$\Rightarrow$ ${M_{Gas}} = 4$ That is, the gas is $He$.
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$Assertion$: The total translational kinetic energy of all the molecules of a given mass of an ideal gas is $1.5\, times$ the product of its pressure and its volume.
$Reason$ : The molecules of a gas collide with each other and the velocities of the molecules change due to the collision.
One mole of an ideal gas requires $207\, J$ heat to raise the temperature by $10 \,K$ when heated at constant pressure. If the same gas is heated at constant volume to raise the temperature by the same $10\, K,$ the heat required is ...... $J$
(Given the gas constant $R = 8.3J/mol{\rm{ - }}K$)
Two ideal polyatomic gases at temperatures $T _{1}$ and $T _{2}$ are mixed so that there is no loss of energy. If $F _{1}$ and $F _{2}, m _{1}$ and $m _{2}, n _{1}$ and $n _{2}$ be the degrees of freedom, masses, number of molecules of the first and second gas respectively, the temperature of mixture of these two gases is