Equilibrium

No significant changes as the overall balance between the intake and output of various acidic and basic substances remains unchanged regardless of macronutrient composition.

A slightly acidic urine due to the acidic nature of amino acids released during protein metabolism, versus the alkaline effects often associated with carbohydrate breakdown.

A slightly basic urine given the larger quantities of hydrogen ions consumed via increased carbohydrate ingestion, leading to excess acid neutralization.

Highly acidic urine due to the rapid accumulation of organic acids as the body struggles to maintain homeostasis with a high load of protein introduction into metabolic pathways.

Lowering volume tends increase collisions pushing equilibrium towards side with more gas moles produced regardless molar ratio present sides involved

Increasing pressure typically shifts the equilibrium towards fewer moles of gas being produced whether those are on side with reactants or products depends on stoichiometry

No matter what changes done atmospheric conditions end result remains same because intrinsic properties compounds dictate final outcome above external interventions applied

Applying additional external force under high pressures causes direct conversion all substances into liquid phase thereby eliminating any relevance regarding mole amounts per state present

Shifts in favor of products forming because heat acts as a reactant.

No shift occurs as temperature affects only rate but not position of equilibrium.

Shifts in favor of reactants due to decreased kinetic energy in system.

Shifts temporarily toward products then back to original balance as new dynamic equality establishes itself quickly after perturbance.

No effect because total number of particles remains unchanged.

Favors side with fewer moles due to lowered partial pressures.

Causes both forward and reverse reactions to speed up equally without shifting balance.

Favors side with more moles of gas due to increased entropy.

The concentration of that substance in solution.

The physical state of that substance.

The number of moles of that substance.

The temperature at which the reaction occurs.

Ionic bonding

London dispersion forces

Dipole-dipole interactions

Hydrogen bonding

When the exothermic reaction produces excess heat.

Neither reactants nor products are affected by the temperature change.

When increasing temperature creates a greater barrier for the endothermic direction only.

When the endothermic direction absorbs heat.

Adding an inert gas to the mixture without changing pressure or volume.

Increasing the total pressure in the system (if gases are involved).

Lowering the total pressure in the system (if gases are involved).

Removing one of the products from the mixture as it is formed.

The reaction will shift to the right.

There will be no effect on the direction of the reaction.

The reaction will shift to the left.

It is impossible to determine the effect on the direction of the reaction.

It slows down both forward and reverse reactions equally but doesn't affect equilibrium position.

A catalyst has no effect on either rate or direction of reversible reactions at chemical equilibrium.

It accelerates both forward and reverse reactions equally without shifting equilibrium position.

It shifts the equilibrium toward more products being formed.