GAS LAWS

Question 1

what assumptions can we make about how the atoms behave in a kinetic model

Answer 1

• large number of molecules in random, rapid motion
• particles occupy negligible volume
• all collisions are elastic
  -forces between particles can be ignored except for collisions

Question 2

what is the change in momentum equal to when a particle collides with a wall

Answer 2

p=2mv

=mv-(-)mv
=mv+mv
=2mv

Question 3

What is Boyles law

Answer 3

pressure of an ideal gas is inversely proportional to its volume, provided temp stays constant

Question 4

how does volume vary with pressure
If temp is constant

Answer 4

as you increase pressure the volume does down
p∝1/v, which will give a straight line on a graph

or pV=constant

Question 5

what happens when you quickly compress a gas

Answer 5

temp increases

Question 6

what is the equation linking pressure and temp

Answer 6

p∝T

Question 7

p/t=?

Answer 7

constant

Question 8

p1xt2/t1=?

Answer 8

p2

Question 9

explain pV=nRT

Answer 9

n=number of moles
R=molar gas constant=8.31 jk^-1mol^-1

Question 10

explain F=nmc^2/L

Answer 10

we want C because its the average speed of all the molecules
n is the total number

Question 11

what is boltzman constant

Answer 11

1.38x10^-23 jk^-1

Question 12

how do u workout number of particles with moles

Answer 12

multiply by avogadros number

Question 13

What is Charles law

Answer 13

at constant pressure, the volume of a gas is directly proportional to its absolute temp

Question 14

what is internal energy

Answer 14

the sum of the randomly distributed kinetic and potential energies of all the atoms or molecules within the system

Question 15

what does RAVED stand for

Answer 15

Random motion
Attraction- none between particles
Volume- the gas particles take up a negligible volume
Elastic collisions
Duration of collisions are negligible

Question 16

state the equation for an ideal gas

Answer 16

pv=nRT