08 when using atm in numerator!

Question 26

Density of a gas

Answer 26

Question 27

Avogadro’s Principle

Answer 27

All gases at a constant pressure and temperature occupy volumes that are directly proportional to the number of moles of gas present.

Question 28

Boyle’s Law

Answer 28

For a given gaseous sample held at constant temperature (isothermal conditions), the volume of the gas is inversely proportional to the pressure.

Question 29

Boyle’s law graph

Answer 29

as pressure increases, the volume decreases and vice versa

Question 30

Charles law

Answer 30

States that at constant pressure, the volume of a gas is proportional to its absolute temperature.

Question 31

Charles law graph

Answer 31

volume and temp are directly proportional: when one increases, the other increases in direct proportion

Question 32

Gay-Lussac’s Law

Answer 32

Relates temperature and pressure

Question 33

Dalton’s law

Answer 33

States that the total pressure of a gaseous mixture is equal to the sum of the partial pressures of the individual components.

Question 34

Partial pressure

Answer 34

the contribution each gas in a mixture of gases makes to the total pressure

Question 35

Henry’s law

Answer 35

States that the amount of gas dissolved in solution is directly proportional to the partial pressure of that gas at the surface of solution.

Question 36

The solubility of a gas will increase with ____________ partial pressure of the gas

Answer 36

The solubility of a gas will increase with __increasing__ partial pressure of the gas

Question 37

Kinetic molecular theory

Answer 37

Attempts to explain the behavior of gas particles. It makes a number of assumptions about them:

1) Gas particles have negligible volume
2) No intermolecular forces
3) Undergo random collisions with them + walls of container
4) Avg. kinetic energy of gas particle is directly proportional to temp.

Question 38

The higher the temp, the _________ the molecules move
The larger the molecules, the ________ they move

Answer 38

The higher the temp, the __faster__ the molecules move
The larger the molecules, the __slower__ they move

Question 39

Graham’s law

Answer 39

Describes the behavior of a gas diffusion or effusion, stating that gases with lower molar masses will diffuse or effuse faster than gases with higher molar masses at the same temperature.

Question 40

Diffusion

Answer 40

The spending out of particles from high concentration to low concentration

Question 41

Effusion

Answer 41

The net movement of gas under pressure from one compartment to another through a small opening