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Gravity
Gas Law with kinetic molecular theory review
Terms in this set (30)
Gas
State of matter in which particles have high kinetic energy, low density, and weak IMFs
Kinetic Molecular Theory
Describes the characteristics and behavior of gas particles: have mass; low density; in constant, random, rapid motion; exert pressure; elastic collisions; exert no force on one another
Ideal Gas
A gas that behaves exactly as the Kinetic Molecular Theory describes
Elastic Collisions
A collision in which no kinetic energy is lost; gas particles have same speed before and after the collision
Barometer
An instrument that measures the pressure of gas particles in the atmosphere
Manometer
An instrument that measures the pressure of a gas in a closed container
Boyle's Law
States that as volume decreases, pressure increases and vice versa; P1V1=P2V2
Charles' Law
States that as temperature increases, volume increases and vice versa; V1/T1=V2/T2
Gay-Lussac's Law
States that as temperature increases, pressure increases and vice versa; P1/T1=P2/T2
Combined Gas Law
Relates the pressure, volume, and temperature of a gas; P1V1/T1=P2V2/T2
Avogadro's Law
States that the quantity and volume of a gas are directly proportional; v1/n1=v2/n2
Ideal Gas Law
A combination of Avogadro's Law and the Combined Gas Law; relates all gas variables through the Universal Gas Constant; PV=nRT
Universal Gas Constant (R)
A number that allows all gas variables to be related; used in the Ideal Gas Law equation; equal to 0.0821 L
atm/mol
K
Dalton's Law of Partial Pressures
The total pressure of a mixture of gases is the sum of the individual pressures (Ptotal=P1+P2+P3...)
Graham's Law
The lighter the gas particle, the faster it will diffuse and effuse
Diffusion
When gas particles move through one another, eventually becoming evenly distributed throughout the mixture
Effusion
When gas particles escape through an opening one at a time
Mole
The SI unit for quantity. One of these is equal to 6.02 x 10^23 particles.
Volume
The amount of 3-dimensional space occupied by an object
Molar Volume
The space taken up by one mole of particles (22.4 L for any gas)
Temperature
A measure of the average kinetic energy of the particles of a substance
Pressure
The force exerted on a given area
STP
Equal to 1 atm and 273K
Kinetic Energy
Energy of motion; speed
Inversely Proportional
As the value of one variable increases, the value of the other decreases and vice-versa (e.g., pressure and volume)
Directly Proportional
As the value of one variable increases, the value of the other increases and vice-versa (e.g., temperature and volume, temperature and pressure)
Gas Density
The mass of gas particles in a given amount of space; formula mass/22.4 L
Faulty Assumptions of KMT
1) that gas particles have no volume; 2) that there are no IMFs between gas particles
When Real Gases are Not Like Ideal Gases
Low temperature and/or high pressure
Equivalent Units of Pressure
1 atm, 760 mmHg, 760 torr, 101,325 Pa, 101.325 kPa, 14.7 psi
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