# Gibbs Free Energy Flashcards Preview

## AP Bio > Gibbs Free Energy > Flashcards

Flashcards in Gibbs Free Energy Deck (13)
1
Q

Total energy =

A

usable energy + unusable energy

2
Q

H=

A

total potential energy

in a compound; based on enthalpy

3
Q

enthalpy

A

energy found in bonds of molecule

4
Q

∆H–negative v positive

A

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.

5
Q

Equation + explanation

A

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

6
Q

T

A

temperature in K

7
Q

S=

A

unusable energy

8
Q

Entropy-

A

disorder

9
Q

S–negative v positive

A

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

10
Q

G=

A

usable/ available energy, or Gibbs free energy

11
Q

free energy

A

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

12
Q

G–positive vs negative

A

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.

13
Q

Energy coupling

A

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