Term
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Definition
| P1T2=P2T1 directly proportional |
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Term
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Definition
| V1T2=V2T1 directly proportional |
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Term
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Definition
| P1V1=P2V2 inversely proportional |
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Term
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Definition
| P1V1T2=P2V2T1 amount of gas does not change |
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Term
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Definition
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Term
| Standard Temperature & Pressure |
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Definition
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Term
| Amount of Atmosphere Gases |
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Definition
| 80% N2,20% O2, and trace amounts of CO2, H20, and Argon |
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Term
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Definition
force per unit area
p=f/a
lower as you go up |
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Term
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Definition
| glass tube with mercury, inverted and held in dish of mercury. Atmosphere supports 1 meter tall of mercury. |
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Term
| What are the units of pressure equal to STP? |
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Definition
1.00 atm
101325 Pa
101.325 kPa
14.7 psi
760. mm Hg
760. torr |
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Term
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Definition
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Term
| Dalton's Law of Partial Pressures |
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Definition
each gas exerts it's own pressure, not affected by other gases in the mixture and each individual pressure is called the partial pressure.
P total = Pa + Pb + Pc |
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Term
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Definition
| sum of the moles of each of the gases divided by each gases's individual moles and is expressed as an percent and can multiply by the pressure to get the partial pressure. |
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Term
| Collected over water gases |
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Definition
| MUST subtract the partial pressure of the vapor from the original pressure to find the pressure of the gas. |
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Term
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Definition
High Pressure (not much room), and low temperature (slow)
Must consider volume of particles
If conditions are extreme enough, may change into liquid |
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Term
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Definition
| High temperature (fast), low pressure (a lot of room) |
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Term
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Definition
KE= 1/2 mv2
1)Gases consist of tiny particles, atoms, or molecules 2) Volume of gas particle is irrelevant compared to the entire sample 3) Gas particles are in constant, random motion 4) No retractive/repulsive forces (move too fast) 5) When heat increases, then velocity, kinetic energy and average kinetic energy increases |
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Term
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Definition
| They flow, transmit & exert pressure equally in all directions, in constant & random motion, collisions are elastic (no loss of kinetic energy), mostly empty space, no free sides, and collisions with walls = pressure. |
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Term
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Definition
| Laws show what happens, so we can make predictions, theories try to explain why. |
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Term
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Definition
| average kinetic energy and is constant during a phase change |
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Term
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Definition
| a gas at a constant temperature and pressure has a volume directly proportional to the number of moles of gas |
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Definition
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Definition
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Definition
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Definition
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Definition
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Definition
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Term
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Definition
solid to gas
always occurs below the triple point |
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Term
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Definition
liquid to gas
occurs at specific temperature
occurs at the bottom
based on vapor pressure and atmospheric pressure |
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Term
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Definition
| movement of one material through another |
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Term
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Definition
| temperature and pressure at which all three phases exist |
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Term
| What happens to the density of a gas as it is compressed? |
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Definition
| It become more dense because there is less room with the same amount of particles present. |
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Term
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Definition
| temperature and pressure at and above which vapor and liquid are the same |
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Term
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Definition
| temperature at which the vapor pressure of a liquid is equal to the external pressure |
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Term
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Definition
liquid to gas below boiling point
occurs at the surface
based on vapor pressure of liquid |
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Term
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Definition
| temperature at 1.00 atm at which something boils |
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Term
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Definition
| increase the pressure, decrease the melting point |
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Term
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Definition
| closed container of water and air water evaporates into vapor until above liquid is saturated with vapor at point of saturation, the vapor condenses back into a liquid at the same rate the liquid evaporates |
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Term
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Definition
| reversible processes at the same rate |
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Term
| As vapor pressure increases... |
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Definition
| temperature increases, evaporation increases, number of particles increases, and collisions increase |
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Term
| What do air pockets do for water? |
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Definition
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