Applications of Thermodynamics

The rate of the reaction generally increases due to more frequent effective collisions between reactants.

Reaction rates decrease as excess reactants can inhibit catalytic processes if present beyond optimal levels.

The rate decreases because there is less space for molecular movement in solution.

There's no significant change unless temperature or pressure also changes simultaneously.

Activation Energy (Ea)

Entropy (S)

Gibbs Free Energy (G)

Enthalpy (H)

Catalyst

Product reagent

Excess reactant

Limiting reactant

The selectivity can be higher or lower under either control, depending on the specific reaction.

The selectivity is always higher under thermodynamic control.

The selectivity is always higher under kinetic control.

The selectivity is not affected by whether a reaction is under thermodynamic or kinetic control.

Equilibrium-controlled

Activation-controlled

Kinetically controlled

Thermodynamically controlled

The amount of reactants equals the amount of products.

All catalysts become inactive.

The system reaches maximum entropy.

The rate of the forward reaction equals the rate of reverse reaction.

Aging wine in barrels for several years allowing its flavors to develop fully through slow chemical reactions with oxygen.

Refining crude oil into gasoline using distillation based on differences in boiling points over time for separation efficiency.

Producing yogurt by letting milk ferment slowly until bacteria reach their optimal growth phase for acidity balance.

Manufacturing ammonia through the Haber process quickly at high temperatures before nitrogen and hydrogen gases reach their most stable state.

Ionic solids

Metallic solids

Molecular solids

Covalent network solids

Products have less energy than reactants

Products have higher enthalpy than reactants

Excess energy must be absorbed from surroundings

The process requires energy input to proceed

The rate of the reaction will decrease.

The temperature change will only affect product solubility, not reaction rate.

The rate of the reaction will remain constant.

The rate of the reaction will increase.