States of matter practice · Easy

Option A ($\mathrm{H}_2$ and $\mathrm{Cl}_2$ mixture) is correct because hydrogen and chlorine react to form HCl under normal conditions, violating the assumption of non-reactivity in Dalton's law.

Option A (2050) is correct because the final pressure is the sum of the partial pressure of benzene and the compressed air pressure.

Option A (13.65 mL) is correct because it is calculated using Graham's law of diffusion, relating diffusion rate to molar mass.

Option A (If both A and R are correct and R is the correct explanation of A) is correct because the kinetic energy increase at higher temperatures allows more liquid molecules to overcome intermolecular forces and enter the vapor phase, thus increasing vapor pressure.

Option C (256) is correct because the molecular weight is calculated using the relative density with respect to $O_2$.

Option C (8 atm) is correct because it is the pressure calculated using Boyle's Law, which states that for a fixed amount of gas at constant temperature, the pressure and volume are inversely proportional.

Option B (1) is correct because the compressibility factor (Z) for an ideal gas is always equal to 1, indicating ideal behavior.

Option C (London forces) is correct because H2 is a nonpolar molecule, and the only intermolecular forces present are London dispersion forces.

Option A ($C{l_2}$) is correct because the van der Waals constant 'b' is directly proportional to the size/volume of the gas molecule.

Option B ($N{H_3}$) is correct because it has the lowest molecular weight among the given gases, leading to the highest rate of diffusion according to Graham's law.

Option B (72) is correct because the molecular weight is calculated using Graham's law of diffusion, relating the rates of diffusion to the square root of their molecular weights.

Option C ($9: 4$) is correct because the ratio of densities is the inverse square of the ratio of diffusion rates.

Option A (Assertion is correct, reason is correct; reason is a correct explanation for assertion) is correct because gases have high kinetic energy, which prevents them from settling at the bottom of a container.

Option A ($2\mathrm{ }\,atm$) is correct because the pressure is calculated using the ideal gas law, $pV = nRT$.

Option C ($\mathrm{N}{\mathrm{m}^{ - \mathrm{1}}}$) is correct because surface tension is defined as force per unit length, hence the unit is Newton per meter.

Option C (N2O, CO2) is correct because gases with equal molecular masses have equal rates of diffusion, and N2O and CO2 both have a molecular mass of 44.

Option A (3.5 cm/s) is correct because the average speed is calculated by summing the speeds and dividing by the number of particles.

Option C (Isoenthalpic process) is correct because Joule-Thomson expansion occurs at constant enthalpy.

Option B (Most probable speed) is correct because the most probable speed is the speed possessed by the majority of gaseous molecules.

Option B (PM/RT) is correct because the density of a gas can be derived from the ideal gas law, PV = nRT, where n = mass/molecular weight.

Option B is correct because a gas can be liquefied at a temperature below its critical temperature (${T_c}$) and a pressure above its critical pressure (${P_c}$).

Option D (A, B, C and D) is correct because the van der Waals constant 'a' increases with the size and complexity of the molecule, reflecting stronger intermolecular forces.

Option C ($PV = RT + Pb$) is correct because at high pressure, the volume 'V' is small, so 'b' is not negligible compared to 'V', and the term $\frac{a}{V^2}$ becomes negligible.

Option B (Manometer) is correct because a manometer is a device used to measure gaseous pressure, often based on the principles of Boyle's law.

Option A (1) is correct because the compressibility factor (Z) for an ideal gas is always 1, as the gas follows the ideal gas law (pV = nRT).

Option B (The pressure decreases) is correct because intermolecular attractions reduce the force with which gas molecules collide with the container walls.