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.*
Starting with the same initial conditions, an ideal gas expands from volume $V_{1}$ to $V_{2}$ in three different ways. The work done by the gas is $W_{1}$ if the process is purely isothermal. $W _{2}$. if the process is purely adiabatic and $W _{3}$ if the process is purely isobaric. Then, choose the coned option
Match the thermodynamic processes taking place in a system with the correct conditions. In the table: $\Delta Q$ is the heat supplied, $\Delta W$ is the work done and $\Delta U$ is change in internal energy of the system
Process
Condition
$(I)$ Adiabatic
$(A)\; \Delta W =0$
$(II)$ Isothermal
$(B)\; \Delta Q=0$
$(III)$ Isochoric
$(C)\; \Delta U \neq 0, \Delta W \neq 0 \Delta Q \neq 0$
Four curves $A, B, C$ and $D$ are drawn in the adjoining figure for a given amount of gas. The curves which represent adiabatic and isothermal changes are
A thermodynamic process is the pressure and volumes corresponding to some points in the figure are, $P_A = 3 \times 10^4 Pa$, $V_A = 2 \times 10^{-3}\, m^3$, $P_B = 8 \times 10^4 Pa$, $V_D = 5 \times 10^{-3}\,m^3$. In process $AB, 600\, J$ of heat and in process $BC, 200\, J$ of heat is added to the system. The change in the internal energy in process $AC$ would be .... $J$
When an ideal gas $(\gamma = 5/3$) is heated under constant pressure, then what percentage of given heat energy will be utilised in doing external work