exergonic reaction
anode
oxidation happens, losing electrons
y + z --> Y+ + Z- (G<0)
how a reaction that is thermodynamically unfavorable occur
volumes proportionality with entropy
as V goes up, so does S
as the more temperature, the more energy, the mor entropy
Cell potential equation
x --> X+ + e-
the energy of a system related to changes in enthalpy and entropy, at a constant temperature.
basically implies that the system is at 1 atm and using 1 M solutions.
delta S =
(sum of S products) - (sum of S reactants)
DO NOT FORGET TO ACCOUNT FOR THE MOLES IN THE REACTION!!!
is H < 0 and S > 0
if a reaction is thermodynamically favorable
delta G and the energy of the product is lower than that of the reactants
1. G = negative = k>1; G = positive = k
voltage equation
V = IR
voltage = current (amps) * resistance (ohms)
cathode
reduction happens, gaining electrons
charging a battery vs using a battery
charging = non-spontaneous
using = spontaneous
3rd law of thermodynamics
as temperature goes to zero, entropy approaches a constant value
how do you calculate Gibbs free energy
cell potential, Ecell, electromotive force (emf)
1 joule of work / coulomb of charge transferred
J/C = units
G = negative = k>1
G = positive = k<1
k is close to 1, G is close to zero
k is far from 1, G is far from zero
galvanic cell vs electrolytic cell
entropy
is H < 0 and S < 0
T=100k
spontaneous, low temperature, T delta S is small
G, S, H
S = entropy
G = Gibbs free energy
H = heat energy
as matter disperses, entropy increase, so, going from solid to liquid to gas would increase entropy, whilst going from gas to liquid to solid would decrease it
2nd law of thermodynamics
galvanic cell
non-spontaneous is...
is H > 0 and S > 0
T = 500k
spontaneous, high temperature, T delta S is large
1st law of thermodynamics
if a reaction is kinetically favorable
it has k>1, relatively low activation energy
