Detailed Reason:
A solution shows positive deviation from Raoult's Law when the cohesive forces between like molecules (A-A and B-B interactions) are stronger than the adhesive forces between unlike molecules (A-B interactions). Because the A-B attraction is weaker, molecules can escape more easily into the vapor phase, resulting in a higher vapor pressure than predicted by Raoult's Law.

Detailed Reason:
Phenol and water form a classic partially miscible liquid pair. At room temperature, they do not mix in all proportions and separate into two distinct liquid phases (a phenol-rich aqueous layer and a water-rich phenol layer). They only become completely miscible above their upper critical solution temperature (UCST) of approximately $66.8^\circ C$.

Detailed Reason:
Raoult's Law states that the relative lowering of the vapor pressure of a dilute solution containing a non-volatile solute is equal to the mole fraction of the solute in the solution. Formula: $\frac{P^\circ - P}{P^\circ} = X_{solute}$.

Detailed Reason:
Adding a non-volatile solute (like common salt, NaCl) to a solvent (water) lowers the vapor pressure of the solvent. As a result, a higher temperature is required for the vapor pressure to equal the atmospheric pressure, leading to an elevation in boiling point. It also causes a depression in freezing point.

Detailed Reason:
According to Le Chatelier's principle, a decrease in volume (which causes an increase in pressure) shifts the equilibrium towards the side with the fewer number of moles of gas.
In reaction (D), there are 2 moles of gas on the left and 3 moles of gas on the right. Therefore, an increase in pressure will shift the equilibrium to the left (towards 2 moles).

Detailed Reason:
In thermodynamics, a multi-component system is in chemical equilibrium when the chemical potential ($\mu$) of each component is equal across all phases. This implies that there is no net driving force for matter to move from one phase to another or for a reaction to proceed in a net direction ($\Delta G = 0$).

Detailed Reason:
Water is anomalous because its solid phase (ice) is less dense than its liquid phase. According to Le Chatelier's principle, applying pressure to an ice-water equilibrium will shift the system towards the denser phase (water) to relieve the pressure. Consequently, ice melts at a lower temperature under higher pressure, meaning the melting point decreases.

Detailed Reason:
The relationship between $K_p$ and $K_c$ is given by $K_p = K_c(RT)^{\Delta n}$, where $\Delta n$ is the change in the number of moles of gas (moles of gaseous products - moles of gaseous reactants). When the number of moles is equal, $\Delta n = 0$. Since $(RT)^0 = 1$, the equation simplifies to $K_p = K_c$.

Detailed Reason:
While the initial dissolution of NaOH in water is highly exothermic, the overall solubility curve of NaOH in water shows that its solubility increases with temperature. At higher temperatures, the kinetic energy of the solvent molecules increases, allowing them to break apart the solute crystal lattice more effectively.

Detailed Reason:
The number of components ($C$) in a system is the minimum number of independent chemical species required to define the composition of all phases in the system. An aqueous sucrose solution consists of water (solvent) and sucrose (solute), which do not react to form a new species. Thus, $C = 2$.

Detailed Reason:
According to the Gibbs Phase Rule, $F = C - P + 2$.
For a 3-component system ($C=3$), $F = 3 - P + 2 = 5 - P$.
However, the question specifies that the system is at standard temperature and pressure. Since both Temperature and Pressure are fixed (held constant), they subtract 2 degrees of freedom from the system.
The condensed phase rule becomes $F = 5 - P - 2 = 3 - P$.

Detailed Reason:
In a ternary phase diagram (an equilateral triangle plot used for 3-component systems), each of the three apices (corners) corresponds to 100% composition of one of the three components. Thus, the corners represent the pure components.

Detailed Reason:
According to the Planck-Einstein relation, the energy ($E$) of a single photon is directly proportional to its frequency ($\nu$). The equation is $E = h\nu$, where $h$ is Planck's constant. It can also be expressed as $E = hc/\lambda$.

Detailed Reason:
When $FeCl_3$ is added to a precipitate of $Fe(OH)_3$, peptization occurs. The $Fe(OH)_3$ particles preferentially adsorb the common ion, which is $Fe^{3+}$ from the $FeCl_3$ solution, onto their surface. The adsorption of these cations imparts a positive charge to the colloidal particles.

Detailed Reason:
The photochemical reaction of hydrogen and chlorine is a classic example of a secondary chain reaction. A single photon cleaves a $Cl_2$ molecule into two highly reactive Cl free radicals. These radicals initiate a propagation chain that can produce up to a million molecules of HCl before termination occurs. Thus, the quantum yield ($\Phi$) is extraordinarily high, in the range of $10^4$ to $10^6$.

Detailed Reason:
In colloid chemistry, a sol is defined as a colloidal suspension composed of very small solid particles dispersed within a continuous liquid medium (e.g., gold sol, paint, blood).

Detailed Reason:
In analytical chemistry, Error refers to the difference between the measured value and the true or accepted value. It encapsulates the inherent uncertainty present in any physical measurement due to limitations in the instrument or the observer.

Detailed Reason:
Method errors are systematic errors that are inherent to the analytical method itself. They arise from non-ideal behaviors such as incomplete reactions, co-precipitation, side reactions, or instability of reagents, which cannot be fixed merely by recalibrating the instrument.

Detailed Reason:
A monochromator separates polychromatic light into distinct wavelengths and consists of an entrance slit, a collimator, a dispersing element (like a prism or grating), and a focusing lens. The Deuterium lamp is an external UV light source that feeds into the monochromator, not a component of the monochromator itself.

Detailed Reason:
In spectrophotometry and analytical chemistry, a Blank solution is prepared to contain all the reagents and solvents present in the actual sample, omitting only the specific analyte being measured. It is used to zero the instrument and cancel out background absorbance caused by the matrix.