Thermochemistry Presentation

Submitted By : Quazi Md Muktadir
ID : 142002040
Topic : Thermo-Chemistry
Date : 17/07/2014

Topic Contains:
• What is Thermo Chemistry ?
• Define Origin of Heat of Reaction..
• Exothermic Reaction..
• Endothermic Reaction..
• Graphical representation of Exothermic
and Endothermic reactions..
• Different type of heat reactions..
• Hess’s law..

What is Thermochemistry ?
Thermochemistry is the study of
the energy and heat associated
with chemical reactions and/or physical
transformations. A reaction may release
or absorb energy, and a phase change may
do the same, such as
in melting and boiling.

Origin of Heat of Reaction
In a chemical reaction, the amount of heat that
must be added or removed in order to keep all of
the substances present at the same temperature.
Some reactions will release energy and some
reactions will adsorb energy and the energy will
work here is Heat.
Whenever a chemical reaction will occur, it will
release heat or will adsorb heat.

In a
Reaction
Heat Released Heat adsorbed
So, We can get two different types of Heat of Reaction.

Exothermic Reaction
Many reactions release energy in the form of heat,
light, or sound. These are exothermic reactions.
In a chemical reaction, the amount of energy
required to break the old bonds of the reactants is
lower than amount of energy released for
formation of new bonds of the products and
thereby heat is transferred from system to
surrounding is referred to as Exothermic reaction.

Energy required to
break the old bonds
of reactants
molecules
Energy release for
formation of new
bonds of the
products molecules<
System Surrounding
Heat transfer

Endothermic Reaction
An endothermic reaction is any chemical
reaction that absorbs heat from its
environment.
In a chemical reaction, the amount of energy
required to break the old bonds of the reactants is
higher than amount of energy released for
formation of new bonds of the products and
thereby heat is penetrated from surrounding to
system is referred to as Exothermic reaction.

Energy required to
break the old bonds
of reactants
molecules
Energy release for
formation of new
bonds of the
products molecules>
System Surrounding
Heat transfer

Graphical representation of Exothermic
and Endothermic reactions
A graph is scatted out putting time or rate of
reaction or reaction coordination along x axis
against energy or heat along y axis. Let A and B
two reactants produce C and D two products by a
reaction.
If the reaction release heat then it will be
exothermic reaction and if the reaction adsorb heat
then it will be endothermic reaction.

Different type of heat reactions
There are four different types of heat
reactions. Those are:
• Heat of formation
• Heat of decomposition
• Heat of combustion
• Enthalpy or Heat of Neutralisation

Heat of Formation
The heat of formation of a
compound may be defined as the
quality of heat change during the
formation of one mole of a
substance from this constituent
elements.

For example, the standard enthalpy of
formation of carbon dioxide would be the
enthalpy of the following reaction under the
conditions above:
C(s,graphite) + O2(g) → CO2(g) ; ∆Hf = -393.5 kJ/mol
Here all elements are written in their standard
states, and one mole of product is formed. This
is true for all enthalpies of formation.

Heat of Decomposition
The amount of heat required to
decompose 1 mole of a substance to its
constituent elements is called Heat of
Decomposition.
H2O (l) = ½ O2 (g) + ½ H2 (g) ;
∆H = +285.5 kJ/mol

Heat of Combustion
The heat of combustion of a compound or
an element is defined as the amount of heat
evolved, when 1 mole of a substance is
burnt completely in oxygen at a given
temperature at 1 atm. Pressure.
CH4 (g) + 2O2 (g) CO2 (g) =2H2O (l) ; ∆H = -890
𝑘𝐽
𝑚𝑜𝑙

Enthalpy or Heat of Neutralisation
Heat of Neutralisation is defined as the
change of heat or enthalpy during the
formation of one mole of water by the
neutralisation reaction of required
amounts of an acid and a base.
HCl (aq) + NaOH (aq) = NaCl (aq) = H2O (l) ; ∆H = -57.34
𝑘𝐽
𝑚𝑜𝑙

Hess’s Law
If a reaction can take place
by more then one routes the
overall change in enthalpy
is the same whichever route
is followed.

Illustration of Hess’s Law
Let us assume that a reactant A gives product
D directly by a single step and its change of
enthalpy is ∆H1.
A D
∆H1

Now the same reactant A produce D into
two steps. First A is converted into B
with an enthalpy change ∆H2 and in the
2nd step intermediate product B is
converted in to D with enthalpy change
∆H3.
A B B D
∆H2 ∆H3

According to the Hess’s law, we get
∆H1 = ∆H2 + ∆H3

It follows also that the standard enthalpy change
for the reaction DA is -∆H and for AD is +
∆H.

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