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A gas can be taken from $A$ to $B$ via two different processes $ACB$ and $ADB$. When path $ACB$ is used $60\, J$ of heat flows into the system and $30\, J$ of work is done by the system. If path $ADB$ is used work down by the system is $10\, J$. the heat flow into the system in path $ADB$ is ..... $J$
$40$
$80$
$100$
$20$
Solution
As temperature at point $A$ and $C$ is same.
$\therefore$ Internal energy change will be same.
$\mathrm{Q}-\mathrm{W}=\mathrm{Q}^{\prime}-\mathrm{W}^{\prime}$
$60-30=Q^{\prime}-10$
$Q^{\prime}=40 \mathrm{J}$
Similar Questions
$List I$ describes thermodynamic processes in four different systems. $List II$ gives the magnitudes (either exactly or as a close approximation) of possible changes in the internal energy of the system due to the process.
| $List-I$ | $List-II$ |
| ($I$) $10^{-3} kg$ of water at $100^{\circ} C$ is converted to steam at the same temperature, at a pressure of $10^5 Pa$. The volume of the system changes from $10^{-6} m ^3$ to $10^{-3} m ^3$ in the process. Latent heat of water $=2250 kJ / kg$. | ($P$) $2 kJ$ |
| ($II$) $0.2$ moles of a rigid diatomic ideal gas with volume $V$ at temperature $500 K$ undergoes an isobaric expansion to volume $3 V$. Assume $R=8.0 Jmol ^1 K^{-1}$. | ($Q$) $7 kJ$ |
| ($III$) On mole of a monatomic ideal gas is compressed adiabatically from volume $V=\frac{1}{3} m^3$ and pressure $2 kPa$ to volume $\frac{v}{8}$ | ($R$) $4 kJ$ |
| ($IV$) Three moles of a diatomic ideal gas whose molecules can vibrate, is given $9 kJ$ of heat and undergoes isobaric expansion. | ($S$) $5 kJ$ |
| ($T$) $3 kJ$ |
Which one of the following options is correct?
