Physics MCQs for NEET — Practice Questions with Answers

The NCERT text states: 'Bohr model, though offering a satisfactory model for explaining the spectra of the hydrogen atom, could not explain the spectra of multi-electron atoms.' The inability to extend to multi-electron atoms suggests a failure to account for complex electron-electron interactions, which are absent in single-electron systems like hydrogen.

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: $P = P_1 + P_2 + \dots$).