148120 If $110 \mathrm{~J}$ of heat are added to a gaseous system, whose internal energy is $40 \mathrm{~J}$, then the amount of external work done is-

148122 The $\mathrm{P}-\mathrm{V}$ diagram of a system undergoing thermodynamic transformation is shown in figure. The work done by the system in going from $A \rightarrow B \rightarrow C$ is $30 J$, and $40 J$ heat is given to the system. The change in internal energy between $A$ and $C$ is :

148124 An ideal gas is subjected to cyclic process involving four thermodynamic states, the amounts of heat $(Q)$ and work $(W)$ involved in each of these states are
$Q_{1}=6000 \mathrm{~J}, Q_{2}=-5500 \mathrm{~J} ; Q_{3}=-3000 \mathrm{~J} ;$
$\mathrm{Q}_{4}=3500 \mathrm{~J}$
$W_{1}=2500 J ; W_{2}=-1000 J ; W_{3}=-1200 J ;$
$\mathrm{W}_{4}=\mathbf{x J}$.
The ratio of the net work done by the gas to the total heat absorbed by the gas is $\eta$ ). The values of $x$ and $\eta$ respectively are

148125 Consider the following figure. Let $\Delta U_{1}$ and $\Delta U_{2}$ be the change in internal energy in processes $A$ and $B$ respectively, $\Delta Q$ be the net heat given to the system in the process $A+B$ and $\Delta W$ be the net work done by the system in the process $A+B$.

Which of the following are correct?

148120 If $110 \mathrm{~J}$ of heat are added to a gaseous system, whose internal energy is $40 \mathrm{~J}$, then the amount of external work done is-

148122 The $\mathrm{P}-\mathrm{V}$ diagram of a system undergoing thermodynamic transformation is shown in figure. The work done by the system in going from $A \rightarrow B \rightarrow C$ is $30 J$, and $40 J$ heat is given to the system. The change in internal energy between $A$ and $C$ is :

148124 An ideal gas is subjected to cyclic process involving four thermodynamic states, the amounts of heat $(Q)$ and work $(W)$ involved in each of these states are
$Q_{1}=6000 \mathrm{~J}, Q_{2}=-5500 \mathrm{~J} ; Q_{3}=-3000 \mathrm{~J} ;$
$\mathrm{Q}_{4}=3500 \mathrm{~J}$
$W_{1}=2500 J ; W_{2}=-1000 J ; W_{3}=-1200 J ;$
$\mathrm{W}_{4}=\mathbf{x J}$.
The ratio of the net work done by the gas to the total heat absorbed by the gas is $\eta$ ). The values of $x$ and $\eta$ respectively are

148125 Consider the following figure. Let $\Delta U_{1}$ and $\Delta U_{2}$ be the change in internal energy in processes $A$ and $B$ respectively, $\Delta Q$ be the net heat given to the system in the process $A+B$ and $\Delta W$ be the net work done by the system in the process $A+B$.

Which of the following are correct?

148120 If $110 \mathrm{~J}$ of heat are added to a gaseous system, whose internal energy is $40 \mathrm{~J}$, then the amount of external work done is-

148122 The $\mathrm{P}-\mathrm{V}$ diagram of a system undergoing thermodynamic transformation is shown in figure. The work done by the system in going from $A \rightarrow B \rightarrow C$ is $30 J$, and $40 J$ heat is given to the system. The change in internal energy between $A$ and $C$ is :

148124 An ideal gas is subjected to cyclic process involving four thermodynamic states, the amounts of heat $(Q)$ and work $(W)$ involved in each of these states are
$Q_{1}=6000 \mathrm{~J}, Q_{2}=-5500 \mathrm{~J} ; Q_{3}=-3000 \mathrm{~J} ;$
$\mathrm{Q}_{4}=3500 \mathrm{~J}$
$W_{1}=2500 J ; W_{2}=-1000 J ; W_{3}=-1200 J ;$
$\mathrm{W}_{4}=\mathbf{x J}$.
The ratio of the net work done by the gas to the total heat absorbed by the gas is $\eta$ ). The values of $x$ and $\eta$ respectively are

148125 Consider the following figure. Let $\Delta U_{1}$ and $\Delta U_{2}$ be the change in internal energy in processes $A$ and $B$ respectively, $\Delta Q$ be the net heat given to the system in the process $A+B$ and $\Delta W$ be the net work done by the system in the process $A+B$.

Which of the following are correct?

148120 If $110 \mathrm{~J}$ of heat are added to a gaseous system, whose internal energy is $40 \mathrm{~J}$, then the amount of external work done is-

148122 The $\mathrm{P}-\mathrm{V}$ diagram of a system undergoing thermodynamic transformation is shown in figure. The work done by the system in going from $A \rightarrow B \rightarrow C$ is $30 J$, and $40 J$ heat is given to the system. The change in internal energy between $A$ and $C$ is :

148124 An ideal gas is subjected to cyclic process involving four thermodynamic states, the amounts of heat $(Q)$ and work $(W)$ involved in each of these states are
$Q_{1}=6000 \mathrm{~J}, Q_{2}=-5500 \mathrm{~J} ; Q_{3}=-3000 \mathrm{~J} ;$
$\mathrm{Q}_{4}=3500 \mathrm{~J}$
$W_{1}=2500 J ; W_{2}=-1000 J ; W_{3}=-1200 J ;$
$\mathrm{W}_{4}=\mathbf{x J}$.
The ratio of the net work done by the gas to the total heat absorbed by the gas is $\eta$ ). The values of $x$ and $\eta$ respectively are

148125 Consider the following figure. Let $\Delta U_{1}$ and $\Delta U_{2}$ be the change in internal energy in processes $A$ and $B$ respectively, $\Delta Q$ be the net heat given to the system in the process $A+B$ and $\Delta W$ be the net work done by the system in the process $A+B$.

Which of the following are correct?