The partition coefficient (logP) is a measure of the equilibrium distribution of a solute between two immiscible liquids, usually water and 1-octanol.

When phenol is behaving as the solute with water and 1-octanaol as the solvents its log P value is 30.2. What does this value say about the relative solubility of a phenol molecule in each solvent liquids? Explain your answer with reference to theory covered in the course regarding miscibility and intermolecular forces. [4 marks]

 Note: in the formula above the equilibrium concentration of a solute S in solvent x is denoted as [S]_x ( e.g. [S]_aq denotes what concentration of a solute is dissolved in the water layer)

OUT OF SYLLABUS of CHEM1832

Calculate the value of K_p for the reaction below given equilibrium concentrations of [NO] = 0.0080 M, [O₂] = 0.014 M and [NO₂] = 0.012 M at 269 K:

2NO(g)  +  O₂(g)  ⇌  2NO₂(g)

Your answer must be given to the correct number of significant figures to receive full marks.

The equilibrium constant in terms of concentrations (K_c) for this reaction:

N₂(g)  + 3H₂(g) ⇌ 2NH₃(g)

equals 4.4 × 10^-3. If, at equilibrium, the concentration of H₂ = 4.9 mol/L and the concentration of NH₃ = 2.4 mol/L, what is the equilibrium concentration of N₂(g)?

Using the information provided in the table below, which of the atoms/ions would you expect to have the smallest atomic radius?

Given the following acids and bases and their corresponding equilibrium constants, which two species you would mix in water in equal quantities to produce a neutral solution?

Which of the the following statements are TRUE?

Tick only the true statements. Ticking false statements will result in reduced marks for this question. 

The reaction, 2MO(s) + CO₂(g) → M₂O₃(s) + CO(g) where M is a metallic element, is spontaneous at high temperatures but non-spontaneous at low temperatures.

If we assume that Δ_rH° and Δ_rS° are constant over a wide temperature range we can deduce that: