Use LEFT and RIGHT arrow keys to navigate between flashcards;
Use UP and DOWN arrow keys to flip the card;
H to show hint;
A reads text to speech;
20 Cards in this Set
- Front
- Back
barometer
|
A device used to measure atmospheric pressure. A tube filled with mercury and inverted into a dish full of mercury. At sea level the mercury rises 760mm above the dish.
|
|
manometer
|
A device used to measure the pressure of a gas in an experiment. In a close-ended one the difference in column heights = gas pressure. In an open-ended one Pgas = Patm - difference in height.
|
|
pascal
|
SI unit for pressure; the force of one newton exerted on an area of one square meter.
|
|
standard atmosphere (atm)
|
101.325 kPa; 1.01325 x 10^5 Pa
|
|
mmHg
|
Based on measurement with a barometer or manometer. 1 torr; 1/760atm; 133.322 Pa; 101.325/760kPa
|
|
bar
|
1 x 10^2kPa; 1 x 10^5 Pa
|
|
Boyle's Law
|
At constant temperature, the volume occupied by a fixed amount of gas is inversely proportional to the applied (external) pressure. V is proportional to 1/P [T and n fixed].
|
|
Charles's Law
|
At constant pressure, the volume occupied by a fixed amount of gas is directly proportional to its absolute (Kelvin) temperature. V is proportional to T [P and n fixed].
|
|
0K
|
The temperature at which an ideal gas would have zero volume.
|
|
pressure-temperature relationship
|
At constant volume, the pressure exerted by a fixed amount of gas is directly proportional to the absolute temperature. P is proportional to T [V and n fixed].
|
|
relationship between volume and amount
|
At fixed temperature and pressure, the volume occupied by a gas is directly proportional to the amount (mol) of gas. V is proportional to n [P and T fixed].
|
|
Avogadro's Law
|
At fixed temperature and pressure, equal volumes of any ideal gas contain equal numbers of particles (or moles).
|
|
standard temperature and pressure (STP)
|
0 degrees Celsius (273.15K) and 1atm (760torr/mmHg)
|
|
standard molar volume
|
22.4L - At STP the volume of 1 mol of an ideal gas is the standard molar volume.
|
|
universal gas constant
|
The R in PV=nRT. R=PV/nT or 0.0821 atm x L / mol x K
|
|
how we get one of the laws from the ideal gas law
|
P1V1/n1T1 = P2V2/n2T2, cancel out the constant variables
|
|
how to find density using the ideal gas law
|
m/V = d = MP/RT
|
|
how to find mass or molar mass using the ideal gas law
|
PV = m/M x RT
|
|
ideal gas law
|
PV = nRT; This law holds for virtually any gas, whether pure or a mixture, at ordinary conditions because gases mix homogeneously in any proportions and each gas in a mixture behaves as if it were the only gas present.
|
|
Dalton's law of partial pressures
|
Ptotal = P1 + P2 + P3...
|