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Each element in the periodic table is assigned an
atomic mass.
One
atomic mass unit
(u)
is exactly onetwelfth the mass of an atom of carbon12. The
molecular mass
of a
molecule is the sum of the atomic masses of its atoms. The number of moles
n
contained
in a sample is equal to the number of particles
N
(atoms or molecules) in the sample
divided by the number of particles per
mole
N
A
,
n = N
/
N
A
, where
N
A
is
Avogadro's
number
and has a value of
N
A
= 6.022 × 10
23
particles per mole. The number of moles is
also equal to the mass of the sample (expressed in grams) divided by the mass per mole
(expressed in grams per mole). The mass per mole of a substance has the same numerical
value as the atomic or
molecular mass
of one of its particles.
The
ideal gas law
relates the absolute
pressure
P
, the volume
V
, the number of moles
n
, and the
Kelvin
temperature
T
of an
ideal gas
according to
PV = nRT
, where
R
= 8.31 J/
(mol · K) is the universal gas constant. An alternative form of the ideal gas law is
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This note was uploaded on 04/09/2008 for the course PHYS 101 taught by Professor Sharp during the Spring '08 term at Ohio State.
 Spring '08
 Sharp
 Mass

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