Solutions practice · Mixed difficulty

Option A is correct because for solutions showing negative deviation from Raoult's law, the mixing process leads to a decrease in entropy (ΔS < 0).

Option C (10m gram, 2V ml) is correct because the mass of gas dissolved is proportional to pressure and volume of liquid, while the volume of gas dissolved is independent of pressure.

Option D (The pressure of a 55.5 molal solution of $\delta$ is 250 bar) is correct because it is derived from Henry's Law using the given Henry's constant and molality.

Option B ($2 N$ solution) is correct because sulfuric acid ($H_2SO_4$) is a diprotic acid, meaning it has two replaceable hydrogen ions, so its normality is twice its molarity.

Option A (59.99) is correct because it is calculated using the isotonicity condition and the molar masses of the substances.

Option A ($\mathrm{N}{\mathrm{H}_3} > C{\mathrm{O}_2} > {\mathrm{O}_2} > {\mathrm{H}_2}$) is correct because ammonia is highly soluble due to hydrogen bonding, followed by CO2 which reacts with water, then oxygen, and lastly hydrogen.

Option D is correct because mechanism B is consistent with the rate law, as the slow step involves one molecule of H2 and one molecule of ICl.

Option C is correct because water in a beaker cannot boil in a boiling water bath as it needs latent heat, which the water bath cannot provide once both reach 100°C.

Option D (none of these) is correct because all the statements about Raoult's law, osmotic pressure, and the order of osmotic pressure are true.

Option C ($100.25^{\circ} \mathrm{C}$) is correct because the boiling point elevation depends on the number of moles of solute, and urea and glucose have the same effect in this case.

Option B (0.82) is correct because it involves using Raoult's law and Dalton's law to find the mole fraction of A in the vapor phase.

The correct answer is Assertion is Wrong but Reason is correct. The formation of a semipermeable membrane is due to diffusion, not osmosis, and the reaction between Cu2+ and Fe(CN)64- forms an insoluble compound.

Option A (1.0342) is correct because it is calculated using the relationship between molality, molarity, density, and molar mass of the solute.

Option D (Distribution coefficient for ${\mathrm{10^\circ }}$ rise in the temperature) is correct because the temperature coefficient describes the change in the distribution coefficient for a 10-degree Celsius temperature increase.

Option D is correct because both the assertion and the reason are false. Elevation in boiling point and depression in freezing point depend on the molality of the solution and the cryoscopic/ebullioscopic constants, not the melting point of the solute. The assertion is false because equal molal concentrations will not necessarily result in equal changes.

Option A (147 torr) is correct because it is calculated using Raoult's law, considering the mole fractions and vapor pressures of the two liquids.

Option A (60 atm) is correct because the osmotic pressure is calculated using the relative lowering of vapor pressure and the ideal gas law.

Option D ($5.30 \times 10^6$) is correct because it is the molar mass calculated using the osmotic pressure formula and the given slope.

Option B (0.1 M $\mathrm{Na}_3 \mathrm{PO}_4$ and 0.1 M $\mathrm{K}_2 \mathrm{SO}_4$) is correct because their van't Hoff factors and concentrations result in different osmotic pressures.

Option D is correct because for an ideal solution, mixing is spontaneous, so ΔG must be negative.

The correct answer is A because benzene has a higher vapor pressure than toluene, so the vapor will be richer in benzene.

Option C (96 mL) is correct because the volume of the mixture is calculated by dividing the total mass by the density of the mixture.

Option B is correct because if the dimer separates out, the effective van't Hoff factor decreases, leading to an increase in the observed molar mass of the solute.

Option D is correct. $\mathrm{AX}_2$ is fully ionized while $\mathrm{AY}_2$ is completely unionized, as determined by the van't Hoff factor.

Option B ($1.0 \text{{ mole of }} \mathrm{AgCl}$) is correct because the complex is $\left[\mathrm{Cr}\left(\mathrm{H}_2 \mathrm{O}\right)_5 \mathrm{Cl}\right] \mathrm{Cl}_2 \cdot \mathrm{H}_2 \mathrm{O}$, and only the chloride ions outside the coordination sphere react with $AgNO_3$.

Option C (3 g) is correct because the mass of urea is calculated using the formula for depression in freezing point, considering the molality and cryoscopic constant.

The correct answer is A (33.3) because at equilibrium, the water will transfer from the less concentrated solution to the more concentrated solution until both solutions have the same vapor pressure.

Option A (${C}_5 {H}_{12}+$ alcohol) is immiscible because pentane is a nonpolar solvent, while alcohols, especially short-chain alcohols, have some polarity due to the -OH group.

Option A (38.71) is correct because it involves calculating the amount of water remaining in the solution at -9.3°C using the freezing point depression formula and then subtracting that from the initial amount of water to find the mass of ice separated.

Option A is correct because freezing, gas-to-solid conversion, and adsorption all result in a decrease in entropy due to increased order.