A diatomic gas of molecules weight $30\,\, gm/mole$ is filled in a container at $27\,^oC$. It is moving at a velocity $100\,\, m/s$. If it is suddenly stopped, the rise in temperature of gas is :
Here $\gamma$ is 1.4 for a diatomic gas, so $150=\frac{R}{1.4-1} \times \Delta T$
$\Delta T=\frac{60}{R}$
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$105$ calories of heat is required to raise the temperature of $3$ moles of an ideal gas at constant pressure from $30^{\circ} C$ to $35^{\circ} C$. The amount of heat required in calories to raise the temperature of the gas through the range $\left(60^{\circ} C\right.$ to $\left.65^{\circ} C \right)$ at constant volume is ........ $cal$ $\left(\gamma=\frac{C_p}{C_v}=1.4\right)$
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$Reason :$ Mean free path varies inversely as pressure of the gas.
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