AMOUNT OF SUBSTANCE
relative atomic mass / Ar) =
theaveragemassofanatomlkg
Hz the mass of a carbon -12 atom 1kg7
relative molecular mass lMr1= total mass of the atoms in a formula or molecule 1kg)
emassof-
carbon -12 atom
1kg1 a
number (1)
avogadro's =
number of particles in a mole
number of atoms present of carbon -12
in
12g
"
6,022×10
Number of I ✗ n moles ( ) mass (9)
species
= n :
Mr / Ar
: 1000
µ
: 1000
concentration 1M) =
n lumber of molest
V 1 volume -
-
dem't mi dmi em
}
7 7
✗ 1000 ✗ 1000
(F)
concentration (c) =
m [mass (g) ]
V lvolvme Chill
""
ideal
gas
:
pV=nRT p
.
pressure 1Pa] v. I 100hPa
"000
:p
:
É
.
<
V. volume
-
1m ]
'
kPa fa If
n= moles ✗ 1000
+273
18.313K moi ] " '
A-
gas constant
F-
temperature 1k] v.
tip .
: 298K
empirical formula =
simplest whole number ratio of atoms of each element in a
compound
molecular formula the actual number of atoms of
=
each element in a
compound
empirical m RMMItablet =
molecular
^ RMM empirical
n
ratio
relative atomic mass / Ar) =
theaveragemassofanatomlkg
Hz the mass of a carbon -12 atom 1kg7
relative molecular mass lMr1= total mass of the atoms in a formula or molecule 1kg)
emassof-
carbon -12 atom
1kg1 a
number (1)
avogadro's =
number of particles in a mole
number of atoms present of carbon -12
in
12g
"
6,022×10
Number of I ✗ n moles ( ) mass (9)
species
= n :
Mr / Ar
: 1000
µ
: 1000
concentration 1M) =
n lumber of molest
V 1 volume -
-
dem't mi dmi em
}
7 7
✗ 1000 ✗ 1000
(F)
concentration (c) =
m [mass (g) ]
V lvolvme Chill
""
ideal
gas
:
pV=nRT p
.
pressure 1Pa] v. I 100hPa
"000
:p
:
É
.
<
V. volume
-
1m ]
'
kPa fa If
n= moles ✗ 1000
+273
18.313K moi ] " '
A-
gas constant
F-
temperature 1k] v.
tip .
: 298K
empirical formula =
simplest whole number ratio of atoms of each element in a
compound
molecular formula the actual number of atoms of
=
each element in a
compound
empirical m RMMItablet =
molecular
^ RMM empirical
n
ratio
