A sample of gas with $\gamma=1.5$ is taken through an adiabatic process in which the volume is compressed from $1200\, {cm}^{3}$ to $300\, {cm}^{3}$. If the initial pressure is $200\, {kPa}$. The absolute value of the workdone by the gas in the process $= \,..... J.$
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One mole of an ideal gas $(\gamma = 1.4)$ is adiabatically compressed so that its temperature rises from $27\,^oC$ to $35\,^oC$ . The change in the internal energy of the gas is .... $J$. (given $R = 8.3\,J/mole-K$ )
$Assertion :$ In adiabatic compression, the internal energy and temperature of the system get decreased.
$Reason :$ The adiabatic compression is a slow process.
When a system is taken from state $i$ to state $f$ along the path $iaf$, it is found that $Q=50$ $cal$ and $W=20$ $cal$ Along the path $ibf\ Q = 36\ cal. \ W$ along the path $ibf$ is ....... $ cal$
An electric appliance supplies $6000\, {J} / {min}$ heat to the system. If the system delivers a power of $90\, {W}$. How long (in $sec$) it would take to increase the internal energy by $2.5 \times 10^{3}\, {J}$ ?
A certain amount of gas of volume $V$ at $27^{o}\,C$ temperature and pressure $2 \times 10^{7} \;Nm ^{-2}$ expands isothermally until its volume gets doubled. Later it expands adiabatically until its volume gets redoubled. The final pressure of the gas will be (Use $\gamma=1.5$ )