States of Matter PYQs Set 8 (PDF)

Set 8 of 8 · Questions 211-228 of 228

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Mere Teacher · Previous Year Questions JEE Main Chemistry · States of Matter · Set 8 (Q211-228)
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211. $Which of the following is NOT a postulate of the kinetic molecular theory of gases?$ (1) $The molecules possess a volume that is negligibly small compared to the of the container.$ (2) $The pressure and volume of a gas are inversely related$ (3) $Gases consist of discrete particles that are in random motion$ (4) $The average kinetic energy of the molecules is directly proportional to the temperature$ 212. $Correct expression for density of an ideal gas mixture of two gases 1 and 2, where m_{1} and m_{2} are masses and n_{1} and n_{2} are moles and M_{1} and M_{2} are molar masses.$ (1) $d = \frac{( m _{1} + m _{2} )}{( M _{1} + M _{2} )}$ (2) $d = \frac{( m _{1} + m _{2} )}{( n _{1} + n _{2} )} \frac{P}{R T}$ (3) $d = \frac{( n _{1} + n _{2} )}{( m _{1} + m _{2} )} \times \frac{P}{R T}$ (4) $None of these$ 213. $A gas cylinder was found unattended in a public place. The investigating team took the cylinder and collected samples from it. The density of the gas was found to be 2.380 g L^{-1} at 15ºC and 736 mm Hg pressure. Hence the molar mass of the gas is :$ (1) $83$ (2) $71$ (3) $32$ (4) $58$ 214. $Sulphur dioxide and oxygen were allowed to diffuse through a porpus partition. 20 d m^{3} of SO2 diffuses through the porous partition is 60 seconds. The volume of O2 in d m^{3} which diffuses under the similar condition in 30 seconds will be (atomic mass of sulphur = 32 u) :$ (1) $7.09$ (2) $14.1$ (3) $10.0$ (4) $28.2$ 215. $Which of the following equations does not represent Charles' law for a given mass of gas at constant pressure?$ (1) $V / T = K$ (2) $log V = log K + log T$ (3) $log K = log V + log T$ (4) $\frac{d ( ln V )}{dT} = \frac{1}{T}$ 216. $The critical volume of a gas when expressed in terms of Van der Waals constants ‘a’ and ‘b’ takes the form:$ (1) $3a$ (2) $a/ 27 b^{2}$ (3) $8a/27Rb$ (4) $3b$ 217. $Which of the following statement (s) is/are true$ (1) $The pressure of a fixed amount of an ideal gas is proportional to its temperature only$ (2) $Frequency of collisions increases in proportion to the square root of temperature$ (3) $The value of van der Waal's constant 'a' is smaller for ammonia than for nitrogen$ (4) $If a gas is expanded at constant temperature, the kinetic energy of the molecules decrease$ 218. $Real gases approach ideal behaviour at :$ (1) $high temperatures and high pressure$ (2) $high temperatures and low pressures$ (3) $low temperatures and low pressures$ (4) $critical point$ 219. $When C O_{2} under high pressure is released from a fire extinguisher, particles of solid C O_{2} are formed, despite the low sublimation temperature (- 77ºC) of C O_{2} at 1.0 atm. It is$ (1) $the gas does work pushing back the atmosphere using KE of molecules and thus lowering the temperature$ (2) $volume of the gas is decreased rapidly hence, temperature is lowered$ (3) $both (a) and (b)$ (4) $None of the above$ 220. $A gas shows positive Joule-Thomson Effect below its$ (1) $Boyle Temperature$ (2) $Critical Temperature$ (3) $Inversion Temperature$ (4) $Transition Temperature$ 221. $The root mean square velocity of S O_{2} is equal to that of oxygen at 27°C when the temperature is$ (1) $327°C$ (2) $127°C$ (3) $227°C$ (4) $600°C$ 222. $Considering air as a 4:1 mixture of nitrogen and oxygen, the mass of air in a hall with dimensions 5 m \times 5 m \times 5 m at STP is approximately$ (1) $160 g$ (2) $160 kg$ (3) $16 g$ (4) $1.60 kg.$ 223. $The product of PV is plotted against P at two temperatures T_{1} and T_{2} and the 'result is shown in figure. What is correct about T_{1} and T_{2} ?$ (1) $T_{1} > T_{2}$ (2) $T_{2} > T_{1}$ (3) $T_{1} = T_{2}$ (4) $T_{1} + T_{2} = 1$ 224. $The van der Waals equation for real gases is (P + a (\frac{n}{V})^{2}) (V - nb) = n R T . In the above equation, the terms a (\frac{n}{V})^{2} and (- nb) respectively represents the corrections for$ (1) $intermolecular attractive forces and inelastic collision$ (2) $intermolecular repulsive force and high temperatures$ (3) $intermolecular attractive forces and molecular volumes$ (4) $deviations in the temperature and pressure.$ 225. $Vander Waal’s equation for a gas is stated as, P = \frac{n R T}{V - nb} - a (\frac{n}{V})^{2} . This equation reduces to the perfect gas equation, P = \frac{n R T}{V} when,$ (1) $temperature is sufficiently high and pressure is low.$ (2) $temperature is sufficiently low and pressure is high.$ (3) $both temperature and pressure are very high.$ (4) $both temperature and pressure are very low.$ 226. $A liquid can exist only$ (1) $between triple point and critical point$ (2) $at any temperature above melting point$ (3) $between melting point and critical point$ (4) $between boiling and melting points.$ 227. $Real gases behave ideally at$ (1) $low pressure and low temperature$ (2) $high pressure and low temperature$ (3) $low pressure and high temperature$ (4) $high pressure and high temperature$ 228. $A gas will approach ideal behaviour at$ (1) $low temperature and low pressure$ (2) $low temperature and high pressure$ (3) $high temperature and low pressure$ (4) $high temperature and high pressure$