Chapter 20 & 21

energy is neither created nor destroyed; total energy content of the universe is constant

the amount of heat (q) absorbed by the system; the enthalpy change for a process is the same whether it occurs in a single step or a series of steps

on e for which a net change in amount(s) is observed to take place without intervention from outside the system; if under a given set of conditions a reaction is spontaneous, then its reverse is not spontaneous

• S = k ln(W)
• entropy = Boltzmann's constant (in J/Kelvin) x l(W), which are microstates
• for every process that occurs, the entropy of the universe will increase (ΔS_univ > 0)

is each way the particles and energy of our system can be distributed within the given volume, at the temperature given; all give the same measured values of P, V, n, T and E (internal energy)

• the entropy of the universe increases in a spontaneous process and remains unchanged in an equilibrium process
• ΔS_univ = ΔS_sys + ΔS_surr > 0

not the entire compound

compounds are oxidizing agents and reducing agents

NONSPONTANEOUS

not spontaneous, CANNOT occur; however the REVERSE of such a process (because it will be positive) is spontaneous

SPONTANEOUS at all temperatures!

SPONTANEOUS!

enthalpy change; aka the amount of heat absorbed by the SYSTEM

the system is at EQUILIBRIUM, so no net changes are occuring

entropy of universe = entropy of the system minus enthalpy of the system/Temp

• if basic, don't forget to add OH- to both sides of the half reaction
• -when figuring out how many e- to add to each side, make sure to factor in stoichiometry when calculating charges (if a compound has a 2 in front of it, you have to multiply the charge by 2)