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Level 65

Conversion Factors


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1 km = ? mi
1 km = 0.6214 mi
1 mi = ? ft
1 mi = 5280 ft
1 mi = ? km
1 mi = 1.609 km
1 m = ? yd
1 m = 1.034 yd
1 in = ? cm
1 in = 2.54 cm
1 cm = ? in
1 cm = 0.3937 in
1 angstrom = ? m
1 angstrom = 10?¹° m
1 kg = ? lb
1 kg = 2.205 lb
1 lb = ? g
1 lb = 453.6 g
1 lb = ? oz
1 lb = 16 oz
1 amu = ? g
1 amu = 1.661 x 10?²4 g
0 K = ? °C
0 K = -273.15 °C
0 K = ? °F
0 K = -459.7 °F
K = ?
K = °C + 273.15
°C =
°C = 5 / 9 (°F - 32°)
°F =
°F = 9 / 5 °C + 32°
1 J = ? kg-m²/s²
1 J = 1 kg-m²/s²
1 J = ? cal
1 J = 0.239 cal
1 J = ? C x ? V
1 J = 1 C x 1 V
1 cal = ? J
1 cal = 4.184 J
1 eV = ? J
1 eV = 1.602 x 10?¹? J
1 Pa = ? N/m²
1 Pa = 1 N/m²
1 Pa = ? kg/m-s²
1 Pa = 1 kg/m-s²
1 atm = ? Pa
1 atm = 101325 Pa
1 atm = ? torr
1 atm = 760 torr
1 atm = ? lb/in²
1 atm = 14.7 lb/in²
1 bar = ? Pa
1 bar = 105 Pa
1 torr = ? mmHg
1 torr = 1 mmHg
1 L = ? m³
1 L = 10?³ m³
1 L = ? dm³
1 L = 1 dm³
1 L = ? cm³
1 L = 10³ cm³
1 L = ? qt
1 L = 1.057 qt
1 gal = ? qt
1 gal = 4 qt
1 gal = ? L
1 gal = 3.784 qt
1 cm³ = ? mL
1 cm³ = 1 ml
1 in³ = ? cm³
1 in³ = 16.4 cm³1 km
100cm
1 m
1 cm
10 mm
1,000,000mm
1 km
1 L
1,000 mL
1 kg
1,000 g
1g
1,000 mg
1,000,000mg
1 kg
km
distance (kilometers)
m
Mol/dm3
cm
centimeter
mm
millimeter
L
thickness of material
ml
Anywhere between + or - l
cubic centimeter
cc or cm3
kg
kilogram
g
symbol of acceleration due to gravity
Mg
What does Fg equal
Water
during the electrolysis of brine, ? molecules are more easily reduced than sodium ions.
1 pt
2 cups
1 qt
4 cups
1 gal
3.79 L
1 tsp
60 drops (gtt)
1 glass
8 fl. oz.
30 mL
1 fl. oz.
1 cup
8 fl. oz.
1 T
3 tsp
1 oz
30 g
2 T
1 fl oz
1 lb
454 g
16 cups
1 gal
Democritus
(460-370 BCE) A Greek philosopher who theorized that all matter could be reduced to particles that could not be divided, which he described as "atomos."
Boyle
called atoms simple bodies
elements
simplest type of matter with unique physical and chemical properties
submicroscopic
macroscopic properties are dependent on these characteristics
compounds
_______ are formed by the chemical combination of two or more of the same or different kinds of atoms.
mixture
A _______ is a combination of two or more substances that do not change chemically when you mix them.
element
2 Hydrogen atoms bonded together is a _______
Dalton
atomic theory based on experiments:
Lavoisier
started the mass conservation discussion
mass conservation
the number of substances and their properties change but the mass remains constant
definite composition
a particular compound of the same elements in the same parts by mass
mass fraction
the part of the compounds mass that each element contributes
Multiple proportions
if element a and b react to form two compounds, the different masses of b that combine with a fixed mass of can be expressed as a ratio of small whole numbers
atoms
all elements are comprised of tiny particles called_______
cathode ray
glass tube with no air inside
Electron
A negatively charged subatomic particle located in the electron cloud outside the nucleus. It determines how atoms combine with other atoms.
tv
modern cathode ray
Thomson
did the cathode ray experiment
Millikan
measured the charge of an electron
Rutherford
had a nucleus based atomic model
Atom
Basic building block of all matter.
Positive
Anode (Electrolytic Cell)
1/20000
nucleus size in relation to the atom
10^14
nuclear density of the atom
isotopes
atoms of the same element that have different masses: the same protons, but different neutrons -same chemical properties
1.66x10^-24
1 amu = _______ grams
wavelength
The distance from a point on a wave and the same point on the next cycle of the wave is called?
frequency
How many wave peaks pass a certain point per given time
amplitude
(A) length of the electric field at wave maximum
speed of light
Ultimate speed in universe
3.00 x 10^8
speed of light constant
monochromatic light
single wavelength
laser
light amplified by stimulated emission of radiation
polychromatic light
multiple wavelengths of light
10^-10
1 Angstrom = _______ m
refraction
occurs when light waves bend as they pass from one material to another
Vacuum
Empty space where there are no gas molecules to collide with anything
diffraction
when waves bend around an object
blackbody radiation
a solid object emits visible light when it is heated
incandescent light bulb
example of blackbody radiation
color
changes as the temperature of light changes
Wedgewood
noted that all objects became red at the same time in the kiln regardless of the material
brighter
the hotter the object, the _______ the light
white
hottest color
Planck
said energy can be finite
The Quantum theory
if only certain quantities of energy are emitted and this energy is emitted by the atoms in the matter then the atoms must be quantized in regards to their energy
particle
energy is treated like a
photon theory
tiny bundles of energy called photons could explain the observations
einstein
came up with the photon theory
energy and frequency
these two are related to each other according to the photon theory
intensity and number of photon
these two are related to each other according to the photon theory
line spectra
a series of fine lines at specific frequencies separated by black spaces
Rydberg
studied the line spectra of hydrogen
classical physics
indicates that a negative particle moving in a curved path around a positive particle must emit radiation and lose energy
Bohr
father of figuring out the construction of the atom
stationary states
the H atom has certain energy levels called these
ground state
the lowest allowable energy state of an atom
radiate energy
an atom does not do this while in a stationary state
excited state
A state in which an atom has a higher potential energy than it has in its ground state
2.18x10^-18 J
the energy of a Hydrogen atom when n=1
De Broglie
said that an objects wavelength is inversely proportional to its mass
momentum
the amount of force needed to chage its motion; it's product of mass and velocity, p=mv
Heisenberg
said that it is impossible to simultaneously know both the position and momentum of a moving particle
The Quantum-Mechanical model of the atom
each solution of the equation gives an energy state that is associated with a given atomic orbital
probability density
a measure of the probability of finding an electron of a particular region of the atom
the principal quantum number
indicates the relative size of the orbital and its distance from the nucleus
the angular momentum quantum number
indicates the shape of the orbital
the magnetic quantum number
indicates the spatial orientation of the orbital
x-ray, uv, visible, infrared, microwaves, radio
arrange them in order of increasing wavelength
charge of an electron
Millikan's oil drop experiment validated the
infrared, visible, and ultraviolet
excited hydrogen atoms radiate energy in these regions
10^12
tera
10^9
giga
10^6
mega
10^3
Energy 1 kJ
10^2
hecto
10^1
deka
10^-1
deci
10^-2
centi
10^-3
milli
10^-6
micro
10^-9
nano
10^-12
pico
10^-15
femto