Applications of Thermodynamics

The third law of thermodynamics

The second law of thermodynamics

The first law of thermodynamics

Hess's Law

Electron affinity values grow progressively larger, making it harder to give up the lone outer shell particle.

Heavier isotopes, those closer to the bottom, tend to display reduced rates due to mass inertia effects.

Atomic size decreases, and reactivity diminishes due to the stronger effective nuclear charge experienced by the remaining shells.

Reactivity increases as larger atoms exhibit lower ionization energies, thus losing valence electrons more readily.

An increase in entropy from splitting phosphate groups makes subsequent enzymatic actions spontaneously favorable.

The phosphorylation state change directly triggers all necessary enzyme conformations without energetic input.

The small amount of heat produced during ATP hydrolysis increases temperature enough to favor subsequent enzymatic actions.

The large negative ΔG associated with ATP hydrolysis provides sufficient free energy to drive multiple types of unfavorable biochemical reactions.

It becomes zero as one process absorbs exactly as much energy as the other releases.

It remains positive since both processes require input of energy.

It could be negative if the ATP hydrolysis releases sufficient free energy.

The sign cannot be determined without information on enthalpy changes only.

Energy must be added continuously for either Reaction X or Y to proceed spontaneously.

Both reactions are non-spontaneous despite a combined negative ΔG° value.

Reaction X inhibits Reaction Y from occurring due to its positive ΔG° value.

Reaction Y drives Reaction X forward by making the overall ΔG° negative.

Sodium (Na)

Lithium (Li)

Fluorine (F)

Potassium (K)

Graduated cylinder

Flask

Test tube

Beaker

Substrate-level phosphorylation

Photosynthesis

Redox reactions

Energy coupling

Reduction processes eliminate the need for regularly recharging devices as they produce electricity independently.

The batteries concentrate large amounts of electricity through single unpaired redox responses.

It allows spontaneous oxidation reactions to provide the necessary electricity to drive non-spontaneous reduction reactions.

Oxidation reactions occur separately from reduction reactions, leaving excess charge inside the battery.

The decomposition of sodium chloride in water softening systems.

The electrolysis of water for hydrogen fuel generation on its own.

The refinement of crude oil into various petroleum products without additional input.

The production of ammonia via the Haber process.