The reaction is spontaneous under standard conditions.
The values of ΔH
and ΔS for the
reaction at 298K are ΔH=
-196 kJ and ΔS
= -188 JK-1. State and explain what will happen to the spontaneity
of the reaction is the temperature of the reaction is increased.
As the entropy term is negative, the second part of the Gibbs
free energy relationship, (-TΔS), becomes positive. The
higher the temperature the more positive the term. Hence, a
temperature will be reached at which the magnitude of the second
term is larger than that of the enthalpy term. At this temperature
the reaction becomes non-spontaneous.