The presence of a non-volatile solute lowers the vapor pressure of the solvent compared to that of the pure solvent.

Using Raoult's Law, the vapor pressure of the solution is P_total = (0.6 * 100) + (0.4 * 50) = 60 + 20 = 80 mmHg.

The total vapor pressure of a solution is the sum of the partial vapor pressures of its components: 80 mmHg + 20 mmHg = 100 mmHg.

For a spontaneous process, the change in Gibbs free energy (ΔG) is negative.

If the sum of clockwise moments equals the sum of counterclockwise moments, the object is in equilibrium.

According to Le Chatelier's principle, increasing the concentration of reactants will shift the equilibrium position to the right to favor the formation of products.

For equilibrium, the net force acting on the system must be zero.

The resultant force can be found using the Pythagorean theorem since the forces are perpendicular.

In a zero-order reaction, the rate is constant and does not depend on the concentration of reactants.

For a zero-order reaction, time = (initial concentration - final concentration) / k = (2 - 0) / 5 = 0.4 s.

In a zero-order reaction, the rate of reaction is independent of the concentration of reactants.

In an endothermic reaction, the enthalpy of the products is higher than that of the reactants.

In an ideal solution, the enthalpy of mixing is zero, indicating no heat is absorbed or released during mixing.

In an irreversible process, the change in entropy of the universe is positive, indicating that the total entropy increases.

In an isothermal process, the work done by the gas is given by W = nRT ln(Vf/Vi).

Reduction refers to the gain of electrons in a chemical reaction.

According to the Aufbau principle, the σ2s orbital is filled first before any other orbitals.

In O2, the π2p orbitals are the highest energy orbitals.

The energy levels of molecular orbitals can vary depending on the specific atoms and their electronegativities.

Nickel in [Ni(CO)4] undergoes sp3 hybridization as it forms four sigma bonds with CO ligands.

Saturation refers to the complete coverage of the adsorbent surface by the adsorbate.

The equilibrium constant Kc is dimensionless because it is a ratio of concentrations raised to their stoichiometric coefficients.

Adding SO2 will shift the equilibrium to the right to produce more SO3, according to Le Chatelier's principle.

Removing SO3 will shift the equilibrium to the right to produce more SO3.

In the Freundlich isotherm, K is the adsorption coefficient that indicates the extent of adsorption.

'n' represents the number of moles of the gas in the ideal gas equation.

The Langmuir isotherm assumes that all adsorption sites are identical and have the same energy.

'b' in the Langmuir isotherm represents the equilibrium constant related to the adsorption process.

In N2, the 2s orbitals (σ2s and σ*2s) are filled before the 2p orbitals.

π molecular orbitals can accommodate a maximum of 2 electrons, similar to all molecular orbitals.