States of matter practice · Mixed difficulty

Option C (Inversion temperature) is correct because the Joule-Thomson coefficient is zero at the inversion temperature, indicating no temperature change during throttling.

Option A (1) is correct because the compressibility factor (Z) for an ideal gas is always equal to 1, as there are no intermolecular forces.

Option C (Charles’ law) is correct because hot air balloons rise due to the decrease in air density as the air is heated, which is a direct application of Charles's Law.

Option B (Kinetic energy of ${\mathrm{O}_2} < \mathrm{kinetic\;energy\;of}\,\;\mathrm{S}{\mathrm{O}_2}$) is correct because kinetic energy is directly proportional to temperature.

Option A (Will remain unchanged in $A$ and $B$) is correct because after removing the wall, each gas expands to fill the entire volume, but the partial pressure of each gas remains the same.

Option D (Ion – dipole interaction) is correct because hydration involves the attraction between ions and the polar water molecules, which is an ion-dipole interaction.

Option A (NH3) is correct because NH3 exhibits stronger intermolecular forces (hydrogen bonding) compared to the other options, leading to a higher 'a' value.

Option D (All of the above) is correct because van der Waals forces are directly related to the size, number of electrons, and molecular weight of the molecule.

Option C is correct. The average speed of gas molecules is given by the formula \sqrt{{$\frac{{8RT}}{{π M}}$}}.

Option A (Boyle’s law) is correct because air density increases with pressure at sea level, which is a direct application of Boyle's Law.

Option B (6.72) is correct because it uses the ideal gas law to find the new volume when the pressure is reduced to one-third while keeping the temperature constant.

Option B ($227^\circ C$) is correct because the most probable speed is proportional to the square root of the temperature divided by the molar mass.

Option C (The two gases contain the same number of molecules) is correct because Avogadro's Law states that equal volumes of gases at the same temperature and pressure contain the same number of molecules.

Option D ($\frac{3}{8}$) is correct because the value of the compression factor, Z, for critical constants is 3/8.

Option B (HF) is correct because HF forms strong hydrogen bonds, and these bonds can persist even in the vapor state due to the high electronegativity of fluorine and the small size of the HF molecule.

Option A ($9:10$) is correct because the rate of diffusion is inversely proportional to the square root of the molecular weight.

Option C (Experimental observations) is correct because Gay-Lussac's law is based on empirical evidence and observations of gas behavior.

Option A ($HCl$ and $Ne$) is correct because HCl is a polar molecule (dipole) and Ne is a nonpolar atom, leading to a dipole-induced dipole interaction.

Option A (Nearer to the HCl end) is correct because HCl has a higher molar mass and thus diffuses slower than NH3.

Option B (N2) is correct because nitrogen gas is relatively insoluble in water, allowing it to be collected over water without significant dissolution.

Option B (0.568 L) is correct because it calculates the volume of CO2 produced at STP using stoichiometry and the ideal gas law.

Option B ($273\,\,^\circ C\,\,and\,\,2{\mkern 1mu} {\mkern 1mu} atm$) is correct because increasing both temperature and pressure proportionally can keep the volume constant according to the ideal gas law.

Option B is correct because both statements are true, but Statement II doesn't explain Statement I.

Option A (${10^6}\mathrm{dyne}\,\mathrm{c}{\mathrm{m}^{ - 2}}$) is correct because one atmosphere is approximately equal to 1.013 × 10⁵ Pascals, which converts to 10⁶ dyne/cm².

Option A (0.65) is correct because the compressibility factor is calculated using Z = PV/nRT.

Option C is correct because gases have the largest intermolecular spaces and are therefore the most easily compressed.

Option C is correct because the van der Waals constant 'b' represents the volume excluded by the gas molecules themselves, which is related to the volume occupied by the molecules.

Option B (4.58 mm and
$0.0098\,\,^\circ \mathrm{C}$) is correct because it represents the specific pressure and temperature at which ice, water, and vapor coexist in equilibrium.

The question is asking for the height the liquid will rise, but the options are given in N/m. This is likely a typo and the question intended to ask for the height in meters or millimeters. Assuming the question asks for the height the liquid will rise in mm, none of the options are correct. However, if we calculate the value and multiply by density and g, we can get the pressure difference, which will have units of N/m². Dividing by 1000, we can get a value close to one of the options. However, the question is flawed.

Option B (Water boils at higher temperature inside the pressure cooker) is correct because the increased pressure raises the boiling point of water, leading to faster cooking.