3 enthalpy
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3 Enthalpy
Units SI unit = joule
1KJ = 1000J = 239.0 cal
1st law of Thermodynamics
The total energy of the universe is constant
i.e energy cannot be created or destroyed but can be changed from one form to another.
Heat (or thermal energy) q is the energy transferred between a system and its surroundings as a result of a difference in temperature only.
All other forms of energy transfer (mechanical, electrical etc) involve some type of work, w, the energy transferred when an object is moved by a force.
State functions A state function is a property dependant on
the current state of the system (e.g. its composition, volume, temp etc)
It is independent of the path the system took to reach that state.
Energy of a system is a state function
So E is a constant for any given change but q and w may vary
(q and w are not state functions)
and E = q + w
Energy can be converted from one form to anothere.g. from mechanical heat electrical light etc.
Energy is released when bonds are madeEnergy is used when bonds are broken
Chemical reactions involve
Bond breakingBond forming
Energy changes for an exothermic reaction – one where heat is released to the surroundings
Energy changes for an endothermic reaction – one where heat is absorbed from the surroundings
Examples of exothermic reactions neutralisation burning hydrocarbons respiration
Examples of endothermic reactions photosynthesis dissolving ammonium nitrate in water
The chemical energy which a system possesses is its enthalpy. Enthalpy is the change in energy at constant pressure
symbol H
And H = H products – H reactants
if energy is absorbed by a system H is positive if energy is released by a system H is negative
Energy changes for an endothermic reaction
A—B + C—D
Reactants
A—C + B—D
Products
A B C D
Bond breaking
Bond forming
Overall energy change
Products have more energy than reactants
E
A—B + C—D
A—C + B—D
Products
Bond formingBond breaking
Overall energy change
EA B C D
Energy changes for an exothermic reaction
Products have less energy than reactants
Reactants
Energy Diagrams
E
Activation energy
H
Reactants
Products
An exothermic reaction
Time
Activation energy
H
Products
An endothermic reaction
E
Reactants
Reactants
Time
Standard enthalpy of formation is the heat absorbed when 1 mole of a substance is formed from its elements in their standard state.
The standard state of a substance is 1 mole of the substance in a specified state (solid, liquid, gas) at 1 atmosphere of pressure. The value of an enthalpy change is quoted for standard conditions: gases at 1 atm, solutions at unit concentration and substances in their normal states at a specified temperature. (usually 273K or 00C)
All elements in their standard state are assigned an enthalpy of formation of 0
Standard enthalpy of reaction is the heat absorbed in a reaction at constant pressure between the number of moles of reactant shown in the equation for the reaction.
Standard enthalpy of combustion is the heat absorbed when 1 mole of a substance is completely burned in oxygen at constant pressure.
Standard enthalpy of solution is the heat absorbed when 1 mole of a substance is dissolved at constant pressure in a stated amount of solvent. This may be 100g or 100ml or an ‘infinite’ amount, i.e. a volume so large that on further dilution there is no further heat change.
HrӨ depends only on the difference between the
standard enthalpy of the reactants and the standard enthalpy of the products, not on the route by which the reaction occurs.
This is Hess’s Law – If a reaction can proceed by more than one route the overall enthalpy is the same regardless of which route is followed.
Find the enthalpy change for the reaction CH2= CH2(g + HCl(g) C2H5Cl(g)
Given the following data
HfӨ = standard enthalpy change of formation
HfӨ CH2CH2 = +52.3 KJ mol-1
HfӨ HCl = - 92.3 KJ mol-1
HfӨ C2H5Cl = -105 KJ mol-1
H = HfӨ products - Hf
Ө reactants
HrӨ = -105 – (+52.3) + (-92.3)
= -65KJ mol-1
Note that the formula H = HfӨ products - HfӨ reactants
Applies when the data given is the enthalpy of formation.
If the data given is the enthalpy of combustion the following formula is used H = HcӨ reactants - HcӨ products
It doesn’t matter what the reaction is called. It may be called a combustion reaction but if the data given is the enthalpy of formation use the formula H = HfӨ products - HfӨ reactants !
Calculate the standard enthalpy of reaction for the following
2C + 2H2(g) + O2 CH3CO2H(l)
Given the following enthalpies of combustion
C -394 KJ/molH2(g) -286 KJ/mol
CH3CO2H(l) -876 KJ/mol
r = (2x -394) + (2x-286) – (-876) KJ/mol = -484 KJ/mol