NEET Practice Questions (MCQs) with Answers & Solutions

The NCERT text defines adolescence as 'a very vulnerable phase of mental and psychological development of an individual,' characterized by 'Curiosity, need for adventure and excitement, and experimentation,' which motivate youngsters towards drug and alcohol use.

According to the KINETIC_THEORY chapter, 'A gas that satisfies Eq. (12.3) [PV = $\mu$RT] exactly at all pressures and temperatures is defined to be an ideal gas.'

The KINETIC_THEORY chapter states, 'Notice that all curves approach the ideal gas behaviour for low pressures and high temperatures.' This is because molecules are far apart and molecular interactions are negligible under these conditions.

The KINETIC_THEORY chapter mentions, 'If we fix $\mu$ and T in Eq. (12.3) [PV = $\mu$RT], we get PV = constant... i.e., keeping temperature constant, pressure of a given mass of gas varies inversely with volume. This is the famous Boyle’s law.'

The KINETIC_THEORY chapter states, 'if you fix P, Eq. (12.1) shows that V $\propto$ T i.e., for a fixed pressure, the volume of a gas is proportional to its absolute temperature T (Charles’ law).'

The THERMAL_PROPERTIES_OF_MATTER chapter states, 'temperature on these scales are related by T = $t_C$ + 273.15 (10.3)'. Lord Kelvin established this scale where 0 K is -273.15 °C.

The THERMODYNAMICS_Physics chapter states, 'An Equation of State (like the ideal gas equation PV = µRT) is a relation connecting different state variables.' Here, R is the universal gas constant, and $\mu$ is the number of moles.

The KINETIC_THEORY chapter states, 'i.e., the average kinetic energy of a molecule is proportional to the absolute temperature of the gas; it is independent of pressure, volume or the nature of the ideal gas.' (Eq. 12.19, $E/N = 1/2 m\bar{v^2} = 3/2 k_B T$).

The KINETIC_THEORY chapter states, 'Eq. (12.18) tells us that internal energy of an ideal gas depends only on temperature, not on pressure or volume.'

The KINETIC_THEORY chapter states, 'Thus, the total pressure of a mixture of ideal gases is the sum of partial pressures.' (Eq. 12.9: $P = P_1 + P_2 + \dots$).