ThermochemistryHard
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.
Create a free account to view solution
View Solution FreeMore Thermochemistry Questions
Which of the following statement(s) is/are true?...The standard molar enthalpy of formation of CO2 is equal to...Under identical conditions, how many millilitres of 1 M-KOH and 2 M-H2SO4 solutions are required to produce a resulting ...The data below refers to gas phase reaction at constant pressure at 25°C.CH3–CH3 → CH3–CH2 + H: ΔH1 = +420 kJ mol–1CH3–C...A solution was prepared by dissolving 7.45 g of KCl in 200 g of H2O in a calorimeter with a water equivalent of 25 g. Th...