Thermodynamics Flashcards
What’s the difference between kinetics and thermodynamics?
Kinetics: Speed of a reaction
Thermodynamics : Energy changes associated with a reaction
What is the first law of thermodynamics
The first type of energy we will consider is enthalpy (H).
You cannot just measure an enthalpy, you must measure a change in enthalpy (ΔH).
ΔH
amount of heat energy given out or taken in as a reaction proceeds at a particular temperature.
A reaction may be EXOTHERMIC or ENDOTHERMIC
Units = kJ per mole of reactant, i.e. kJmol-1
Exothermic
ΔH is negative
Endothermic
ΔH is positive
Hess’s Law of Constant Heat Summation
The enthalpy change going from reactants to products is the same regardless of which route is taken
Entropy
Entropy is harder to understand as it refers to the order (or disorder) in a system.
High entropy = high disorder
You can increase entropy by heating or providing more space for the molecules
The entropy of a liquid is higher than a solid and a gas is higher than a liquid
As T=0 is neutral entropy then entropy
is usually positive (but not always)
Gibbs free energy
At constant temperature and pressure (i.e. enthalpy is zero):
ΔG = - T ΔS
Therefore it is another way of expressing
entropy at a constant temperature
Van’t Hoff Equation
For a reversible reaction, the equilibrium constant can be measured at a variety of temperatures then plot lnKeq vs. 1/T.
This is the van ‘t Hoff plot and is widely used to estimate the enthalpy and entropy of a chemical reaction.
By measuring the equilibrium constant, Keq, at different temperatures, the Van ‘t Hoff plot can be used to assess a reaction when temperature changes.
Knowing the slope and intercept from the van ‘t Hoff plot, the enthalpy and entropy of a reaction can be easily obtained:
ΔH = - R x slope
ΔS = R x intercept
The van ‘t Hoff plot can be used to quickly determine
the enthalpy of a chemical reaction both
qualitatively and quantitatively.