Real gases experience intermolecular forces, which causes deviations from ideal behavior.

A catalyst lowers the activation energy of a reaction, thereby increasing the rate without being consumed.

A saturated solution is in dynamic equilibrium where the rate of dissolution equals the rate of crystallization.

Adsorption is generally an exothermic process, as it releases energy.

In an endothermic reaction, heat is absorbed from the surroundings.

Catalysts provide an alternative pathway with a lower activation energy, thus increasing the reaction rate without being consumed.

Chemisorption involves the formation of a chemical bond and is generally an irreversible process.

Colligative properties depend on the number of solute particles, not their identity.

Dynamic equilibrium occurs when the rate of the forward reaction equals the rate of the reverse reaction, not necessarily when concentrations are equal.

Enthalpy is a state function, meaning it depends only on the initial and final states, not the path taken.

Entropy is a state function, meaning it depends only on the state of the system and not on how it reached that state.

The correct equation for Gibbs Free Energy is ΔG = ΔH - TΔS, which relates enthalpy, entropy, and temperature.

Ideal solutions obey Raoult's Law without any deviation, meaning their properties are consistent with the law across all concentrations.

Non-ideal solutions show positive or negative deviations from Raoult's Law due to interactions between different molecules.

Raoult's Law is primarily applicable to ideal solutions, where the solute and solvent behave similarly.

Oxidizing agents are reduced in redox reactions.

The activation energy (Ea) of a reaction is always positive.

Activation energy is always positive as it represents the minimum energy required for a reaction to occur.

The boiling point of a liquid increases with increasing atmospheric pressure.

For second period elements, σ2p is lower in energy than π2p.

The equilibrium constant (K) is dependent on temperature; it changes with temperature variations.

The equilibrium constant Kc is dependent on temperature; changing the temperature will change the value of Kc.

The Langmuir adsorption isotherm assumes that adsorption occurs in a monolayer on a surface with a finite number of identical sites.

O2 has 2 unpaired electrons in its molecular orbital configuration, making it paramagnetic.

Molecular orbital theory explains the magnetic properties of molecules, such as paramagnetism in O2.

The rate of a reaction generally increases with increasing temperature.

The rate of reaction decreases with time for a reactant and increases with time for a product.

The Van der Waals equation accounts for the volume of gas particles and intermolecular forces.

Gases can be compressed the most due to the large spaces between particles.

Solids have a definite shape and volume due to closely packed particles.