States of matter practice · Medium

Option B (Avogadro’s hypothesis) is correct because Avogadro's hypothesis states that equal volumes of all gases, at the same temperature and pressure, have the same number of molecules, leading to the 22.4 L molar volume at NTP.

Option A (Decreases) is correct because as pressure increases, the molecules are closer together, leading to more frequent collisions and a shorter mean free path.

Option A ($623.25\mathrm{ }J$) is correct because it is the change in kinetic energy calculated using the formula KE = (3/2)RT.

Option B (Boyle temperature) is correct because Boyle temperature is the temperature at which a real gas obeys the ideal gas law over a wide range of pressures.

Option A ($\frac{1}{4}$) is correct because it is calculated using Graham's law of diffusion after 5 diffusion steps.

Option A (1.0043) is correct because the relative rates of diffusion are inversely proportional to the square root of their molar masses.

Option C (The parameter $a$ accounts for intermolecular interaction’s present in the molecule) is correct because the 'a' parameter in the van der Waals equation accounts for the attractive intermolecular forces between gas molecules.

Option D (28.3) is correct because it is the mass percentage of Ne calculated from the total kinetic energy and total mass of the mixture.

Option D (Van der Waals’ forces) is correct because non-polar molecules interact through weak, temporary dipoles induced by electron fluctuations.

Option A (400) is correct because the critical temperature can be calculated using the critical compressibility factor and the ideal gas law.

Option C (Mole fraction) is correct because, according to Dalton's law of partial pressures, the ratio of the partial pressure of a gas to the total pressure is equal to its mole fraction.

Option A (6) is correct because using the ideal gas law in terms of density, the ratio of pressures can be found to be 6.

The correct answer is B ($KE$ of the molecules becomes zero and the molecular motion also becomes zero) because at absolute zero (0 Kelvin), all molecular motion ceases, and the kinetic energy becomes zero.

Option C (0.9213) is correct because the average speed of gas molecules is approximately 0.9213 times their root-mean-square (RMS) speed, based on the kinetic theory of gases.

Option B is correct because both statements are correct, but the second statement (pressure difference) does not explain the first statement (boiling point difference); the boiling point difference is a direct consequence of the pressure difference.

Option D (26.94 cc) is correct because it involves converting the given conditions to STP, then using stoichiometry to find the volume of oxygen required for complete combustion of methane.

Option B ($6.17 \times {10^{ - 21}}\mathrm{J}$) is correct because it is the average kinetic energy calculated using the formula $\frac{3}{2}kT$ with the correct Boltzmann constant and temperature.

Option C ($\frac{{2{P_{\mathrm{total}}}}}{3}$) is correct because the partial pressure of a gas is the product of the total pressure and its mole fraction.

The correct answer is B ($\sqrt{6} \mathrm{~V}_0$) because the new RMS velocity can be found by relating it to the initial most probable velocity, considering the dissociation of hydrogen molecules into atoms.

Option A ($2.5$) is correct because the relative density is calculated using the ideal gas law and the definition of relative density, resulting in approximately 2.5.

Option C ($T_i=2T_b$) is correct because the inversion temperature ($T_i$) is twice the Boyle's temperature ($T_b$).

Option B (2) is correct because the ratio of diffusion rates is inversely proportional to the square root of the molar masses, resulting in a ratio of 2.

Option B ($40\mathrm{ }L$) is correct because the change in volume is calculated using Charles's Law, resulting in a 40 L increase.

Option B ($p\mathrm{S}{\mathrm{O}_2} > p\mathrm{C}{\mathrm{H}_4} > p{\mathrm{H}_2}$) is correct because the rate of diffusion is inversely proportional to the square root of the molecular mass. Therefore, the gas with the highest molecular mass will have the lowest diffusion rate and hence the highest partial pressure after 3 hours.

Option B (40) is correct because using Charles's Law, the volume increases proportionally with temperature, and the percentage of air escaped is calculated based on the change in volume.

The correct answer is A (Due to the presence of ${\mathrm{H}^ + }$ and ${\mathrm{OH}^ - }$ions in water) because the high boiling point of water is primarily due to hydrogen bonding between water molecules.

Option B (5 atm) is correct because the partial pressure of a gas in a mixture is equal to its mole fraction multiplied by the total pressure. Since the mole fraction of Helium is 0.5, its partial pressure is 5 atm.

Option B (40) is correct because using Charles's Law, the volume increases proportionally with temperature, and the percentage of air escaped is calculated based on the change in volume.

Option D (Remains unchanged) is correct because at constant temperature, the vapor pressure of a saturated vapor remains constant regardless of volume changes.

Option A (Both Statement I and Statement II are correct and Statement II is the correct explanation of Statement I) is correct because viscosity is directly related to intermolecular forces, with stronger forces leading to higher viscosity.