Physics MCQs for NEET — Practice Questions with Answers

According to the equilibrium theorem, the molar heat capacities should be independent of temperature How ever, variations in $C_v$ and $C_p$ are observed as the temperature changes. At very high temperatures, vibrations are also inportant and that affects the values of $C_v$ and $C_p$ for diatomic and poly atomic gases. Here in the question according to given information (D) may be correct answer.

At constant pressure, the gas does work in expanding against the external pressure. This work requires additional energy, which is why the specific heat at constant pressure (C_p) is greater than the specific heat at constant volume (C_v).

$ \gamma _{mix} = { { 1\gamma_1 \over \gamma_1 -1 } + { 2\gamma_2 \over \gamma_2 -1 } \over { 1 \over \gamma_1 - 1 } + {2 \over \gamma_2 -1 } } = { { 1 \times 5/3 \over ( 5/3 - 1 ) } + { 1 \times 7/5 \over 7/5 - 1 } \over {1 \over (5/3 -1)} + {1 \over ( 7/5 -1 ) } }= { 3 \over 2} = 1.5 $

$ \gamma = 1 + { 2 \over f } \Rightarrow \gamma -1 = { 2 \over f } \Rightarrow { f \over 2} = { 1 \over \gamma -1 } $ $ \therefore f = { 2 \over \gamma - 1 } $

molar specific heat at constant pressure, $C_p = 7 \over 2 R $ Since $ C_p - C_v = R \Rightarrow C_v = C_p - R = { 7 \over 2} R -R = { 5 \over 2 } R $

$ \gamma = 7/5 $ for a diatomic gas

The time of collision of molecules being of the order of \( 10^{-8} \text{ s} \\) is an experimental fact, and it is true. This time is very small compared to the time between two successive collisions. Therefore, both the assertion and the reason are true, and the reason correctly explains the assertion.

The mean free path (\

$ F = ma = m \left( \nu^2 - u^2 \over 2S \right) $