2nd law with entropyas 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
voltage equation
how a reaction that is thermodynamically unfavorable occur
x --> X+ + e-
1st law of thermodynamicsin an isolated system energy can neither be created or destroyed; only transferred or converted, meaning E lost = negative E gained
exergonic reactionproducts have less energy than reactants, spontaneous, graph will end lower than it started
if a reaction is kinetically favorableit has k>1, relatively low activation energy
Frozen!
Frozen!
S = entropy
G = Gibbs free energy
H = heat energy
as V goes up, so does S
as the more temperature, the more energy, the mor entropy
spontaneous at all Temps, delta G <0
how do you calculate Gibbs free energydelta G = delta H - (T * delta S)
gibbs free energy = enthalpy - (temperature times entropy)
*note T is in kelvin, not Celsius
delta S =(sum of S products) - (sum of S reactants)
DO NOT FORGET TO ACCOUNT FOR THE MOLES IN THE REACTION!!!
cell potential, Ecell, electromotive force (emf)
2nd law of thermodynamics
what is Gibb's free energy
entropydegrees of freedom of a molecule
delta G and the energy of the product is lower than that of the reactants
1. G = negative = k>1; G = positive = k
overall cell reaction
Frozen!
Frozen!
galvanic cellchemical energy is converted to electrical energy with spontaneous redox reaction
Voltage
consists of oxidizing agent in one compartment that pulls electrons through a wire from a reducing agent
Cell potential equationEcell = E (cathode) - E (anode)
IMPORTANT: if the reaction gets reversed (in order to balance, sometimes it will need to be reversed), the sign of the Ecell must switch, however if it gets multiplied (in order to balance) IT REMAINS THE SAME!!
3rd law of thermodynamicsas temperature goes to zero, entropy approaches a constant value
Boost!
Boost!
chemical energy is converted to electrical energy with spontaneous redox reaction
Voltage
consists of oxidizing agent in one compartment that pulls electrons through a wire from a reducing agent
reduction happens, gaining electrons
Boost!
Boost!
cell potential, Ecell, electromotive force (emf)1 joule of work / coulomb of charge transferred
J/C = units
volumes proportionality with entropyas V goes up, so does S
as the more temperature, the more energy, the mor entropy
if a reaction is kinetically favorableit has k>1, relatively low activation energy
exergonic reactionproducts have less energy than reactants, spontaneous, graph will end lower than it started
is H < 0 and S > 0spontaneous at all Temps, delta G <0
G, S, HS = entropy
G = Gibbs free energy
H = heat energy
galvanic cell vs electrolytic cell
what is Gibb's free energy
x --> X+ + e-
how do you calculate Gibbs free energydelta G = delta H - (T * delta S)
gibbs free energy = enthalpy - (temperature times entropy)
*note T is in kelvin, not Celsius
how K and G relate to each other
voltage equationV = IR
voltage = current (amps) * resistance (ohms)
how a reaction that is thermodynamically unfavorable occur
Frozen!
Frozen!
entropydegrees of freedom of a molecule
in an isolated system energy can neither be created or destroyed; only transferred or converted, meaning E lost = negative E gained
non-spontaneous is...
anodeoxidation happens, losing electrons
if a reaction is thermodynamically favorabledelta G and the energy of the product is lower than that of the reactants
1. G = negative = k>1; G = positive = k
is H < 0 and S < 0T=100k
spontaneous, low temperature, T delta S is small
overall cell reaction
2nd law with entropyas 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
delta S =
Cell potential equation
charging a battery vs using a battery
Frozen!
Frozen!
entropy of an isolated system is never decreasing, only if it is in a 2 or more system
is H > 0 and S > 0T = 500k
spontaneous, high temperature, T delta S is large