,1. Stoichiometric relationships
Element The mole concept
.
a single pure substance made of only one type of atom No . of particles = no . Of moles × Avogadro constant
,
( n ) ( L )
G. 02 × 1023
Compound Mass of 1 molecule =
g.o×o }
•
chemical combination of different elements
,
containing fixed
ratio of atoms
Relative atomic mass
'
pure substance formed when two or more elements combine chemically
.
average mass of the naturally occurring isotopes of the element
relative to the mass of ¥ of an atom of carbon -
12
Mixtures
-
composed of two or more substances in which no chemical
Relative formula mass
combination has occurred .
sum of weighted average of masses of atoms in a formula
unit relative to % Of an atom of carbon -12
1
Homogeneous mixture
-
has uniform composition and properties throughout
-
can be separated by physical means
Mole
.
the amount of substance that contains 6.02 ✗ 1023 particles
2 Heterogeneous mixture
.
has non - uniform composition and properties is not the same
throughout Molar mass
,
mass of one mole of any substance
.
can be separated by mechanical means
mass (g)
NO Of moles =
ass
.
'
( 9m01 )
_
States of matter
solid liquid gas
arrangement close packed more spaced spread out
inter particle weak negligible Empirical formula
force strong
-
simplest whole number ratio of atoms
movement vibrate at fixed slide over move freely
position
Molecular formula
actual / real no Of atoms
shape / Volume fixed fixed shape fixed
'
no no
.
fixed V01 Shape / V01
Calculation Of Empirical formula
kinetic theory of matter
element
.
average kinetic theory of particle is directly related to the molar mass
010 by mass n =
temperature empirical formula mass
Ar
-
temperature is a measure of average kinetic energy of
moles
particles of a substance
/ by smallest no
Diffusion
.
particles of a substance become evenly distributed as a
Limiting reactant
,
-
determines the amount of product that can form
result of their random movements
Theoretical yield
-
quantity of product that can form from complete conversion
changes of state of limiting reactant
so ,
,Éiiga ,
0/0 yield =
e×Perimen+atY
theoretical yield
× you %
ᵗ"É
law
Avogadro 's
-
equal volumes of all gases when measured at same temp
,
and pressure ,
contain equal number of particles
endothermic
exothermic
.
V x n
Volume
no - Of moles of gas =
molar volume
Heating curve molar volume is the volume occupied by one mole of
any
.
gas
B / C
$
C -1g
,
Mp / FP
, conditions STP
of Ideal gas
22.7 dm"mor-I obeys the ideal DV=nRT under all conditions
gas law
273K /00C ·no such thing as an ideal gas
100kPa known as
all gases are real gases
A
200
Gas laWS high temp
1000K
Gas behave like an ideal gas at
Boyle's Law
- deal gas
low pressure
relationship between volume and pressure
p/pa
·
pct
PV a
=
constant
2 Assumptions made in describing ideal gas in kinetic molecular theory
volume of gas particles is negligible (molecules have no volume
p P PV
2
there are no attractive forces between particles
I
↓ P
Charle's Law
p
zV
+
-
b RT
=
relationship between volume and temperature
VxT Concentration a
of solution
I a
= constant is
solvent p resentin
component the quantity
greatest
V V
n cV
=
gdm moldm
=
mass required const x
Mr Xthe
on
T(0 T(K)
Dilution of solutions
C,V, (zVz
=
Gay-Lussac's law
·relationshipbetween pressure and temperature
pxT
I a
=
constant
Volumetric Analysis
T
determine the concentration a
of solution
P P
Titration
T(0) T(k) ·used determine
to the reacting volumes precisely
changes colour at its end point
Relationship between P.V and + To find concentration
unknown acid
of
P conch
n(alkali) = vo l
x
ifpressure
PCI a
of gas is doubled c onstant
at
n(acid) =
temperature then volume will be halved
[acid] I
V Acid Alkali->
+
Salt +H20
V
VaT
if temperature is doubled the volume will double
Back titration
used when the concentration is too small
T(K
P
pdT mass s olute
of
concentration in ppm = 106
is doubled will double mass s olution
of
if temperature the pressure
T/K
=volumeofgasan
combined gas laws
E a
=
constant
xHy (x
1)02xCO2 Hc0
#Y P2V
+ + +
=
19 1000mg
=
The ideal gas equation
19 0.001
=
kg
PV n RT
=
pressure Pa
= kPa:X
by 103
volume =
m3 am3: -103 cm3: =106
m oleS n
no. of =
temperature K
= 0: +
273
PV =
RT Mr =
m.piT RT =
d =
density
Element The mole concept
.
