NCSU Chem 101 Final - Lalloo

Exergonic

Spontaneous ΔG<O

Endergonic

Not Spontaneous ΔG>0

ΔS

Entropy

ΔH

Enthalpy

ΔG>0 —> Keq?

Keq<1

ΔG<0 —> Keq?

Keq>1

ΔG~0 —> Keq?

Keq~1

Endothermic

Solid —> Liquid —> Gas

Exothermic

Solid <— Liquid <— Gas

Solid —> Liquid —> Gas (ENDO)

ΔH>0 and ΔS>0

Solid <— Liquid <— Gas (EXO)

ΔH<0 and ΔS<0

ΣBroken-ΣFormed where do I put heat if ENDO vs EXO?

ENDO - Reactant Side

EXO - Product side

Soluble if

both polar or both are nonpolar

Insoluble if

one is polar and one is nonpolar

Work done ON the system

POSITIVE (+)

Work done BY the system

NEGATIVE (-)

ABSORB heat

POSITIVE (+)

RELEASE heat

NEGATIVE (-)

Select all that are driving forces behind a process (e.g. a chemical reaction): 

A. To lower the potential energy of the system

B. To raise the potential energy of the system

C. To minimize the number of ways the system can distribute its energy

D. To maximize the number of ways the system can distribute its energy

A. To lower the potential energy of the system

D. To maximize the number of ways the system can distribute its energy

Half Reactions: for oxidation put e^-

product side (M → Mn+ + ne1-)

Half Reactions: for reduction put e^-

reactant side (M^n+ + ne1- → M )

ΔG favorable?

ΔG<0

ΔH favorable?

ΔH<0

ΔS favorable?

ΔS>O

Increasing pressure shifts with _____ moles of gas

fewer

VESPR 2 LINEAR

180°

VESPR 3 TRIGONAL

120°

VESPR 4 TETRAHEDRAL

No LP: 109.5° 1+ LP: <109.5°