5.2.2 Enthalpy and entropy Flashcards
what is entropy
the dispersal of energy in a system.
Entropy increases as a system becomes more disordered
what leads to entropy becoming more positive
-change of state eg-from solid to liquid OR liquid to gas
-reactions that produce a gas
-increases in the number of moles
-dissolving (solid dissolving in water)
eg-NaCl(s)——->NaCl(aq)
what leads to entropy becoming more negative
-change in state (gas to liquid or liquid to solid)
-decrease in the number of moles
-randomness of particles decreases
how do you calculate entropy changes
deltaS=products-reactants
-use molar ratio
what are entropy units
Jk-1 mol-1
are standard entropies positive or negative
positive
which has a larger increase in entropy
A) Solid to liquid
b) Liquid to Gas
B) liquid to gas
what is Gibbs equation
deltaG=deltaH-TdeltaS
what must deltaG be for a reaction to be feasible
deltaG<0
units for Gibbs equation
delta S must be divide by 1000
degrees c in K by +273
how do you work out the temperature the reaction is feasible
T=deltaH/deltaS