The enthalpy of vaporization of water is $186.5 \, kJ \, mol^{-1}$. What is the entropy of vaporization in $kJ \, K^{-1} \, mol^{-1}$?

For a reversible spontaneous change,$\Delta S$ is:

What is the change in entropy of the surroundings for the reaction, $H_2(g) + 1/2 O_2(g) \rightarrow H_2O(l)$ at $298 \text{ K}$, if the standard enthalpy of formation of water is $-286 \text{ kJ mol}^{-1}$?

What happens to the total entropy of the system and surroundings during a spontaneous irreversible process?

Which of the following is the least $random$ state of water?

The total amount of energy in the universe is fixed,but