In a reversible expansion,one mole of gas is expanded isothermally at $200 \ K$ till its volume increases $10$ times. Calculate $\Delta S_{total}$ at equilibrium (in $J \ K^{-1}$)?

The standard entropies of $CO_{2(g)}$,$C_{(s)}$ and $O_{2(g)}$ are $213.5$,$5.690$ and $205 \ J \ K^{-1} \ mol^{-1}$ respectively. The standard entropy of formation of $CO_{2(g)}$ is ...... $J \ K^{-1} \ mol^{-1}$.

According to the second law of thermodynamics,which of the following is true for a spontaneous process?

Entropy is maximum in case of

The entropy change involved in the isothermal reversible expansion of $2 \, \text{mole}$ of an ideal gas from a volume of $10 \, dm^3$ to a volume of $100 \, dm^3$ at $27 \, ^oC$ is : .............. $J \, K^{-1}$

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