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chem chapter 5
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kinetic molecular theory
a way to visualize what the molecules are doing
E
k
= 1/2mv
2
m = mass v=velocity
*both affect the kinetic energy
one
molecules (or atoms) of gases are continuously in motion
always have NRG
two
the volume of gas molecules is negligible compared to the volume of the container
three
the attractive and repulsive forces of gas molecules are negligible
no affect on NRG transfer during a collision
four
as long as the temperature remains constant, the average kinetic energy of the molecules is constant
individual molecules can transfer NRG from one to another, but the
average
remains constant.
five
the average kinetic energy is directly proportional to absolute temperature
not dependent on the identity of gas
all gases have the same average NRG at same temperature
pressure is a result of...
collisions of molecules with sides of container
increase V at constant T and n...
# of collisions of molecs with the wall of container decreases
volume goes up, pressure goes down P
1
V
1
= P
2
V
2
increase T at constant V and n...
increase T
increase average kinetic NRG
increase # of collisions & speed of collisions
overall...pressure goes up
P
1
/T
1
= P
2
/
T
2
Author
Anonymous
ID
45846
Card Set
chem chapter 5
Description
october 28, 2010
Updated
2010-10-29T04:58:59Z
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