Kinetic molecular theory U9

P - pressure

mmHg, kPa, atm

V- volume

mL, L (1000mL =1 L)

n - mole

convert any amount in gram to mole (given grams/molar mass =mole)

R- gas law constant (units of pressure will change the number only)

0.0821 L x atm/ mol x K

8.314 Lx kPa/ mol x K

T - tempreture

kelvin

Pressure

the force of all the gas particle/ wall collisions divided by the area of the wall , unit atm, torr, mmHg, kPa

Hg is

mercury

Volume

the amount of space occupied by a sample of matter. The volume of a regular object can be calculated by multiplying its length by its width and height, mL, L, cm3, dm3

Tempreture

average kinetic energy of particles

the kelvin scale is based

on the concept of absolute zero, no negative numbers on the kelvin scale

celsius to kelvin

K = C +273

kelvin to celsius

K- 273

movement

ideal gas particles are assumed to be in constant nd random motion

Particle volumee

scientists assume that in a sample of an ideal gas, the volume of a gas particle is very small compared to the volume of the sample. Most of the volume of a gas is empty space

Inter molecular forces

scientists assume that ideal gas particles are far apart, there are no significant forces of traction or repulsion between gas particles (they go in a straight line)

Energy

the collins’s between ideal gas particles are assumed to be elastic that is, no kinetic energy is lost

The fur assumptions of ideal gases

movement, particle volume, intermolecular forces, energy

Real gases ___ behave ideally

do not

the four characteristics of real gases

they do experience intermolecular tractions

they do have volume

they do not have elastic collisions

Ideal gas

a gas that obeys the gas laws, and the gas equation PV=nRT strictly at all temps and pressures

No gas is truly

ideal

high pressure means

small volume

low temperatures mean

they move slowly

Likely to behave nearly ideally

low pressure (high volume)

high tempreture (moving fast)

Not likely to behave ideally

high pressure

low tempreture

All gases (real gases) found in nature behave like ideal gases

false

gas particles have less energy compared to solids or liquids

false

gas particles have less amount of attraction among particles compared to solids or liquids

true

Tempreture is the measure of potential energy in particles

false

Kinetic energy of particles increases as the tempreture is increased

true

Gases are less dense than solids because there is a lot of space between the particles of gas

true

The random motion of gas particles causes a gas to expand until it fills the container

true

The density of a gas decreases as its compressed

false

a gas can flow into a space occupied by another gas

true

the diffusion of gas is caused by the random motion of the particles of gas

true

lighter gas particles diffuse less rapidly than do heavier gas particles

false

and ideal gas is one whose particles take up space

false

at low temps ideal gases liquify

false

in the real world, gases consisting of small molecules are the only gases that are truly ideal

false

most gases behave like ideal gases at many temps and pressures

true

no inter molecular attractive forces exist in an ideal gas

true

non polar gas molecules behave more like ideal gases than do gases that are polar

true

real gases deviate from most ideal gas behavior at high pressures and low temperatures

true

the smaller the gas molecule the more the gas behaves like an ideal gas

true