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Gas Laws, Moles & Gas Properties | Definitions
Diffusion
The spontaneous spreading out of a substance from an area of higher concentration to an area of lower concentration.
Equal volumes of gases under the same conditions of temperature and pressure contain equal numbers of molecules.
Boyle's Law
For a fixed mass of gas kept at constant temperature, the volume is inversely proportional to the pressure.
Charles' Law
For a fixed mass of gas kept at constant pressure, the volume is directly proportional to the temperature (measured on the Kelvin scale).
Gay Lussac's Law of Combining Volumes
When gases react, the volumes consumed in the reaction bear a simple whole number ratio to each other and to the volumes of any gaseous products under the same conditions of temperature and pressure.
Ideal Gas
A gas that perfectly obeys all of the gas laws at all temperatures and pressures. No such gas exists.
Equation of State for an Ideal Gas
PV = nRT
Mole
A mole of any substance is defined as the amount of that substance that contains as many particles as there are atoms in 12g of the C-12 isotope.
L = 6 x 10^23 per mole.
Relative Molecular Mass (Mr)
The average mass of a molecule of that substance compared with one twelfth of the mass of the carbon-12 isotope.
Molar Mass
The mass in grams of one mole of a substance, e.g. 1 mole of sodium has a mass of 23g.
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Gas Laws, Moles & Gas Properties | Definitions
Diffusion
The spontaneous spreading out of a substance from an area of higher concentration to an area of lower concentration.
Equal volumes of gases under the same conditions of temperature and pressure contain equal numbers of molecules.
Boyle's Law
For a fixed mass of gas kept at constant temperature, the volume is inversely proportional to the pressure.
Charles' Law
For a fixed mass of gas kept at constant pressure, the volume is directly proportional to the temperature (measured on the Kelvin scale).
Gay Lussac's Law of Combining Volumes
When gases react, the volumes consumed in the reaction bear a simple whole number ratio to each other and to the volumes of any gaseous products under the same conditions of temperature and pressure.
Ideal Gas
A gas that perfectly obeys all of the gas laws at all temperatures and pressures. No such gas exists.
Equation of State for an Ideal Gas
PV = nRT
Mole
A mole of any substance is defined as the amount of that substance that contains as many particles as there are atoms in 12g of the C-12 isotope.
L = 6 x 10^23 per mole.
Relative Molecular Mass (Mr)
The average mass of a molecule of that substance compared with one twelfth of the mass of the carbon-12 isotope.
Molar Mass
The mass in grams of one mole of a substance, e.g. 1 mole of sodium has a mass of 23g.
Cut dotted horizontal lines. Fold vertical line.
Diffusion
The spontaneous spreading out of a substance from an area of higher concentration to an area of lower concentration.
Equal volumes of gases under the same conditions of temperature and pressure contain equal numbers of molecules.
Boyle's Law
For a fixed mass of gas kept at constant temperature, the volume is inversely proportional to the pressure.
Charles' Law
For a fixed mass of gas kept at constant pressure, the volume is directly proportional to the temperature (measured on the Kelvin scale).
Gay Lussac's Law of Combining Volumes
When gases react, the volumes consumed in the reaction bear a simple whole number ratio to each other and to the volumes of any gaseous products under the same conditions of temperature and pressure.
Ideal Gas
A gas that perfectly obeys all of the gas laws at all temperatures and pressures. No such gas exists.
Equation of State for an Ideal Gas
PV = nRT
Mole
A mole of any substance is defined as the amount of that substance that contains as many particles as there are atoms in 12g of the C-12 isotope.