chapters 13 and 14 Flashcards
How is temperature related to kinetic energy?
They are directly proportional
How do the melting points of ionic solids compare with those of molecular solids?
Molecular solids have higher melting points because ionic bonds are stronger than the covalent bonds in molecular solids.
Why does a real gas deviate from an ideal gas?
Because particles of real gases have mass and are affected by natural forces of attraction.
What gas under high pressure is closest to that of an ideal gas?
Hydrogen gas
Boyle’s law
P x V = constant
When P increases, V decreases. When V increases, P decreases.
Variables: P and V
Constants: # particles and temperature
mass at constant temp, gas inversely varies with pressure
Absolute zero
0K
When is a gas most likely to turn to a liquid?
When pressure increases and temperature decreases
760mmHg
1 atm
How does a barometer work?
As pressure increases, mercury goes up
What does the triple point on a phase diagram describe?
Equilibrium
What is vapor pressure?
A measure of the force exerted by a gas on a liquid in a closed container.
What are the fundamental assumptions of the kinetic theory of gases?
No attraction/repulsion, move random and rapidly, continue in a straight line and bounce off of walls/each other.
Charles Law
Variables: T and V
Constants: pressure
When T increases, V increases
E.G. balloon from freezer to room temp
Charles Law
Variables: T and V Constants: pressure When T increases, V increases E.G. balloon from freezer to room temp Mass is proportional to K temp if pressure is constant
Guy-Lussac’s Law
Variables: P and T Constants: volume and # particles When T increases, P increases If P decreases, T would decrease E.G. pressure cookers pressure is directly proportional to K temp is volume is constant
Kinetic energy
the energy an object has because of its motions
Atmospheric pressure
results from the collisions of atoms and molecules in air with objects
Condensation
the change of a gas or vapor directly to a liquid
intermolecular attractions
the forces between molecules
Normal boiling point
the boiling point of a liquid at a pressure of 101.3 kPa
Crystal
has a regular 3D arrangement of particles
unit cell
smallest group of particles within a crystal that remains in the geometric shape
amorphous
a solid with randomly arranged particles
melting point
the point at which a solid becomes a liquid
freeze drying
a method of removing water from food, using sublimation
phase diagram
graph that shows the relationship among the states of a substance
triple point for water
0.016C, 0.61 kPa
sublimation
change of solid to a vapor without going through the liquid phase
10 times the diameter of a particle
distance between particles in an enclosed gas at room temperature
compressibility
how much the volume of matter decreases under pressure
kPa
SI unit of pressure
piston
used to compress gas in a cylinder
combined gas law
P1xV1/T1 = P2xV2/T2
Absolute zero
0K or -273.15 C
ideal gas law
PV=nRT (R=3.81)
real gas
a gas that can be liquified by applying pressure, has mass
ideal gas
a gas that follows all gas laws at any condition of pressure and temperature
ideal gas constants
8.31(LxkPa/Kxmol)
partial pressure
the pressure exerted by each gas in a gaseous mixture
effusion
the escape of gas through a tiny hole in its container
law of effusion
rate of effusion of a gas is inversely proportional to the square root of it’s formulas
effusion equation
rate a/rate b = sq.rt. molar mass b/molar mass a
