The reaction, H_(2(g)) + 1/2O_(2(g)) to H_2O_((l)), is spontaneous. The DeltaS^(@) = - 163.1 J mol^(-1) K^(-1). The absolute entropies of H_(2(g)) and O_(2(g)) are 130.6 JK^(-1)mol^(-1) and 205 JK^(-1) mol^(-1) respectively. Calculate the absolute entropy of water.

The reaction, H_(2(g)) + 1/2O_(2(g)) to H_2O_((l)), is spontaneous. Th

1.	The reaction, H_(2(g)) + 1/2O_(2(g)) to H_2O_((l)), is spontaneous. The DeltaS^(@) = - 163.1 J mol^(-1) K^(-1). The absolute entropies of H_(2(g)) and O_(2(g)) are 130.6 JK^(-1)mol^(-1) and 205 JK^(-1) mol^(-1) respectively. Calculate the absolute entropy of water.
Answer» Solution :CHANGE in STANDARD entropy, `DeltaS^(@) = S_(H_2O_(l))^(@) - [S_(H_2)^(@) + 1/2S_(O_2)^(@)]` Absolute entropy of WATER = `69.9 JK-mol^(-1).`