Term
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Definition
| Mass of 1 atom in amu (Atomic Mass Units) |
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Term
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Definition
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Term
| Atomic Mass is the number |
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Definition
| below the element in the periodic table |
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Term
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Definition
| Mass of 1 molecule or 1 formula unit (for Ionic compounds) in amu |
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Term
| To derive Formula Mass you |
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Definition
| Add Atomic masses of all elements in the formula |
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Term
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Definition
| Mass of one mole in grams |
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Term
| Molar Mass for an element |
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Definition
| is the number below the element in the periodic table (atomic mass) in grams |
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Term
| For the molar mass of a compound |
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Definition
| add the atomic masses of all the elements in the in grams |
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Term
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Definition
| Amount that contains Avogado's number of units (Atoms, molecules, or ions). |
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Term
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Definition
| Is the number of particles in one mole of a substance |
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Term
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Definition
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Term
| Avogadro's number equality |
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Definition
| 1 mol = 6.022 X 10^23 Particles |
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Term
| Avogadro's conversion factor |
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Definition
6.002 X 10^23 Particles / 1 Mol
1 Mol / 6.002 X 10^23 Particles |
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Term
| Avogadro's Number converts |
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Definition
Moles of a substance to number of particles of a substance
Number of particles of a substance to moles. |
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Term
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Definition
| collection that contains 6.022 X 10^23 of particles (atoms, molecules, or ions) |
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Term
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Definition
Gases have no definite shape or volume
Fill the whole volume of any container
Molecules are far apart
Can be easily compressed |
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Term
| Kinetic Molecular Theory of Gases |
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Definition
Gas consist of small particles that
Move randomly in straight lines, with high velocities.
are very far apart and have essentially no attractive or repulsive forces
Have Very small volumes compared to the volume of the container they occupy
have kinetic energies that increase with an increase in temperature. |
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Term
| Properties of Gases described in terms of four properties |
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Definition
Pressure
Volume
Temperature
Amount |
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Term
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Definition
| The force exerted by a gas against the walls of a the container. |
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Term
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Definition
| The space occupied by the gas |
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Term
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Definition
Liters (L)
Milliliters (mL) |
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Term
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Definition
| Determines the kinetic energy |
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Term
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Definition
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Term
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Definition
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Term
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Definition
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Term
| For gas we always us what for our calculations |
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Definition
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Term
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Definition
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Term
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Definition
| pressure exerted by a column of air from the top of the atmosphere to the surface of the earth |
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Term
| What is the atmospheric Pressure at sea level |
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Definition
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Term
| what happens to atmospheric pressure at high altitudes |
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Definition
| it becomes lower because the density of air is less |
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Term
| Below sea level atmosphere pressure is |
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Definition
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Term
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Definition
| is used to measure atmospheric pressure |
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Term
| Barometers indicate atmospheric pressure as the |
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Definition
| height in mm of the mercury column |
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Term
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Definition
The pressure of a gas is inversely related to its volume when T and n are constant.
If pressure increases then volume decreases |
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Term
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Definition
| The Kelvin temperature of a gas is directly related to the volume when P and n are constant. |
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Term
| Charles's law when the temperature of a gas increases |
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Definition
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Term
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Definition
| The pressure exerted by a gas is directly related to the Kelvin temperature, when V and n are constant |
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Term
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Definition
The volume of a gas is directly related to the number of moles of gas when T and P are constant
when the number of moles of a gas increases its volumes increases. |
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Term
| Dalton's Law of partial pressure |
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Definition
| the partial pressure of a gas is the pressure exerted by each gas in a mixture. |
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Term
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Definition
| Pressure created by the vapor molecules above the surface of liquid |
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Term
| Vapor Pressure increases as |
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Definition
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Term
| At the boiling point of liquid |
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Definition
| vapor pressure above the liquid is equal to the atmospheric pressure |
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Term
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Definition
| are homogeneous mixtures of two or more substances |
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Term
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Definition
| of a solvent and one or more solutes |
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Term
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Definition
| in the solvent to make a solution |
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Term
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Definition
| not react with each other, Just mix |
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