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.

Increased Surface Area Leads To Stronger Van Der Waals Attractions

Increased Volatility Due To Reduced Molecular Weight

Weaker Hydrogen Bonds Due To Strain On Bond Angles

Decreased Strength Of Hydroxyl Bonding

Activation energy

Entropy

Enthalpy

Free energy

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.

By increasing the pressure

By decreasing the temperature

By reducing the concentration of reactants

Through the use of coupled reactions

Fluorine (F)

Sodium (Na)

Oxygen (O)

Chlorine (Cl)

It has good capacity against bases but poor capacity against acids.

It can neutralize large amounts of added acid or base equally well.

Its pH significantly decreases upon addition of small amounts of strong base.

Adding strong acid shifts NH₄⁺/NH₃ ratio much more than CH₃COOH/CH₃COO⁻

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.