whole concert
-
- define the term "mole" in terms of =
the amount Ofa substance that contains as many elementary entities
the avogadro's constant as there are atoms in exactly 129 Of carbon 12
* 1m01 Of any substance __ 6022×1023 particles
19mn the mass Ofa carbon I2A-1OM =L -661×10-24 grams
-
=
- 1 amu ...
-
=
represents the average mass of the naturally occurring mixture of isotopes
- define relative atomic mass based
on the carbon-12 scale
average mass = -19mn ✗ I. abundance / +
[ amux -
1. abundance ] -1 . . .
- how to calculate average mass (C)
the massinatomicmassunitslamulofan individual molecule
=
~
to calculate
- definition of molecular mass . . .
Molecular mass of 1-120=211 ) -116=189 my
=
unit used when during empirical formula
- what is formula mass
I. molecular formula =
the type and number of atoms in a molecule
- molecular formula vs empirical ~
H20
formula 2 empirical formula = the simplest formula
~
used to indicate the mole ratio of elements in a compound
~
glucose empirical formula -_
CH20
~
glucose molecular formula =C6Hi2Oo
-
formula mass also used to denote the sum of the atomic weights of the atoms
- what is the formula mass used to in empirical formula Mr Of GLUCOSE = 61121+12+6116)
denote / =
1809mn
~
molecular formula = [ 64,20 ,
empirical formula __ CH20
\ empirical formula mass __ 12+2+16
= 309mn
- what is the avogadro's number -
Na =
6.022×1023 MO1
'
'
6.022×1023 particles
- 1 mol of any substance ...
= ~
1m01 =
=
the mass ofamoleofa substance
- define molar mass ~
molar mass __
91m01
numerically equal -10 atomic mass of an element / molecular moss
-
Of a compound
- formulas to convert mass to mole mass -_ M01 ✗ 191m01 )
to particles (& vice versa) MO11 from mass )=
Grams
91m01
mass
M01 MAY MO1 ( from particles )= 6.022×1023
particles
particles (from mot )
=
MO1X 6.022×1023
=
alistofthepercentbymassofeaonelenentina compound
- what is the percent composition by ~
☐
to mass of an element __
n ✗ atomic mass of element
"
molecular /formula mass of compound
mass Where n-_ number Ofatomsoftreelementinamolecule / formula unit
- formula
=
The empirical formula only gives the ratio of atoms in molecule
- why may there be multiple
compounds with the same empirical
formula
-
- define the term "mole" in terms of =
the amount Ofa substance that contains as many elementary entities
the avogadro's constant as there are atoms in exactly 129 Of carbon 12
* 1m01 Of any substance __ 6022×1023 particles
19mn the mass Ofa carbon I2A-1OM =L -661×10-24 grams
-
=
- 1 amu ...
-
=
represents the average mass of the naturally occurring mixture of isotopes
- define relative atomic mass based
on the carbon-12 scale
average mass = -19mn ✗ I. abundance / +
[ amux -
1. abundance ] -1 . . .
- how to calculate average mass (C)
the massinatomicmassunitslamulofan individual molecule
=
~
to calculate
- definition of molecular mass . . .
Molecular mass of 1-120=211 ) -116=189 my
=
unit used when during empirical formula
- what is formula mass
I. molecular formula =
the type and number of atoms in a molecule
- molecular formula vs empirical ~
H20
formula 2 empirical formula = the simplest formula
~
used to indicate the mole ratio of elements in a compound
~
glucose empirical formula -_
CH20
~
glucose molecular formula =C6Hi2Oo
-
formula mass also used to denote the sum of the atomic weights of the atoms
- what is the formula mass used to in empirical formula Mr Of GLUCOSE = 61121+12+6116)
denote / =
1809mn
~
molecular formula = [ 64,20 ,
empirical formula __ CH20
\ empirical formula mass __ 12+2+16
= 309mn
- what is the avogadro's number -
Na =
6.022×1023 MO1
'
'
6.022×1023 particles
- 1 mol of any substance ...
= ~
1m01 =
=
the mass ofamoleofa substance
- define molar mass ~
molar mass __
91m01
numerically equal -10 atomic mass of an element / molecular moss
-
Of a compound
- formulas to convert mass to mole mass -_ M01 ✗ 191m01 )
to particles (& vice versa) MO11 from mass )=
Grams
91m01
mass
M01 MAY MO1 ( from particles )= 6.022×1023
particles
particles (from mot )
=
MO1X 6.022×1023
=
alistofthepercentbymassofeaonelenentina compound
- what is the percent composition by ~
☐
to mass of an element __
n ✗ atomic mass of element
"
molecular /formula mass of compound
mass Where n-_ number Ofatomsoftreelementinamolecule / formula unit
- formula
=
The empirical formula only gives the ratio of atoms in molecule
- why may there be multiple
compounds with the same empirical
formula