a single pure substance made of only one type of atom No . of particles = no . Of moles × Avogadro constant
,
( n ) ( L )
G. 02 × 1023
Compound Mass of 1 molecule =
g.o×o }
•
chemical combination of different elements
,
containing fixed
ratio of atoms
Relative atomic mass
'
pure substance formed when two or more elements combine chemically
.
average mass of the naturally occurring isotopes of the element
relative to the mass of ¥ of an atom of carbon -
12
Mixtures
-
composed of two or more substances in which no chemical
Relative formula mass
combination has occurred .
sum of weighted average of masses of atoms in a formula
unit relative to % Of an atom of carbon -12
1
Homogeneous mixture
-
has uniform composition and properties throughout
-
can be separated by physical means
Mole
.
the amount of substance that contains 6.02 ✗ 1023 particles
2 Heterogeneous mixture
.
has non - uniform composition and properties is not the same
throughout Molar mass
,
mass of one mole of any substance
.
can be separated by mechanical means
mass (g)
NO Of moles =
ass
.
'
( 9m01 )
_
States of matter
solid liquid gas
arrangement close packed more spaced spread out
inter particle weak negligible Empirical formula
force strong
-
simplest whole number ratio of atoms
movement vibrate at fixed slide over move freely
position
Molecular formula
actual / real no Of atoms
shape / Volume fixed fixed shape fixed
'
no no
.
fixed V01 Shape / V01
Calculation Of Empirical formula
kinetic theory of matter
element
.
average kinetic theory of particle is directly related to the molar mass
010 by mass n =
temperature empirical formula mass
Ar
-
temperature is a measure of average kinetic energy of
moles
particles of a substance
/ by smallest no
Diffusion
.
particles of a substance become evenly distributed as a
Limiting reactant
,
-
determines the amount of product that can form
result of their random movements
Theoretical yield
-
quantity of product that can form from complete conversion
changes of state of limiting reactant
so ,
,Éiiga ,
0/0 yield =
e×Perimen+atY
theoretical yield
× you %
ᵗ"É
law
Avogadro 's
-
equal volumes of all gases when measured at same temp
,
and pressure ,
contain equal number of particles
endothermic
exothermic
.
V x n
Volume
no - Of moles of gas =
molar volume
Heating curve molar volume is the volume occupied by one mole of
any
.
gas
B / C
$
C -1g
,
Mp / FP
, conditions STP
of Ideal gas
22.7 dm"mor-I obeys the ideal DV=nRT under all conditions
gas law
273K /00C ·no such thing as an ideal gas
100kPa known as
all gases are real gases
A
200
Gas laWS high temp
1000K
Gas behave like an ideal gas at
Boyle's Law
- deal gas
low pressure
relationship between volume and pressure
p/pa
·
pct
PV a
=
constant
2 Assumptions made in describing ideal gas in kinetic molecular theory
volume of gas particles is negligible (molecules have no volume
p P PV
2
there are no attractive forces between particles
I
↓ P
Charle's Law
p
zV
+
-
b RT
=
relationship between volume and temperature
VxT Concentration a
of solution
I a
= constant is
solvent p resentin
component the quantity
greatest
V V
n cV
=
gdm moldm
=
mass required const x
Mr Xthe
on
T(0 T(K)
Dilution of solutions
C,V, (zVz
=
Gay-Lussac's law
·relationshipbetween pressure and temperature
pxT
I a
=
constant
Volumetric Analysis
T
determine the concentration a
of solution
P P
Titration
T(0) T(k) ·used determine
to the reacting volumes precisely
changes colour at its end point
Relationship between P.V and + To find concentration
unknown acid
of
P conch
n(alkali) = vo l
x
ifpressure
PCI a
of gas is doubled c onstant
at
n(acid) =
temperature then volume will be halved
[acid] I
V Acid Alkali->
+
Salt +H20
V
VaT
if temperature is doubled the volume will double
Back titration
used when the concentration is too small
T(K
P
pdT mass s olute
of
concentration in ppm = 106
is doubled will double mass s olution
of
if temperature the pressure
T/K
=volumeofgasan
combined gas laws
E a
=
constant
xHy (x
1)02xCO2 Hc0
#Y P2V
+ + +
=
19 1000mg
=
The ideal gas equation
19 0.001
=
kg
PV n RT
=
pressure Pa
= kPa:X
by 103
volume =
m3 am3: -103 cm3: =106
m oleS n
no. of =
temperature K
= 0: +
273
PV =
RT Mr =
m.piT RT =
d =
density
