One gm mol of a diatomic gas $(\gamma = 1.4)$ is compressed adiabatically so that its temperature rises from ${27^o}C$ to ${127^o}C$. The work done will be
Experience the future of education. Simply download our apps or reach out to us for more information. Let's shape the future of learning together!No signup needed.*
In a Carnot engine, when ${T_2} = {0^o}C$ and ${T_1} = {200^o}C,$ its efficiency is ${\eta _1}$ and when ${T_1} = 0{\,^o}C$ and ${T_2} = - 200{\,^o}C$, Its efficiency is ${\eta _2}$, then what is ${\eta _1}/{\eta _2}$
An ideal gas is made to undergo the cyclic process shown in the figure below. Let $\Delta W$ depict the work done, $\Delta U$ be the change in internal energy of the gas and $Q$ be the heat added to the gas. Sign of each of these three quantities for the whole cycle will be (0 refers to no change)
One mole of an ideal gas at temperature $T_1$ expends according to the law $\frac{P}{{{V^2}}} =a$ (constant). The work done by the gas till temperature of gas becomes $T_2 $ is
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 $R = 8.3 \,J/mole/K$)
$Assertion :$ The Carnot cycle is useful in understanding the performance of heat engines.
$Reason :$ The Carnot cycle provides a way of determining the maximum possible efficiency achievable with reservoirs of given temperatures.