Potential, Free Energy, Equilibrium

ΔG°

________ is negative.

cell potential

E°cell= the standard ________.

standard potential

If the ________ (E°cell) of a redox reaction is negative, then the reaction is nonspontaneous at standard conditions.

ΔG°

________= the standard free energy change.

If the calculated standard cell potential (E°cell) of a redox reaction is positive, then

the reaction is spontaneous at standard conditions.

If the standard potential (E°cell) of a redox reaction is negative, then

the reaction is nonspontaneous at standard conditions.

A redox reaction is spontaneous if

E°cell is positive

ΔG° is negative

K is greater than 1

E°cell =

the standard cell potential

n =

the number of moles of electrons transferred in the balanced redox reaction.

F =

the Faraday constant; this is the charge of a mole of electrons; 9.648 × 104 J/mol . V

Voltage will increase and the reaction will become more spontaneous if

The concentration of a reactant is increased

The concentration of a product is decreased     (  smaller Q)

Voltage will decrease and the reaction will become less spontaneous if

The concentration of reactant is decreased

The concentration of product is increased   ( larger Q)

if Q < 1, then

E is GREATER than E°