ThermochemistryMedium
Question
For the equilibrium H2O(l) ⇋ H2O(g) at 1atm and 298 K :
Options
A.standard free every change is equal to zero (ᐃGo = 0)
B.Free energy change is less than zero (ᐃGo < 0)
C.standard free energy change is less than zero (ᐃGo < 0)
D.standard free energy change is greater than zero (ᐃGo > 0)
Solution
The process, H2O(l) ⇋ H2O(g), is an endothermic process, (ᐃH = + ve).
Hence this process is spontsneous at all temperature above 0oC (TᐃS > ᐃH, so ᐃG is negative, ᐃG = ᐃH - TᐃS). Thus free energy change (ᐃG) will be less than zero (negative) at atm and 298 K.
Hence this process is spontsneous at all temperature above 0oC (TᐃS > ᐃH, so ᐃG is negative, ᐃG = ᐃH - TᐃS). Thus free energy change (ᐃG) will be less than zero (negative) at atm and 298 K.
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