Question #1445a

Feb 10, 2016

Gibbs' Free Energy Change is given by $\Delta$G =$\Delta$H - T$\Delta$S where $\Delta$H is the change in Enthalpy associated with the reaction ,T is the temperature at which given reaction takes place and $\Delta$S is the change in Entropy for the given reaction.
If the value of $\Delta$G is negative,the reaction is said to be spontaneous ,if it is positive,the reaction is said to be non-spontaneous.
For the given reaction of conversion of liquid form water to solid form ice,the value of $\Delta$S would be negative and thus -T$\Delta$S would be positive.For the spontaneity of the reaction,the enthalpy change $\Delta$H must be negative and its magnitude would be greater than magnitude of T$\Delta$S.