In a closed insulated container,a liquid is stirred with a paddle to increase its temperature. Which of the following is correct?

Assuming that water vapour is an ideal gas,the internal energy change $(\Delta U)$ when $1\, mol$ of water is vaporised at $1\, bar$ pressure and $100\, ^{\circ}C$,(given: molar enthalpy of vaporisation of water at $1\, bar$ and $373\, K = 41\, kJ\, mol^{-1}$ and $R = 8.3\, J\, mol^{-1}\, K^{-1}$) will be .............. $kJ\, mol^{-1}$

In a closed insulated container,a liquid is stirred with a paddle to increase its temperature. In this process,which of the following is true?

What is the change in internal energy when a system releases $8 \ kJ$ of heat and performs $660 \ J$ of work on the surroundings (in $J$)?

Choose the correct option for the free expansion of an ideal gas under adiabatic conditions from the following:

Joule-Thomson expansion is: