The increase in entropy in $J K^{-1}$ of a substance when it absorbs $1 \ kJ$ of heat energy at $3 \ K$ is

For an isolated system,$\Delta U = 0,$ what will be $\Delta S?$

The entropy change involved in the conversion of $1 \, \text{mole}$ of liquid water at $373 \, K$ to vapour at the same temperature will be $[\Delta H_{vap} = 2.257 \, kJ/g]$. (in $, kJ/K$)

For which of the following reactions will $\Delta S$ be maximum?

The entropy change in the isothermal reversible expansion of $2$ moles of an ideal gas from $10 \ L$ to $100 \ L$ at $300 \ K$ is: (in $JK^{-1}$)

Among the following processes,for which process is the change in entropy $(\Delta S)$ negative?