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Enthalpy of a Reaction
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Enthalpy (
H
)
"
energy change
"
quantifies the
heat flow
into or out of the system in a process the occurs at
constant pressure
tells us about the "
heat content
" of a system
Enthalpy of Reactions (ΔH_rxn)
heat transferred
in a
chemical reaction
held at
constant pressure
the
difference
between the
enthalpies of the products
and the
enthalpies of the reactants
ΔH_rxn = H(products) - H(reactants)
ΔH > 0 (+): endothermic
ΔH < 0 (-): exothermic
Enthalpy Changes unit:
kJ/mol
Interpreting Thermochemical Equations
1.)
Physical states
of all the
reactants
and
products
must be
specified.
2.)
Reversing a reaction
would result in a
change
in
sign
but the
magnitude
of ΔH
remains the same.
3.)
Multiplying
both sides of the equation by a
factor n
, would also change ΔH by the
same factor n.
4.) The
stoichiometric coefficients
always refer to the
number of moles
of a substance.
Standard Molar Enthalpy of Formation (ΔHof)
Standard states:
natural state
of a substance at 1 atm
an
element
in its
standard state
has an ΔHof =
0 kJ/mol
Standard Molar Enthalpy of Formation (ΔHof)
Formation Reaction:
a reaction where
one mole
of a substance is
formed
from elements in their
standard states
It is a formation reaction if it satisfied all of the following:
both reactants are in their standard states
only 1 mole of the product is produced
Standard Enthalpy of Reaction (ΔHo_rxn)
enthalpy of a reaction
carried out at
1 atm
ΔHo_rxn = ∑(nΔHof products) - ∑(nΔHof reactants)
For calculating ΔHo_rxn:
Direct
Method
use when only
one
equation/reaction is given
Indirect
method
for
multiple step
reactions
Hess Law:
the
overall enthalpy change
in
converting reactants to products
is the
same
, regardless if it took place in
one step
or
multiple steps reaction
Hess law:
Balance
the chemical reaction.
Align
the
reactants
and
products
in the
same position
as the
one-step
(
main
) process.
Manipulate
the
coefficients
align with the
main process.
Cancel
like
substances
in
reactants
and
products.
Add the enthalpies.
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