Chapter 13 (gases/gas laws)

Question 1

Pressure

Answer 1

The force acting on an area

Question 2

Temperature and volume

Answer 2

As temperature increases volume increases

Question 3

Kinetic energy theory of gases

Answer 3

• Some particles move fast, some move slow
• Particles are always moving in a constant, random motion
• Pressure of gas is due to collisions of gas particles
• Increased gas temp causes more collisions

Question 4

Difference between real and ideal gases

Answer 4

Ideal gases have
NO volume
NO attraction

Question 5

Difference between solids and gases

Answer 5

Solids– definite shape and volume
High density

Gases– NO definite shapes and volumes
Extremely Low density

Question 6

If a gas is compressed, the

Answer 6

Pressure will increase

Question 7

Heating up gas makes the particles

Answer 7

Have more kinetic energy and increase in pressure

Question 8

Pressure units

Answer 8

1 ATM = 760 mmHg = 760 torr = 101.3 kpa = 1.7 psi

Question 9

What is 515 mmHg in kpa ?

Answer 9

515 mmHg x 101.3kpa/760mmhg

Question 10

Boyles law / constant temperature and pressure

Answer 10

(Inverse relationships)

As pressure increases, volume decreases

Question 11

Boyles law formula

Answer 11

PV1=PV2

Tip(asking to find either volume or pressure with three given variables)

Question 12

Charles law – temperature and volume at constant pressure

Answer 12

As volume increases temperature increases

Question 13

Charles law formula

Answer 13

V/T=V/T

Tip(when asking for volume or temperature with three given variables –one temp and one volume)
ALL ASWERS IN KELVIN (c+273)

Question 14

GayLussacs Law – temperature and pressure at constant volume

Answer 14

As pressure increases, temperature increases

Question 15

Gay lussacs formula

Answer 15

P/T= P/T

Tip(asking for pressure or temperature given three variable –one temp and one pressure)
ALWAYS IN KELVIN

Question 16

Combined gas law

Answer 16

PV = P2V2
T T2

When you’re given all three and asked to find one
If one remains constant, eliminate it from the equation..

Question 17

Dalton’s law of partial pressure

Answer 17

The total pressure of a mixture of gas is the sum of all their individual pressures

Question 18

Graham’s law of diffusion and effusion

Answer 18

The big gas particles move slowly, small move fast

Question 19

Diffusion

Answer 19

Random mixing of particles

Question 20

Effusion

Answer 20

Escape of small particles

Question 21

Which particles love fast? The ones in the heavier mass element or lighter mass element?

Answer 21

Lighter mass element

Question 22

STP

Answer 22

Standard temperature and pressure

1atm=760mmhg

Question 23

Density of gas equation

Answer 23

D = (mm)(p)/rt

Question 24

Molar mass of gas equation

Answer 24

g(RT)/PV

Question 25

Ideal gas law

Answer 25

``` PV = nRT P-pressure V-volume(L) n-moles R-ideal gas constant T- temperature (K) ``` Does not relate to the amount of gas that is present, but rather the amount of substance

Question 26

Avogadro's hypothesis

Answer 26

States that one mole of any gas occupies the same volume as long as the temperature and pressure are held constant. R=PV (To determine value of ideal gas constant) — nT

Question 27

Molecular weight (molar mass) gas formula

Answer 27

dRT —— = MW P