Word 

Definition 

1 
3^{rd} law of thermodynamics 



2 
Absolute zero 
(0 K) 
The temperature at which the volume of an ideal gas becomes zero; a theoretical coldest temperature that can be approached but never reached. Absolute zero is zero on the Kelvin scale, 273.15°C on the Celsius scale, and 459.67°F on the Fahrenheit scale. 

3 
Atmosphere of pressure 
(atm) 
A unit of pressure, equal to a barometer reading of 760 mm Hg. 1 atmosphere is 101325 pascals and 1.01325 bar. 

4 
average kinetic energy 



5 
Avogadro’s law 

Equal volumes of an ideal gas contain equal numbers of molecules, if both volumes are at the same temperature and pressure. For example, 1 L of ideal gas contains twice as many molecules as 0.5 L of ideal gas at the same temperature and pressure. 

6 
Barometer 

An instrument that measures atmospheric pressure. A mercury barometer is a closed tube filled with mercury inverted in a mercury reservoir. The height of the mercury column indicates atmospheric pressure (with 1 atm = 760 mm of mercury). An aneroid barometer consists of an evacuated container with a flexible wall. When atmospheric pressure changes, the wall flexes and moves a pointer which indicates the changing pressure on a scale. 

7 
Boyle’s Law 

The pressure of a ideal gas is inversely proportional to its volume, if the temperature and amount of gas is held constant. Doubling gas pressure halves gas volume, if temperature and amount of gas don't change. If the initial pressure and volume are P_{1} and V_{1} and the final pressure and volume are P_{2}V_{2}, then P_{1}V_{1} = P_{2}V_{2} at fixed temperature and gas amount. 

8 
C to K conversion 



9 
Charles’ Law 

The volume of a gas is directly proportional to its temperature in kelvins, if pressure and amount of gas remain constant. Doubling the kelvin temperature of a gas at constant pressure will double its volume. If V_{1} and T_{1} are the initial volume and temperature, the final volume and temperature ratio V_{2}/T_{2} = V_{1}/T_{1} if pressure and moles of gas are unchanged. 

10 
Combined gas law 



11  
12 
Dalton’s law of partial pressure 
Dalton's law 
The total pressure exerted by a mixture of gases is the sum of the pressures that each gas would exert if it were alone. For example, if dry oxygen gas at 713 torr is saturated with water vapor at 25 torr, the pressure of the wet gas is 738 torr. 

13  diffusion  When particles move from areas of high concentration to areas of low concentration. For example, if you open a bottle of ammonia on one end of the room, the concentration of ammonia molecules in the air is very high on that side of the room. As a result, they tend to migrate across the room, which explains why you can smell it after a little while. Be careful not to mix this up with effusion  
14 
Directly proportional 



15  effusion  When a gas moves through an opening into a chamber that contains no pressure. Effusion is much faster than diffusion because there are no other gas molecules to get in the way.  
16  gas laws  
17 
GayLussac’s law 



18 
GayLussac’s law of combining volumes of gases 



19 
Graham’s law of effusion 



20  ideal gas  
21 
Ideal gas constant 
(R) ideal gas constant; universal gas constant. 
A constant R equal to PV/(nT) for ideal gases, where the pressure, volume, moles, and temperature of the gas are P, V, n, and T, respectively. The value and units of R depend on the units of P, V, and T. Commonly used values and units of R include: 82.055 cm^{3} atm K^{1} mol^{1}; 0.082055 L atm mol^{1} K^{1}; 8.31434 J mol^{1} K^{1}; 1.9872 cal K^{1} mol^{1}; 8314.34 L Pa mol^{1} K^{1}; 8.31434 Pa m^{3} mol^{1} K^{1}. 

22 
Ideal gas law 
ideal gases; perfect gas; 
A gas whose pressure P, volume V, and temperature T are related by PV = nRT, where n is the number of moles of gas and R is the ideal gas law constant. Ideal gases have molecules with negligible size, and the average molar kinetic energy of an ideal gas depends only on its temperature. Most gases behave ideally at sufficiently low pressures. 

234 
Inversely proportional 



24 
K to C conversion 



25 
Millimeters of mercury 



26  monoatomic gas  
27 
Newton 



28 
Partial pressure 

The pressure of one gas in a mixture. For example, if you had a 50:50 mix of helium and hydrogen gases and the total pressure was 2 atm, the partial pressure of hydrogen would be 1 atm. 

29 
Pascal 
(Pa) 
The SI unit of pressure, equal to a force of one newton per square meter. 101325 pascals = 1 atmosphere; 10^{5} pascals = 1 bar. 

30 
Pressure 
(P) 
Force per unit area. The SI unit of pressure is the pascal, defined as one newton per square meter. Other common pressure units are the atmosphere, the bar, and the Torr. 

31  Standard Atmospheric Pressure  
32 
Standard molar volume of gas 

The volume of 1 mole of an ideal gas at STP, equal to 22.414 liters. 

33 
STP 
standard temperature and pressure. 
Used to describe a substance at standard pressure and a temperature of 0°C (273.15 K). 

34  Temperature  
35 
Universal gas constant 
Ideal gas constant 


36  volitile  A substance with a high vapor pressure. 