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Chemistry AS
Unit 2
Topic 6
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enthalpy change
heat energy change
measured at
constant pressure
Standard conditions for enthalpy change:
specified temperature - normally
298K
100
kPa
1
mole of specified
substance
all
reactants
and
products
in their standard state
units are always kJ/mol
exothermic
where
heat energy
is
transferred
from the
system
to the
surroundings
, and has a
negative
sign
endothermic
where
heat energy
is
transferred
from the
surroundings
to the system, and has a
positive
sign
standard enthalpy change of formation
enthalpy change when
1 mole
of substance is formed from its
elements
in their
standard
state at
100 kPa
and a specified
temperature
The standard enthalpy change of
formation
of an
element
is always
0.
standard enthalpy change of combustion
enthalpy change when
1
mole of a substance burns
completely
in
excess oxygen
under
standard conditions
of 100 kPa and a specified temperature
The standard enthalpy change of combustion is always
exothermic
, so always has a
negative
sign.
standard enthalpy change of neutralisation
enthalpy change when an
acid
and an
alkali
react under standard conditions of
100
kPa and a specified temperature to form
1
mole of water
The standard enthalpy change of neutralisation is always
exothermic
, so always has a
negative
sign. It's ionic equation is
H+
+
OH-
->
H2O.
standard enthalpy change of atomisation
enthalpy change for the
formation
of
one
mole of
gaseous
atoms from the
element
in
standard
state
The standard enthalpy change of atomisation is always
exothermic
, so always has a
negative
sign.
energy transferred (J) =
mass
(
g
) x
specific heat capacity
(
J g-1 C-1
) x
temperature change
(
C
)
Once energy transferred is calculated, divide by
1000
to convert from
J
to
kJ
, then divide by
moles.
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