Applications of Thermodynamics

The metal components within the engine naturally conduct external heat from the environment.

Friction between moving parts of the engine generates significant amounts of heat energy.

Endothermic reactions absorb heat from the surroundings, heating up the metal casing of the engine.

The engine's operation involves exothermic chemical reactions that release heat.

Varying the color of light passing through the reaction mixture.

Altering the partial pressures of gaseous reactants and products.

Switching the type of material used as a container for the reaction.

Changing the concentration of solid catalysts in the system.

H

G

S

E

Temperature in Kelvin

Heat transfer coefficient

Time over which reaction occurs

Total energy of products

There’s no effect on cell potential as it's independent of changes in temperature or entropy.

It decreases cell potential because higher temperatures favor reactions with negative entropy changes.

It increases cell potential because higher temperatures reduce kinetic energy barriers for electron transfer.

It increases cell potential because higher temperatures favor reactions with positive entropy changes.

Decreasing reactant concentrations while maintaining product levels constant.

Adding a step that couples it with a larger exergonic process.

Increasing system volume without changing molar quantities involved in reactions.

Implementing a catalyst that speeds up both forward and reverse reactions equally.

K decreases because increased temperature favors the reverse endothermic process according to Le Châtelier’s Principle.

K remains unchanged since equilibrium constants are not affected by changes in pressure or volume but only by catalysts which do not alter them either.

K fluctuates unpredictably since it depends on specific activation energies unique to each possible step within the overall exothermic process involved.

K increases due to more reactants converting into products with increased kinetic energy at higher temperatures.

The volume of the system decreases.

The disorder of the system increases.

The temperature of the system decreases.

The disorder of the system decreases.

Heat capacity (Cp)

Entropy (S)

Internal energy (U)

Enthalpy (H)

Microstates multiplicities increase during compression, raising positional momenta, which impacts negatively on ΔG.

Vibration speed of molecules enhances dramatically, shifting the equilibrium position and altering K but negligibly affecting ΔG.

The number of collisions per unit time goes up, converting kinetic forms of heat, affecting ΔH but not necessarily ΔG.

Rotational degrees of freedom become more accessible, thereby incrementing internal energies yet scarcely modifying ΔG.