Reaction Thermodynamics, Equilibrium, and Kinetics

△E formula

△E = Q + W

△E is change in internal energy of the system

△H formula

△H = Q + W

△H is enthalpy

△G formula

△G = △G* + RTlnK

decrease in enthalpy (△H)

makes reaction more favorable

Increase in △S

Makes reaction more favorable

Third law

Entropy is zero at absolute zero temperature

What causes a -△G

a decrease in enthalpy

an increase in entropy

Which △G is favorable?

Negative △G

Exergonic reactions are…

Favorable

-△G

Endergonic reactions are…

NOT favorable

Positive △G

Rxn at standard conditions

NOT at equilibrium

standard H+ concentration

at PH=7 [H+] is 10^-7M

other standard concentrations

1M

standard conditions

R = 8.314 J/mol*K or 0.008314 KJ/mol*K

T = temp in K = C + 273

everything besides water = 1 M

When Q<K

reaction is exergonic and favors forward

△G is negative

When Q>K

Reaction is endergonic and favors reverse

△G is positive