In a given process,for an ideal gas,$\Delta W = 0$ and $\Delta Q < 0$. Then,for the gas,

Which of the following is not a thermodynamic state function?

In how many ways can the internal energy of a system be changed?

$1.00 \ kg$ of liquid water at $100^{\circ} C$ undergoes a phase change into steam at $100^{\circ} C$ at $1.0 \ atm$ (take it to be $1.00 \times 10^5 \ Pa$). The initial volume of the liquid water was $1.00 \times 10^{-3} \ m^3$ which is changed to $2.001 \ m^3$ of steam. Find the change in the internal energy of the system. [Use heat of vaporization $\simeq 2000 \ kJ \ kg^{-1}$] (in $kJ$)

If heat is added at constant volume,$6300 \ J$ of heat are required to raise the temperature of an ideal gas by $150 \ K$. If instead,heat is added at constant pressure,$8800 \ J$ are required for the same temperature change. When the temperature of the gas changes by $300 \ K$,the internal energy of the gas changes by ..... $J$.

$A$ diatomic gas has an initial internal energy of $80 cal$. $A$ work of $18 cal$ is done on the gas and the gas releases heat energy of $42 J$. The final internal energy of the gas is