Photosynthesis is an endothermic process as it absorbs energy from sunlight.

Physisorption involves weak van der Waals forces, and the adsorption of oxygen on activated charcoal is a classic example.

Volume is an extensive property, as it depends on the amount of substance present.

Adsorption is a surface phenomenon, while absorption is a bulk phenomenon.

Chemisorption is typically irreversible, unlike physisorption which is reversible.

Gases do not have a definite volume; they expand to fill their container.

Liquids have a definite volume but take the shape of their container, hence they do not have a definite shape.

Raoult's Law is applicable under conditions of ideal solutions, and high pressure is not a requirement.

Raoult's Law applies to ideal solutions, and it is not necessary for the solute to be volatile.

Color of solute does not affect its solubility; solubility is influenced by temperature, pressure, and the nature of solute and solvent.

The color of the solute does not affect its solubility; solubility is influenced by temperature, pressure, and the nature of the solute and solvent.

Increasing temperature generally decreases the rate of adsorption for exothermic processes, while the other options increase the rate.

The kinetic molecular theory assumes that gas particles do not attract each other, which is why option 3 is NOT a postulate.

Heat is not a state function; it depends on the path taken during a process.

All listed options are states of matter; however, 'Plasma' is often considered a fourth state, while 'Bose-Einstein condensate' is another state not listed.

Henry's law describes solubility, not adsorption, while Langmuir, Freundlich, and BET are types of adsorption isotherms.

The kinetic molecular theory assumes that gas particles do not attract or repel each other.

The van der Waals equation is (P + a(n/V)^2)(V - nb) = nRT.

The mole is the SI unit for measuring the amount of substance.

Molality is defined as moles of solute per kilogram of solvent, hence the unit is mol/kg.

Molarity is defined as moles of solute per liter of solution, hence the unit is mol/L.

A buffer solution resists changes in pH upon the addition of small amounts of acid or base.

A saturated solution contains the maximum amount of solute that can dissolve at a given temperature.

In an exothermic reaction, the enthalpy change (ΔH) is negative because heat is released.

Entropy is a measure of disorder in a system, and it tends to increase in spontaneous processes.

The Freundlich adsorption isotherm is applicable to heterogeneous surfaces and describes multilayer adsorption.

For a spontaneous process, the Gibbs free energy change (ΔG) is less than 0 (ΔG < 0).

A negative Gibbs free energy change (ΔG < 0) indicates that the process is spontaneous.

Heat capacity depends on the amount of substance; it is not a constant value.

In an endothermic reaction, heat is absorbed, resulting in a positive ΔH.