APCHEM Unit 3
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19 Terms
What is the relationship between mass and velocity in the KE = ½ mv² equation?
Inverse
How do you convert C to K?
273 + C
If temperature is the same between gases, then what is also the same?
Kinetic Energy
What is the relationship between pressure and movement?
As movement increases, collisions against the container increase, and pressure increases.
What is the relationship between pressure and temperature?
As temperature increases, kinetic energy increases, which causes velocity to increase, which leads to more frequent collisions, and more forceful collisions, which increases pressure.
What is the relationship between pressure and # of moles?
As number of moles (n) increases, more moles are frequently colliding against the container, which increases pressure.
What is the relationship between pressure and volume?
As volume increases, moles have to travel farther to collide, this decreases the number of collisions, which decreases the pressure.
When temperature change has happened what must you also mention?
Kinetic Energy
Molar Mass equation is what?
MM = dRT/P
What are STP Conditions
1atm, 22.4L, 273K/0C
How to calculate percent error?
Experimental - Theoretical / Theoretical
What is E and T in percent error?
E: Experimental # i get
T: the truth
When you want to see if the temperature has doubled, what do you look at?
Kelvin, NOT Celsius.
What is percent yield equation?
( A / T ) x 100
How does temp behave at ideal gas behavior?
High Temp, High Kinetic Energy. High energy collisions, elastic collisions.
How does temp behave at NON-ideal gas behavior?
Low temp, Low Kinetic Energy. Low energy collisions, IMFS start to work.
How do volume, pressure and IMF distance behave at ideal gas behavior?
Large Volume, low pressure, large IMF distances. Ignore atomic radii; very low IMF interactions.
How do volume, pressure and IMF distance behave at NON-ideal gas behavior?
Small Volume, High pressure (big pressure), small IMF distances. Consider the atomic radii, consider their IMFS.
What 2 main factors best describe why a gas deviates from ideal behavior at any condition?
IMF’s, and Volume (size of atom / atomic radii)