Gibbs Free Energy

Question 1

Total energy =

Answer 1

usable energy + unusable energy

Question 2

H=

Answer 2

total potential energy

in a compound; based on enthalpy

Question 3

enthalpy

Answer 3

energy found in bonds of molecule

Question 4

∆H–negative v positive

Answer 4

If ∆H, or the change in H during a reaction is negative, that means that energy is being released. This is spontaneous.

We want to have a –∆H because that means that with regard to the
total energy of the system, energy has been released.

Question 5

Equation + explanation

Answer 5

∆G = ∆H – (T∆S)
Free (available) energy = change in total energy – (temperature x
Change in disorder)

Question 6

T

Answer 6

temperature in K

Question 7

S=

Answer 7

unusable energy

Question 8

Entropy-

Answer 8

disorder

Question 9

S–negative v positive

Answer 9

If ∆S is positive, then randomness has increased, which is spontaneous

We want ∆S
to be positive because that means randomness is increased, which
is more spontaneous. The – sign in front of the S will make the ∆G
also more negative

Question 10

G=

Answer 10

usable/ available energy, or Gibbs free energy

Question 11

free energy

Answer 11

Free energy- portion of a system’s energy that can perform work

Question 12

G–positive vs negative

Answer 12

If free energy is released by a reaction, (meaning that the free
energy at the end of the reaction is less than the free energy at the
start of the reaction), ∆G will be negative. This means that the
reaction is spontaneous.

Question 13

Energy coupling

Answer 13

using the energy from the exergonic reactions to
power the endergonic ones
Cells usually use ATP as a coupling agent. By breaking down
ATP and releasing energy, that energy can be used to
power an endergonic reaction
a -7.3 could power a +5.4